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Indian Navy SSR (Sailor) Solutions — practice questions

Explore 19 free Solutions questions in Indian Navy SSR (Sailor) Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Solutions questions and exercises with answers

Showing questions 1–19 of 19.

In ideal solutions, ΔH_mix is:Read the answer and worked solution →Molality of a solution does not depend on:Read the answer and worked solution →Osmotic pressure of 0.1 M Glucose at 27°C is π_g. For 0.1 M NaCl at same T, the osmotic pressure is approximately:Read the answer and worked solution →Molarity M is defined as:Read the answer and worked solution →Molality m is defined as:Read the answer and worked solution →Osmotic pressure π for dilute solution:Read the answer and worked solution →For salt CaCl₂ (assume full dissociation), i =Read the answer and worked solution →Complete the two concentration definitionsRead the answer and worked solution →Molarity or molality?Read the answer and worked solution →True or false: concentrationRead the answer and worked solution →Naming the measureRead the answer and worked solution →Complete the meaning of colligativeRead the answer and worked solution →True or false: colligative propertiesRead the answer and worked solution →Tap every statement true of molalityRead the answer and worked solution →Assertion and reasonRead the answer and worked solution →Two are true, one is notRead the answer and worked solution →Three of these are wrong. Find the one that holds.Read the answer and worked solution →Flip and pair: measure with its denominatorRead the answer and worked solution →Spot the one that does not belongRead the answer and worked solution →

Worked practice questions

In ideal solutions, ΔH_mix is:

  1. Negative
  2. Positive
  3. Zero
  4. Variable
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Correct answer: C. Zero

For ideal solutions, ΔH_mix = 0 (no enthalpy change when components mix). Real solutions often show positive (endothermic mixing) or negative (exothermic) ΔH_mix.

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Molality of a solution does not depend on:

  1. Molar mass of solute
  2. Mass of solute
  3. TEMPERATURE
  4. Mass of solvent
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Correct answer: C. TEMPERATURE

Molality = moles solute / kg solvent. Mass does not change with temperature. Volume does. So molarity changes with T, but molality does not. This is why molality is preferred for colligative property calculations.

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Osmotic pressure of 0.1 M Glucose at 27°C is π_g. For 0.1 M NaCl at same T, the osmotic pressure is approximately:

  1. π_g
  2. 0
  3. 2π_g (assuming full dissociation, i=2)
  4. π_g/2
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Correct answer: C. 2π_g (assuming full dissociation, i=2)

NaCl dissociates into Na⁺ + Cl⁻, doubling particle count. So π_NaCl ≈ 2 × π_glucose ≈ 4.92 atm. Glucose stays as molecules, i = 1.

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