Physical Chemistry - The Solid State 📖

SHORT QUESTION ANSWER (2 MARKS) - 200 Questions

JIPMAT 2026 Online Form Started: Apply Now |10 May 2026

 

JIPMAT 2026 Online Form Started: Apply Now for 5-Year IPM at IIM Jammu & IIM Bodh Gaya – Last Date 10 May 2026, Eligibility & Step-by-Step Guide

The wait is finally over for management aspirants! The National Testing Agency (NTA) has officially commenced the registration process for the Joint Integrated Programme in Management Admission Test (JIPMAT) 2026. This national-level entrance examination serves as the exclusive gateway for admission to the prestigious 5-Year Integrated Programme in Management (IPM) offered by IIM Jammu and IIM Bodh Gaya.

The JIPMAT 2026 online form was made available on 16 April 2026, marking the beginning of a crucial journey for Class 12th students who dream of securing a seat in the Indian Institutes of Management (IIMs) right after school. Studying at an IIM is a hallmark of excellence, and the IPM curriculum is uniquely designed to blend undergraduate and postgraduate management studies into a seamless five-year journey.

Prospective candidates must act quickly, as the JIPMAT last date 10 May 2026 (11:50 PM) is approaching fast. The JIPMAT exam date 7 June 2026 has been confirmed, giving students a clear timeline for their preparation. If you aspire to lead the corporate world of tomorrow, this is your golden opportunity to join the IIM fraternity. Candidates are urged to visit the official portal at exams.nta.nic.in/jipmat to complete their JIPMAT 2026 apply online process immediately.

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JIPMAT 2026 Important Dates

To stay ahead of the competition, it is vital to keep track of the official schedule. Below is the detailed timeline for NTA JIPMAT online form 2026:

Event	Date
JIPMAT 2026 Registration Start Date	16 April 2026
JIPMAT Last Date 10 May 2026 (11:50 PM)	10 May 2026
Last Date for Online Fee Payment	11 May 2026 (11:50 PM)
JIPMAT Correction Window	12 May to 14 May 2026
Admit Card Release	Last Week of May 2026
JIPMAT Exam Date 7 June 2026	07 June 2026 (Sunday)
Answer Key & Result Declaration	To be notified soon

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Participating Institutes & Courses Offered

The JIPMAT admission form 2026 is specifically for the 5-Year Integrated Programme in Management (IPM). Unlike the traditional path of doing an MBA after graduation, the IPM allows students to enter the management fold directly after Class 12.

1. IIM Jammu: Known for its global outlook and rigorous academic framework.

2. IIM Bodh Gaya: Known as the "Enlightening IIM," it offers a world-class environment for nurturing future business leaders.

The programme grants a combined Bachelor’s and Master’s degree (BBA+MBA) upon successful completion of the five-year duration.

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JIPMAT Eligibility Criteria 2026

Before you proceed with the JIPMAT IIM Jammu Bodh Gaya IPM admission 2026, ensure you meet the following JIPMAT eligibility criteria 2026:

Educational Qualification

• Standard XII/HSC: Candidates should have passed the Standard XII/HSC or equivalent examination in 2024, 2025, or appearing in 2026.

• Minimum Marks: At least 60% marks in Standard X/SSC and Standard XII/HSC or equivalent examinations (55% for SC/ST/PwD candidates).

• Calculation: The percentage of marks obtained by the candidate in Class 10 and Class 12 shall be calculated based on the Board’s aggregate marks of all subjects that appear in the mark sheet.

Age Limit

• There is no age limit for JIPMAT 2026 as per the latest NTA guidelines; however, individual IIMs may have specific criteria. Generally, candidates should not be more than 20 years of age as of 1 August 2026. (Please refer to the JIPMAT 2026 notification PDF for specific category relaxations).

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JIPMAT Application Fee 2026

The JIPMAT application fee 2026 must be paid through online modes (Net Banking, Credit Card, Debit Card, or UPI).

Category	Application Fee
General / OBC (NCL) / EWS	₹2,200
SC / ST / PwD / Transgender	₹1,100

Note: Processing charges and GST as applicable are to be paid by the candidate.

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How to Apply JIPMAT 2026: Step-by-Step Guide

Applying for a national-level exam can be daunting. Follow these steps for a hassle-free JIPMAT 2026 apply online experience:

1. Registration: Visit the official website exams.nta.nic.in/jipmat. Click on the 'New Registration' link. Register using a valid email ID and mobile number to receive your Application Number.

2. Fill Application Form: Complete the JIPMAT online form 2026 by entering personal details, educational qualifications, and choosing your preferred exam cities.

3. Upload Documents: Upload scanned images of:

   • Recent Photograph (Color or BW with 80% face visible).

   • Candidate’s Signature.

   • Category Certificate (if applicable).

   • 10th and 12th Marksheets (as per size specifications).

4. Fee Payment: Pay the JIPMAT application fee 2026 using the integrated payment gateway.

5. Final Submission: Preview your form to ensure all details are correct. Submit and download the Confirmation Page.

Pro Tip: Keep at least 3-4 printouts of the confirmation page for future reference during the counseling process.

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JIPMAT Exam Pattern & Syllabus Overview

Understanding the exam structure is vital for success in NTA JIPMAT 2026.

• Mode of Exam: Computer Based Test (CBT).

• Duration: 150 Minutes (2.5 Hours).

• Medium: English only.

• Marking Scheme: +4 for each correct answer and -1 for each incorrect answer.

Subject Distribution

Section	Number of Questions	Marks
Quantitative Aptitude	33	132
Data Interpretation & Logical Reasoning	33	132
Verbal Ability & Reading Comprehension	34	136
Total	100	400

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Important Links Section

• Official Website: exams.nta.nic.in/jipmat

• JIPMAT 2026 Notification PDF: Download Information Bulletin (Placeholder)

• Direct Apply Online Link: Register Here

• JIPMAT Syllabus PDF: Download Syllabus (Placeholder)

• Previous Year Question Papers: View Papers (Placeholder)

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Frequently Asked Questions (FAQs)

Q1. What is the last date for JIPMAT 2026 application?

The last date to submit the JIPMAT 2026 online form is 10 May 2026 (until 11:50 PM).

Q2. What is the eligibility for JIPMAT IPM admission?

Candidates must have passed Class 12 with at least 60% marks (55% for SC/ST/PwD). They must have passed Class 12 in 2024, 2025, or be appearing in 2026.

Q3. How much is the JIPMAT application fee?

The fee is ₹2,200 for General/OBC/EWS candidates and ₹1,100 for SC/ST/PwD/Transgender candidates.

Q4. When is the JIPMAT 2026 exam date?

The NTA will conduct the JIPMAT 2026 exam on 7 June 2026.

Q5. How to apply online for JIPMAT 2026?

You can apply online by visiting exams.nta.nic.in/jipmat, registering your profile, filling in details, uploading documents, and paying the fee.

Q6. Which IIMs accept JIPMAT score?

Currently, IIM Jammu and IIM Bodh Gaya accept JIPMAT scores for their 5-Year Integrated Programme in Management (IPM).

Q7. Is there any age limit for JIPMAT?

Candidates should generally be born on or after August 01, 2006 (Maximum 20 years). Please check the notification for specific category relaxations.

Q8. When will JIPMAT 2026 result be declared?

While the exact date is not fixed, results are typically declared within 3-4 weeks after the exam date of 7 June 2026.

BCECE 2026 Online Form: Apply Now | APNA CAREER

BCECE 2026 Online Form: Apply Now for Bihar Engineering, Medical & Agriculture Admission

MP Board 10th & 12th Result 2026 | आज 11 बजे जारी | result

 

MP Board 10th & 12th Result 2026 आज 11 बजे जारी – MPBSE High School & Intermediate Result Live Updates, Roll Number से चेक करें

नमस्ते छात्रों! इंतज़ार की घड़ियाँ खत्म हुईं। Madhya Pradesh Board of Secondary Education (MPBSE) आज यानी 11 April 2026 को सुबह 11 बजे कक्षा 10वीं और 12वीं का वार्षिक परीक्षा परिणाम घोषित करने जा रहा है। अगर आप भी इस साल MP Board Exams में शामिल हुए थे, तो यह खबर आपके लिए सबसे महत्वपूर्ण है।

लाखों छात्र-छात्राएं बेसब्री से MP Board 10th & 12th Result 2026 का इंतजार कर रहे थे। शिक्षा मंत्री और बोर्ड अधिकारियों की मौजूदगी में प्रेस कॉन्फ्रेंस के जरिए रिजल्ट की घोषणा की जाएगी। पिछले साल के मुकाबले इस बार बोर्ड ने कॉपियों की चेकिंग प्रक्रिया को काफी तेज रखा था, जिसके कारण रिजल्ट समय से पहले जारी किया जा रहा है। आप अपना स्कोरकार्ड आधिकारिक वेबसाइट mpbse.nic.in और mpresults.nic.in पर जाकर तुरंत चेक कर पाएंगे।

इस आर्टिकल में हम आपको MP Board result live updates, Direct Links, और Step-by-step process बताएंगे ताकि आप बिना किसी सर्वर एरर के अपना रिजल्ट सबसे पहले देख सकें।

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MP Board Result 2026: मुख्य विवरण (Quick Overview)

नीचे दी गई टेबल में आप आज के रिजल्ट से जुड़ी सभी महत्वपूर्ण जानकारी देख सकते हैं:

विवरण (Details)	जानकारी (Information)
बोर्ड का नाम	Madhya Pradesh Board of Secondary Education (MPBSE)
परीक्षा का नाम	MP Board High School (10th) & Intermediate (12th) Exam 2026
रिजल्ट की तारीख	11 April 2026
रिजल्ट का समय	सुबह 11:00 बजे (11 AM)
चेक करने का माध्यम	Online (Roll Number & Application Number)
आधिकारिक वेबसाइट	mpbse.nic.in
रिजल्ट स्टेटस	आज जारी होगा (Live Soon)

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MP Board 10th 12th Result 2026 कैसे चेक करें? (Step-by-Step Guide)

रिजल्ट जारी होते ही वेबसाइट पर भारी ट्रैफिक की वजह से सर्वर स्लो हो सकता है। इसलिए, अपना MP Board result today 11 AM चेक करने के लिए इन स्टेप्स को फॉलो करें:

1. Step 1: सबसे पहले MP Board की आधिकारिक वेबसाइट mpresults.nic.in या mpbse.nic.in पर जाएं।

2. Step 2: होमपेज पर आपको दो लिंक दिखाई देंगे: "MPBSE - HSC (Class 10th) Examination Results - 2026" या "MPBSE - HSSC (Class 12th) Examination Results - 2026"। अपनी कक्षा के अनुसार लिंक पर क्लिक करें।

3. Step 3: अब एक नया लॉगिन पेज खुलेगा। यहाँ अपना 9-digit Roll Number और 8-digit Application Number दर्ज करें। (यह जानकारी आपके एडमिट कार्ड पर उपलब्ध होगी)।

4. Step 4: 'Submit' बटन पर क्लिक करें।

5. Step 5: आपका MP Board 10th 12th marksheet स्क्रीन पर दिखाई देगा।

6. Step 6: अपने मार्क्स चेक करें और भविष्य के लिए इसका प्रिंटआउट या PDF Download कर लें।

[Placeholder for Screenshot: MP Board Result Login Window with Roll Number Fields]

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MP Board Passing Marks & Grading System 2026

MP Board में पास होने के लिए छात्रों को कुछ न्यूनतम मापदंड पूरे करने होते हैं। MPBSE High School & Intermediate Result में पास होने के नियम निम्नलिखित हैं:

• Minimum Passing Marks: प्रत्येक विषय (Subject) में पास होने के लिए आपको कम से कम 33% अंक प्राप्त करने होंगे।

• Practical Exams: थ्योरी के साथ-साथ प्रैक्टिकल परीक्षाओं में भी अलग से पास होना अनिवार्य है।

• Grace Marks: यदि कोई छात्र एक या दो विषयों में कुछ ही अंकों से फेल हो रहा है, तो बोर्ड के नियमों के अनुसार उसे Grace Marks देकर पास किया जा सकता है।

MP Board Grading Table:

• A+ Grade: 90% से 100% (Outstanding)

• A Grade: 80% से 89% (Very Good)

• B Grade: 70% से 79% (Good)

• C Grade: 60% से 69% (Average)

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Toppers List & Overall Pass Percentage (Live Updates)

जैसे ही 11 बजे रिजल्ट घोषित होगा, MPBSE द्वारा Toppers List 2026 भी जारी की जाएगी। यहाँ हम टॉपर्स के नाम और जिले की जानकारी अपडेट करेंगे:

• Class 10th Topper: (रिजल्ट के बाद अपडेट होगा)

• Class 12th Topper: (रिजल्ट के बाद अपडेट होगा)

• Overall Pass Percentage: इस बार उम्मीद जताई जा रही है कि पासिंग प्रतिशत पिछले साल से बेहतर रहेगा।

नोट: रिजल्ट के तुरंत बाद हम यहाँ टॉपर्स की जिलेवार लिस्ट अपलोड करेंगे। कृपया इस पेज को Refresh करते रहें।

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Revaluation और Supplementary Exam की जानकारी

अगर कोई छात्र अपने अंकों से संतुष्ट नहीं है या किसी विषय में फेल हो जाता है, तो MP Board उसे दूसरा मौका देता है:

1. Revaluation / Scrutiny: अगर आपको लगता है कि आपके नंबर कम आए हैं, तो आप Re-checking के लिए आवेदन कर सकते हैं। इसकी प्रक्रिया रिजल्ट के 10-15 दिन बाद शुरू होती है।

2. Supplementary Exam: जो छात्र एक या दो विषयों में फेल हो जाते हैं, वे MP Board Supplementary Exam 2026 दे सकते हैं। यह परीक्षाएं आमतौर पर जून या जुलाई के महीने में आयोजित की जाती हैं।

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Important Links for MP Board Result 2026

अपना रिजल्ट और मार्कशीट डाउनलोड करने के लिए नीचे दिए गए सीधे लिंक का उपयोग करें:

• Official Result Portal: mpresults.nic.in

• MPBSE Official Website: mpbse.nic.in

• MP Board 10th Result 2026 Direct Link: [यहाँ क्लिक करें - Link Active at 11 AM]

• MP Board 12th Result 2026 Direct Link: [यहाँ क्लिक करें - Link Active at 11 AM]

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FAQ: MP Board Result 2026 से जुड़े अक्सर पूछे जाने वाले सवाल

Q1. MP Board 10th 12th result 2026 कितने बजे आएगा?

उत्तर: रिजल्ट आज 11 अप्रैल 2026 को सुबह 11:00 बजे जारी किया जाएगा।

Q2. रिजल्ट चेक करने के लिए किन चीजों की जरूरत होगी?

उत्तर: आपको अपना Roll Number और Application Number तैयार रखना होगा।

Q3. क्या मैं बिना इंटरनेट के रिजल्ट देख सकता हूँ?

उत्तर: हाँ, आप SMS के जरिए भी रिजल्ट देख सकते हैं। 'MPBSE10 (Space) Roll Number' लिखकर 56263 पर भेजें।

Q4. MP Board की आधिकारिक वेबसाइट क्या है?

उत्तर: आधिकारिक वेबसाइट mpbse.nic.in और mpresults.nic.in है।

Q5. अगर मैं अपना Roll Number भूल गया हूँ तो क्या करूँ?

उत्तर: आप अपने स्कूल से संपर्क कर सकते हैं या अपने एडमिट कार्ड की फोटोकॉपी चेक करें।

Q6. क्या ओरिजिनल Marksheet आज ही मिल जाएगी?

उत्तर: नहीं, आज सिर्फ ऑनलाइन स्कोरकार्ड मिलेगा। ओरिजिनल मार्कशीट आपको कुछ दिनों बाद आपके स्कूल से प्राप्त होगी।

Q7. अगर वेबसाइट ओपन नहीं हो रही तो क्या करें?

उत्तर: घबराएं नहीं, भारी ट्रैफिक के कारण ऐसा होता है। 10-15 मिनट बाद दोबारा प्रयास करें या हमारी वेबसाइट पर दिए गए अल्टरनेटिव लिंक्स का उपयोग करें।

Q8. Supplementary परीक्षा के फॉर्म कब भरे जाएंगे?

उत्तर: आमतौर पर रिजल्ट घोषित होने के 2 सप्ताह के भीतर आवेदन शुरू हो जाते हैं।

Q9. क्या 10वीं और 12वीं का रिजल्ट एक साथ आएगा?

उत्तर: हाँ, MP Board अक्सर हाई स्कूल और इंटरमीडिएट दोनों का रिजल्ट एक ही दिन और एक ही समय पर जारी करता है।

Q10. फेल होने पर क्या साल खराब हो जाएगा?

उत्तर: नहीं, आप Supplementary परीक्षा देकर अपना साल बचा सकते हैं।

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आज सुबह 11 बजे का समय मध्य प्रदेश के लाखों छात्रों के लिए निर्णायक होने वाला है। हमारी पूरी टीम की ओर से आपको भविष्य के लिए बहुत-बहुत शुभकामनाएँ! यदि आपके अच्छे अंक आते हैं, तो यह आपकी कड़ी मेहनत का फल है। और यदि परिणाम आपकी उम्मीद के मुताबिक न रहे, तो निराश न हों; जीवन में सुधार के कई मौके मिलते हैं।

अपना MP Board 10th 12th marksheet download करने के बाद उसका प्रिंट सुरक्षित जरूर रख लें। रिजल्ट से जुड़ी किसी भी समस्या के लिए नीचे कमेंट बॉक्स में अपना सवाल पूछें।

Unit 1: Solutions

 Unit 1: Solutions 

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Section 1: Types of Solutions & Concentration Terms

1. Which of the following concentration units is independent of temperature? A) Molarity B) Normality C) Molality D) Formality

2. An example of a solid solution (solid in solid) is: A) Salt in water B) Brass (Alloy) C) Camphor in nitrogen D) Aerated drinks

3. The number of moles of solute dissolved in 1 kg of solvent is called: A) Molarity B) Molality C) Mole fraction D) Normality

4. Which of the following is a 'Liquid in Solid' type solution? A) Fog B) Smoke C) Amalgam of mercury with sodium D) Dissolved oxygen in water

5. The sum of the mole fractions of all components in a solution is always: A) 0 B) 1 C) 100 D) Varies with temperature

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Section 2: Solubility of Gases in Liquids (Henry's Law)

6. According to Henry's Law, the solubility of a gas in a liquid is directly proportional to: A) The volume of the liquid B) The partial pressure of the gas C) The density of the gas D) The molecular mass of the gas

7. With an increase in temperature, the solubility of gases in liquids generally: A) Increases B) Decreases C) Remains constant D) First increases then decreases

8. Scuba divers use tanks diluted with Helium to avoid a painful condition called: A) Anoxia B) Bends C) Hyperoxia D) Nitrogen narcosis

9. The Henry’s Law constant (KH) value: A) Is the same for all gases B) Increases with an increase in temperature C) Decreases with an increase in temperature D) Is independent of the nature of the gas

10. Low blood oxygen levels in climbers at high altitudes (Anoxia) is caused by: A) High atmospheric pressure B) Low partial pressure of oxygen C) Low temperature D) High humidity

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Section 3: Raoult's Law & Ideal Solutions

11. Raoult's Law states that for a solution of volatile liquids, the partial vapor pressure of each component is proportional to its: A) Molarity B) Molality C) Mole fraction D) Weight percentage

12. For an ideal solution, which of the following is TRUE? A) ΔH_mixing > 0 B) ΔV_mixing < 0 C) ΔH_mixing = 0 and ΔV_mixing = 0 D) It obeys Henry’s law only

13. A mixture of Ethanol and Acetone shows: A) Positive deviation from Raoult's Law B) Negative deviation from Raoult's Law C) Ideal behavior D) No vapor pressure

14. A mixture of Chloroform and Acetone shows negative deviation because: A) Heat is absorbed B) Intermolecular H-bonding is formed between components C) Molecules repel each other D) Volume increases upon mixing

15. Constant boiling mixtures that distill without change in composition are called: A) Ideal solutions B) Azeotropes C) Isotonic solutions D) Saturated solutions

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Section 4: Colligative Properties

16. Colligative properties depend only on: A) Nature of the solute B) Nature of the solvent C) Number of solute particles D) Chemical properties of the solute

17. The relative lowering of vapor pressure is equal to: A) Molarity of solute B) Mole fraction of solute C) Molality of solute D) Mole fraction of solvent

18. The unit of Molal Elevation Constant (Kb) is: A) K kg mol B) K kg mol⁻¹ C) mol kg⁻¹ K⁻¹ D) K mol kg⁻¹

19. The process of movement of solvent molecules through a semi-permeable membrane is: A) Diffusion B) Osmosis C) Effusion D) Sedimentation

20. Isotonic solutions have the same: A) Boiling point B) Freezing point C) Osmotic pressure D) Vapor pressure

21. Which property is best used to determine the molecular mass of polymers and proteins? A) Elevation of boiling point B) Depression of freezing point C) Osmotic pressure D) Relative lowering of vapor pressure

22. The freezing point of a solution is ______ than that of the pure solvent. A) Higher B) Lower C) Equal D) Twice

23. Adding salt to ice helps in clearing snowy roads because it: A) Increases the melting point B) Lowers the freezing point of water C) Acts as a catalyst for melting D) Increases the vapor pressure

24. Reverse Osmosis (RO) occurs when the applied pressure is: A) Equal to osmotic pressure B) Less than osmotic pressure C) Greater than osmotic pressure D) Zero

25. The osmotic pressure (π) of a solution is given by the equation: A) π = MRT B) π = CRT (where C is molarity) C) π = nRT D) π = Kb × m

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Section 5: Van't Hoff Factor & Abnormal Molecular Mass

26. The Van't Hoff factor (i) for a non-electrolyte (like glucose) is: A) 0 B) 1 C) 2 D) 0.5

27. If a solute undergoes dissociation in a solution, the value of 'i' will be: A) i < 1 B) i > 1 C) i = 1 D) i = 0

28. The Van't Hoff factor (i) for BaCl₂ (assuming 100% dissociation) is: A) 1 B) 2 C) 3 D) 4

29. When acetic acid dimerizes in benzene, its Van't Hoff factor (i) is: A) More than 1 B) Less than 1 C) Equal to 1 D) Equal to 2

30. Abnormal molar mass is observed when: A) The solution is ideal B) Solute undergoes association or dissociation C) The solution is very dilute D) The solute is non-volatile

31. The correct relationship for 'i' is: A) i = Normal Molar Mass / Observed Molar Mass B) i = Observed Molar Mass / Normal Molar Mass C) i = Calculated Colligative Property / Observed Colligative Property D) i = Moles before dissociation / Moles after dissociation

32. Which of the following will have the highest boiling point? A) 0.1 M Glucose B) 0.1 M NaCl C) 0.1 M Na₂SO₄ D) 0.1 M Urea

33. Which of the following 0.1 M aqueous solutions will have the lowest freezing point? A) Al₂(SO₄)₃ B) NaCl C) KCl D) Glucose

34. If i = 1 + α(n-1), what does 'α' represent? A) Mole fraction B) Degree of dissociation C) Molality D) Osmotic constant

35. The Van't Hoff factor for K₄[Fe(CN)₆] (complete dissociation) is: A) 4 B) 5 C) 6 D) 1

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Section 6: General Concepts & Calculations

36. Ebullioscopic constant is another name for: A) Cryoscopic constant B) Molal elevation constant C) Henry’s constant D) Gas constant

37. A plant cell shrinks when placed in a hypertonic solution due to: A) Endosmosis B) Exosmosis C) Diffusion D) Absorption

38. The vapor pressure of a pure solvent is ______ than the vapor pressure of its solution. A) Higher B) Lower C) Same D) Half

39. Cryoscopic constant (Kf) depends upon: A) Nature of solute B) Nature of solvent C) Pressure D) Concentration

40. For a non-volatile solute, which property is directly proportional to its molality? A) Relative lowering of vapor pressure B) Elevation of boiling point C) Osmotic pressure D) All of the above

41. 0.91% (w/v) NaCl solution is ______ with human blood. A) Hypertonic B) Hypotonic C) Isotonic D) Saturated

42. Maximum boiling azeotropes are formed by solutions showing: A) Positive deviation B) Negative deviation C) Ideal behavior D) No deviation

43. Semi-permeable membranes allow the passage of: A) Solute particles only B) Solvent molecules only C) Both solute and solvent D) Neither solute nor solvent

44. Which of the following is not a colligative property? A) Osmotic pressure B) Surface tension C) Depression in freezing point D) Relative lowering in vapor pressure

45. Parts per million (ppm) is used to express the concentration of: A) Concentrated acids B) Trace pollutants in water C) Solid alloys D) Saturated sugar solution

46. What is the molality of pure water? A) 18 B) 55.5 C) 100 D) 1

47. Camphor in Nitrogen gas is an example of: A) Gas in Liquid B) Solid in Gas C) Liquid in Gas D) Solid in Solid

48. Raoult's Law becomes a special case of Henry's Law when: A) KH = P° B) KH = 1 C) P° = 0 D) Molality is 1

49. Which of the following shows a decrease in volume on mixing? A) Ethanol + Water B) Chloroform + Acetone C) Benzene + Toluene D) n-Hexane + n-Heptane

50. The molar mass determined by colligative properties is 'abnormal' when the solute: A) Is non-volatile B) Associates or dissociates in the solvent C) Does not dissolve completely D) Is in the gaseous state

Unit 1: Solutions - NEET Level MCQs

I. Concentration Terms & Solubility

1. The molarity of a solution obtained by mixing 750 mL of 0.5 M HCl with 250 mL of 2 M HCl is: A) 0.875 M B) 1.0 M C) 1.75 M D) 0.975 M
2. What is the molality of a 15% (w/w) solution of $H_{2}S{O}_4$ (Molecular mass = 98)? A) 1.2 mol/kg B) 1.8 mol/kg C) 1.5 mol/kg D) 2.1 mol/kg
3. Density of a 2.03 M cane sugar solution is 1.063 g/mL. Its molality is: A) 2.97 m B) 3.12 m C) 2.03 m D) 2.51 m
4. The value of Henry's constant $K_H$ is: A) Greater for gases with higher solubility. B) Greater for gases with lower solubility. C) Constant for all gases. D) Not related to the nature of the gas.
5. Which of the following units is used for reporting the concentration of trace pollutants in water? A) Molarity B) Molality C) ppm D) Mole fraction

II. Raoult's Law & Ideal/Non-Ideal Solutions

1. For an ideal solution, the correct condition is: A) $\Delta H_{mix}=0,\Delta V_{mix}=0,\Delta S_{mix}=0$ B) $\Delta H_{mix}=0,\Delta V_{mix}=0,\Delta G_{mix}<0$ C) $\Delta H_{mix}>0,\Delta V_{mix}>0$ D) $\Delta H_{mix}<0,\Delta V_{mix}<0$
2. A mixture of $CHC{l}_3$ and $C{H}_{3}COC{H}_3$ (acetone) shows negative deviation from Raoult's law because: A) $A-A$ and $B-B$ interactions are stronger than $A-B$. B) $A-B$ interaction is stronger than $A-A$ and $B-B$ due to H-bonding. C) It forms a minimum boiling azeotrope. D) The molecules are identical in size.
3. Which of the following liquid pairs shows a positive deviation from Raoult's law? A) Water + Nitric acid B) Benzene + Methanol C) Water + HCl D) Acetone + Chloroform
4. Maximum boiling azeotropes are formed by: A) Ideal solutions B) Solutions with positive deviation C) Solutions with negative deviation D) Non-volatile solutes
5. At a given temperature, the total vapor pressure of a solution containing components A and B is $P=120-75x_B$. The vapor pressure of pure A ($P_A^o$) is: A) 120 B) 75 C) 45 D) 195

III. Colligative Properties (VP, BP, FP)

1. Relative lowering of vapor pressure is a colligative property because: A) It depends on the concentration of a non-electrolyte solute. B) It depends on the number of particles of solute. C) It is the ratio of vapor pressure of solution to solvent. D) It depends on the nature of the solute.
2. The vapor pressure of water at $20^{o}C$ is 17.5 mm Hg. When 18 g of glucose is added to 178.2 g of water at $20^{o}C$, the vapor pressure of the solution will be: A) 17.675 mm Hg B) 17.325 mm Hg C) 15.5 mm Hg D) 17.0 mm Hg
3. Which solution will have the highest boiling point? A) 1% Glucose in water B) 1% $NaCl$ in water C) 1% $CaC{l}_2$ in water D) 1% Sucrose in water
4. The molal elevation constant ($K_b$) depends on: A) Nature of solute B) Nature of solvent C) Enthalpy of solution D) Molarity
5. If the elevation in boiling point of a solution of non-volatile, non-electrolyte solute in solvent is $0.8^{o}C$, then the depression in freezing point of the same solution would be ($K_b=0.52,K_f=1.86$): A) $2.86^{o}C$ B) $1.86^{o}C$ C) $0.8^{o}C$ D) $0.52^{o}C$
6. Why is the molecular mass of a polymer determined by osmotic pressure rather than other colligative properties? A) Change in freezing point is too large to measure. B) Osmotic pressure is large enough to be measured at room temperature. C) Polymers are insoluble at high temperatures. D) Polymers dissociate at high temperatures.
7. A $5\%$ solution of cane sugar (MW = 342) is isotonic with $0.877\%$ solution of urea. The molecular weight of urea is: A) 60 B) 30 C) 90 D) 120
8. The osmotic pressure of a solution can be increased by: A) Increasing volume B) Increasing temperature C) Decreasing solute amount D) Increasing solvent amount
9. Blood cells retain their normal shape in solution which are: A) Hypotonic to blood B) Isotonic to blood C) Hypertonic to blood D) Equimolar to blood
10. Which of the following $0.10$ M aqueous solutions will exhibit the largest freezing point depression? A) $KCl$ B) $C_6{H}_{12}{O}_6$ C) $A{l}_2(S{O}_4{)}_3$ D) $K_{2}S{O}_4$

IV. Van't Hoff Factor & Abnormal Molar Mass

1. The Van't Hoff factor ($i$) for a dilute solution of $K_4[Fe(CN{)}_6]$ is: A) 4 B) 5 C) 3 D) 2
2. If '$\alpha$' is the degree of dissociation of $N{a}_{2}S{O}_4$, the Van't Hoff factor ($i$) used for calculating molecular mass is: A) $1+\alpha$ B) $1-\alpha$ C) $1+2\alpha$ D) $1-2\alpha$
3. The Van't Hoff factor ($i$) for a compound which undergoes dimerization in benzene is: A) 0.5 B) 1.5 C) 2 D) 1
4. Which of the following has $i=1$? A) $NaCl$ B) Urea C) $CaC{l}_2$ D) $C{H}_{3}COOH$ in water
5. The ratio of the colligative property of $BaC{l}_2$ solution to that of sucrose solution of same molar concentration is: A) 1 B) 2 C) 3 D) 0.5
6. For which of the following solutes is the observed molar mass less than the theoretical molar mass? A) Glucose B) $KCl$ C) Benzoic acid in benzene D) Sucrose
7. A $0.004$ M solution of $N{a}_{2}S{O}_4$ is isotonic with a $0.010$ M solution of glucose. The degree of dissociation of $N{a}_{2}S{O}_4$ is: A) $75\%$ B) $85\%$ C) $50\%$ D) $25\%$
8. The Van't Hoff factor ($i$) for a $0.1$ M $A{l}_2(S{O}_4{)}_3$ solution is $4.20$. The degree of dissociation is: A) $80\%$ B) $90\%$ C) $70\%$ D) $100\%$
9. Which property is used to calculate the degree of association or dissociation? A) Surface tension B) Viscosity C) Van't Hoff factor D) Refractive index
10. In the case of association, the observed colligative property is: A) Higher than calculated B) Lower than calculated C) Same as calculated D) Zero

V. Advanced Conceptual & Numerical Mix

1. $12$ g of a non-volatile solute dissolved in $108$ g of water produces a relative lowering of vapor pressure of $0.1$. The molecular mass of the solute is: A) 20 B) 40 C) 60 D) 80
2. A solution of $CaC{l}_2$ and $NaCl$ are both $0.1$ M. If the osmotic pressure of $NaCl$ is $P_1$ and that of $CaC{l}_2$ is $P_2$, then: A) $P_1=P_2$ B) $P_1>P_2$ C) $P_2>P_1$ D) $P_1=2P_2$
3. Which has the minimum freezing point? A) 1 M $NaCl$ B) 1 M $KCl$ C) 1 M $CaC{l}_2$ D) 1 M $AlC{l}_3$
4. If $K_f$ for water is $1.86$, the freezing point of $0.1$ m $NaCl$ solution (assuming $100\%$ ionization) is: A) $-1.86^{o}C$ B) $-0.372^{o}C$ C) $-0.186^{o}C$ D) $-3.72^{o}C$
5. The vapor pressure of pure benzene is $640$ mm Hg. $2.175$ g of a non-volatile solute is added to $39$ g of benzene, and the vapor pressure of the solution becomes $600$ mm Hg. The molar mass of the solute is: A) 65.25 B) 130.5 C) 45 D) 90
6. $0.1$ m solution of $Pt(N{H}_3{)}_{4}C{l}_4$ in water freezes at $-0.558^{o}C$. $K_f$ for water is $1.86$. The number of ions produced per molecule of the complex is: A) 1 B) 2 C) 3 D) 4
7. For a dilute solution, Raoult's law states that: A) The lowering of vapor pressure is equal to the mole fraction of solute. B) The relative lowering of vapor pressure is equal to the mole fraction of solute. C) The vapor pressure of solution is equal to the mole fraction of solvent. D) The vapor pressure of solution is proportional to the mole fraction of solute.
8. The unit of cryoscopic constant ($K_f$) is: A) $K$ B) $kg/mol$ C) $Kkg/mol$ D) $mol/kgK$
9. Henry's Law is NOT applicable if: A) The gas is highly soluble. B) The gas reacts chemically with the solvent. C) The pressure is very high. D) All of the above.
10. Equimolar solutions in the same solvent have: A) Different boiling points B) Same boiling points C) Same freezing points D) Both B and C (for non-electrolytes)
11. Direction of osmosis can be reversed by applying pressure: A) Lower than osmotic pressure on solution side. B) Higher than osmotic pressure on solution side. C) Equal to osmotic pressure on solvent side. D) Higher than atmospheric pressure on solvent side.
12. Azeotropic mixtures are: A) Liquid mixtures that boil at a constant temperature. B) Binary mixtures having the same composition in liquid and vapor phase. C) Also called constant boiling mixtures. D) All of the above.
13. Sea water can be converted into fresh water by: A) Osmosis B) Reverse Osmosis C) Diffusion D) Filtration
14. Which of the following is an example of a gas in solid solution? A) Solution of hydrogen in palladium B) Solution of camphor in nitrogen C) Solution of iodine in alcohol D) All of the above
15. When $Hg{I}_2$ is added to $KI$ solution, the freezing point: A) Lowers B) Increases C) Remains same D) Becomes zero
16. $0.6$ g of urea was dissolved in $9.9$ g of water. If the vapor pressure of pure water is $P^o$, the vapor pressure of solution is: A) $0.10P^o$ B) $1.10P^o$ C) $0.98P^o$ D) $0.90P^o$
17. The elevation in boiling point of $0.01$ M $BaC{l}_2$ solution is about ______ times that of $0.01$ M glucose solution. A) 1 B) 2 C) 3 D) 5
18. $X$ g of a non-electrolyte (MW = 40) is dissolved in $100$ g of water. If $\Delta T_b$ is $0.52^{o}C$ and $K_b$ for water is $0.52$, the value of $X$ is: A) 4 g B) 40 g C) 10 g D) 20 g
19. In cold countries, ethylene glycol is added to water in car radiators. This helps to: A) Reduce the boiling point B) Lower the freezing point C) Act as a fuel D) Clean the engine
20. At high altitudes, the boiling point of water decreases because: A) Atmospheric pressure is high. B) Atmospheric pressure is low. C) Temperature is low. D) Oxygen content is low.
21. JEE Level MCQs: Unit 1 - Solutions
    I. Advanced Concentration & Mixing
    1. A 1000g sample of a solution contains 0.1 moles of solute. If the density of the solution is $d$ g/mL, the molarity ($M$) and molality ($m$) are related by: A) $M=m(1000d/(1000+m\cdot MW))$ B) $m=1000M/(1000d-M\cdot MW)$ C) Both A and B D) $M=m\cdot d$
    2. Calculate the mole fraction of a solute in a 2.0 m aqueous solution. A) 0.0347 B) 0.036 C) 0.045 D) 0.018
    3. How many grams of $N{a}_{2}C{O}_3$ (MW=106) should be dissolved in 250g of water to prepare a 0.1 m solution? A) 2.65g B) 1.06g C) 5.30g D) 0.265g
    4. Which concentration term changes with temperature for a solution containing a volatile solute and a non-volatile solvent? A) Mole fraction B) Molality C) Weight percentage D) Molarity
    5. A solution of $H_{2}S{O}_4$ is 98% by weight and has a density of 1.84 g/mL. The volume of this acid required to make 1L of 0.1 M $H_{2}S{O}_4$ is: A) 10 mL B) 5.43 mL C) 18.4 mL D) 2.5 mL
    II. Solubility & Henry’s Law
    1. The Henry's law constant for $O_2$ in water is $4.34\times 10^4$ atm at 25°C. If the partial pressure of $O_2$ in air is 0.2 atm, calculate the concentration (in mole fraction) of dissolved $O_2$. A) $4.6\times 10^{-6}$ B) $2.1\times 10^{-4}$ C) $1.5\times 10^{-5}$ D) $8.6\times 10^{-5}$
    2. A gas $X$ is bubbled through water at 293 K. $K_H$ for $X$ is 100 kbar. If the gas exerts a partial pressure of 0.98 bar, how many millimoles of $X$ dissolve in 1L of water? A) 0.54 B) 0.45 C) 0.98 D) 1.2
    3. Considering Henry's law, which of the following is correct for a gas dissolving in a liquid? A) $\Delta G<0,\Delta S<0,\Delta H<0$ B) $\Delta G<0,\Delta S>0,\Delta H<0$ C) $\Delta G<0,\Delta S<0,\Delta H>0$ D) $\Delta G>0,\Delta S<0,\Delta H<0$
    III. Raoult’s Law & Binary Mixtures
    1. Two liquids A and B form an ideal solution. At 300 K, the vapor pressure of a solution containing 1 mole of A and 3 moles of B is 550 mm Hg. At the same temperature, if 1 more mole of B is added, the vapor pressure increases to 560 mm Hg. The vapor pressures of pure A and B ($P_A^o,P_B^o$) are: A) 400, 600 B) 600, 400 C) 500, 500 D) 450, 550
    2. The vapor pressure of a pure liquid A is 40 mm Hg at 310 K. The vapor pressure of this liquid in a solution with liquid B is 32 mm Hg. If the solution obeys Raoult's law, the mole fraction of B in the solution is: A) 0.8 B) 0.2 C) 0.4 D) 0.5
    3. For a non-ideal solution showing positive deviation from Raoult's law: A) $P_{total}>P_A^o{X}_A+P_B^o{X}_B$ B) $\Delta V_{mix}>0$ C) $\Delta H_{mix}>0$ D) All of the above
    4. In a binary solution of A and B, if $A-B$ interactions are weaker than $A-A$ and $B-B$ interactions, then: A) The solution will show negative deviation. B) The boiling point will be higher than expected. C) The vapor pressure will be higher than predicted by Raoult's law. D) Mixing will be exothermic.
    5. Benzene and Toluene form an ideal solution. The vapor pressure of pure benzene is 100 torr and pure toluene is 40 torr. In a solution where the mole fraction of benzene is 0.5, the mole fraction of benzene in the vapor phase ($Y_{benzene}$) is: A) 0.50 B) 0.71 C) 0.29 D) 0.60
    IV. Azeotropes & Non-Ideal Behavior
    1. A mixture of two liquids A and B has a boiling point higher than the boiling points of both A and B. This mixture is: A) An ideal solution. B) A minimum boiling azeotrope. C) A maximum boiling azeotrope. D) A solution showing positive deviation.
    2. Which of the following forms a maximum boiling azeotrope? A) $H_{2}O+C_2{H}_{5}OH$ B) $C_6{H}_6+C_6{H}_{5}C{H}_3$ C) $HCl+H_{2}O$ D) $C_2{H}_{5}Br+C_2{H}_{5}I$
    3. At a specific composition, a solution of $HN{O}_3$ and $H_{2}O$ behaves like a pure liquid. This implies: A) It is an ideal solution. B) The vapor has the same composition as the liquid. C) It can be separated by simple distillation. D) $\Delta H_{mix}=0$.
    V. Colligative Properties & Van't Hoff Factor
    1. The Van't Hoff factor for a $0.1$ M $Ba(N{O}_3{)}_2$ solution is 2.74. The degree of dissociation ($\alpha$) is: A) 87% B) 74% C) 91% D) 100%
    2. Which of the following aqueous solutions will have the highest boiling point? A) 0.1 M $N{a}_{2}S{O}_4$ B) 0.1 M $K_4[Fe(CN{)}_6]$ C) 0.1 M $A{l}_2(S{O}_4{)}_3$ D) 0.1 M $NaCl$
    3. If the elevation in boiling point of a solution of a non-volatile solute in a solvent ($K_b=0.52$) is $0.156^{o}C$, then the depression in freezing point of the same solution ($K_f=1.86$) will be: A) $0.558^{o}C$ B) $0.156^{o}C$ C) $1.86^{o}C$ D) $0.052^{o}C$
    4. The osmotic pressure of a decinormal ($0.1$ N) solution of $BaC{l}_2$ at 27°C is (assume $i=2.5$): A) 3.08 atm B) 6.15 atm C) 1.23 atm D) 4.56 atm
    5. $1.0$ g of a non-electrolyte solute (MW = 250) was dissolved in $51.2$ g of benzene. If $K_f$ for benzene is $5.12$ K kg/mol, the freezing point depression ($\Delta T_f$) is: A) 0.2 K B) 0.4 K C) 0.5 K D) 0.8 K
    6. What is the freezing point of a solution containing $0.5$ g $KCl$ in $100$ g water ($K_f=1.86$)? Assume $KCl$ is 100% ionized. A) $-0.25^{o}C$ B) $-0.124^{o}C$ C) $-0.248^{o}C$ D) $-0.496^{o}C$
    7. The molar mass of a solute determined by measuring the elevation of boiling point is found to be double the actual molar mass. This indicates the solute has: A) Dissociated into two particles. B) Associated into a dimer. C) Remained unchanged. D) Reacted with the solvent.
    8. For a $1$ m aqueous solution of the following compounds, which one will show the maximum freezing point depression? A) $[Co(N{H}_3{)}_6]C{l}_3$ B) $[Co(N{H}_3{)}_{5}Cl]C{l}_2$ C) $[Co(N{H}_3{)}_{4}C{l}_2]Cl$ D) $[Co(N{H}_3{)}_{3}C{l}_3]$
    9. The relative lowering of vapor pressure of a dilute aqueous solution of glucose is 0.018. The molality of the solution is: A) 1.01 m B) 1.0 m C) 0.18 m D) 0.018 m
    10. Calculate the osmotic pressure of a solution obtained by mixing 100 mL of 0.1 M $CaC{l}_2$ and 100 mL of 0.1 M $N{a}_{2}S{O}_4$ at 300 K (assume complete dissociation and no precipitation). A) 7.38 atm B) 4.92 atm C) 3.69 atm D) 12.3 atm
    11. A certain non-volatile solute associates in benzene. If the degree of association is 0.8 and it forms tetramers, the Van't Hoff factor $i$ is: A) 0.2 B) 0.4 C) 0.6 D) 0.8
    12. Which of the following has the lowest freezing point? A) 0.1 m $C{a}_3(P{O}_4{)}_2$ B) 0.1 m $A{l}_2(S{O}_4{)}_3$ C) 0.1 m $K_3[Fe(CN{)}_6]$ D) 0.1 m $MgS{O}_4$
    13. At 25°C, the highest osmotic pressure is exhibited by 0.1 M solution of: A) $CaC{l}_2$ B) $KCl$ C) Glucose D) Urea
    14. If $K_b$ of a solvent is $X$ K kg/mol, then the elevation in boiling point of a $0.2$ m solution of a non-electrolyte solute is: A) $0.1X$ B) $0.2X$ C) $0.5X$ D) $X$
    VI. Thermodynamic & Complex Numericals
    1. For the process of dissolving a non-volatile solute in a liquid solvent, which of the following is always TRUE? A) $\Delta H_{soln}<0$ B) $\Delta S_{soln}>0$ C) $\Delta G_{soln}<0$ D) $\Delta V_{soln}=0$
    2. A solution of two volatile liquids A and B obeys $P_{total}=100+50X_A$. The ratio of $P_A^o/P_B^o$ is: A) 1.5 B) 0.5 C) 2.0 D) 3.0
    3. The vapor pressure of water at 25°C is 24 mm Hg. If 1 mole of a non-ionic solute is dissolved in 9 moles of water, the vapor pressure of the solution is: A) 21.6 mm Hg B) 2.4 mm Hg C) 24 mm Hg D) 20 mm Hg
    4. The cryoscopic constant ($K_f$) of water is $1.86$ K kg/mol. A $0.01$ molal solution of a complex $CoC{l}_3\cdot 6N{H}_3$ freezes at $-0.0744^{o}C$. The number of chloride ions in the coordination sphere is: A) 0 B) 1 C) 2 D) 3
    5. The freezing point of a $0.08$ molal solution of $NaHS{O}_4$ is $-0.372^{o}C$. $K_f$ for water is $1.86$. The Van't Hoff factor is: A) 2.0 B) 2.5 C) 3.0 D) 1.5
    6. Two solutions, 0.1 M urea and 0.1 M sucrose, are separated by a semi-permeable membrane. Which of the following will occur? A) Water flows from urea to sucrose. B) Water flows from sucrose to urea. C) There is no net movement of water. D) Urea moves to the sucrose side.
    7. A $1.17\%$ NaCl solution is isotonic with a $7.2\%$ solution of a non-electrolyte. The molar mass of the non-electrolyte is: A) 180 B) 342 C) 60 D) 120
    8. Which of the following will have the same boiling point as 0.1 M $NaCl$ solution? A) 0.1 M $N{a}_{2}S{O}_4$ B) 0.1 M Glucose C) 0.1 M $MgC{l}_2$ D) 0.1 M $KCl$
    9. The vapor pressure of a solution of a non-volatile solute is 90% of the vapor pressure of the pure solvent. The molality of the solution is: A) 6.17 m B) 5.55 m C) 1.11 m D) 0.9 m
    10. The molal elevation constant of a solvent is the elevation in boiling point produced by dissolving: A) 1g solute in 100g solvent. B) 1 mole solute in 1L solvent. C) 1 mole solute in 1kg solvent. D) 1 mole solute in 1kg solution.
    11. Reverse osmosis is used in: A) Water purification B) Determining MW of protein C) Concentration of fruit juices D) Both A and C
    12. An ideal solution is formed when its components: A) Have the same molecular size. B) Have similar intermolecular forces. C) Show no volume change on mixing. D) All of the above.
    13. A $0.2$ M aqueous solution of a weak acid (HX) is 20% ionized. The freezing point of this solution is ($K_f=1.86$): A) $-0.45^{o}C$ B) $-0.37^{o}C$ C) $-0.53^{o}C$ D) $-0.22^{o}C$
    14. The elevation of boiling point for $13.44$ g of $CuC{l}_2$ (MW = 134.4) in 1 kg of water using $K_b=0.52$ is (assume $i=3$): A) $0.052$ B) $0.156$ C) $0.104$ D) $0.208$
    15. Which of the following statements about $K_b$ is FALSE? A) It is called the Ebullioscopic constant. B) It depends on the boiling point of the solvent. C) It is a property of the solute. D) Its units are K kg/mol.
    16. The degree of dissociation of $Ca(N{O}_3{)}_2$ in a dilute aqueous solution, containing $7$ g of the salt per $100$ g of water at 100°C, is 70%. If the vapor pressure of water at 100°C is 760 mm Hg, the vapor pressure of the solution is: A) 746 mm Hg B) 750 mm Hg C) 740 mm Hg D) 755 mm Hg
    17. $1$ mole of liquid A and $2$ moles of liquid B are mixed. The vapor pressure of the solution is found to be 300 torr. $P_A^o=400$ torr and $P_B^o=200$ torr. The solution is: A) Ideal B) Showing positive deviation C) Showing negative deviation D) Saturated
    18. Calculate the percentage of $N{a}_{2}S{O}_4$ in a mixture of $N{a}_{2}S{O}_4$ and glucose if the mixture is isotonic with $1$ M $MgC{l}_2$ (assume 100% ionization for salts). A) Insufficient data B) 50% C) 25% D) 75%
    19. In the depression of freezing point experiment, it is found that: A) The vapor pressure of the solution is less than that of pure solvent. B) Only solvent molecules solidify at the freezing point. C) Only solute molecules solidify at the freezing point. D) Both A and B.
    20. At high altitude, water boils at 95°C. To make water boil at 100°C, the amount of $NaCl$ added to 1 kg of water ($K_b=0.52$) should be approximately: A) 280g B) 140g C) 58.5g D) 100g