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Indian Navy 10+2 B.Tech Cadet Solutions — practice questions

Explore 18 free Solutions questions in Indian Navy 10+2 B.Tech Cadet Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Showing questions 1–18 of 18.

The van't Hoff factor $i$ for a $0.01$ M aqueous solution of NaCl, assuming complete dissociation, is approximately:Read the answer and worked solution →What is the molarity of a solution containing 5.85 g of NaCl (M.W. = 58.5) in 250 mL of solution?Read the answer and worked solution →For 0.5 m solutions of NaCl, KCl, and BaCl2, which gives largest ΔT_f?Read the answer and worked solution →Molarity M is defined as:Read the answer and worked solution →For salt CaCl₂ (assume full dissociation), i =Read the answer and worked solution →HENRY'S LAW states that at constant temperature: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

The van't Hoff factor $i$ for a $0.01$ M aqueous solution of NaCl, assuming complete dissociation, is approximately:

  1. $1$
  2. $0.5$
  3. $2$
  4. $3$
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Correct answer: C. $2$

NaCl dissociates in water: $\mathrm{NaCl} \rightarrow \mathrm{Na^+} + \mathrm{Cl^-}$. One formula unit produces two particles in solution. Van't Hoff factor $i = \dfrac{\text{actual moles of particles}}{\text{moles of solute formula units}}$. For complete dissociation of NaCl, $i = 2$. In reality, ion pairing slightly reduces $i$ below the theoretical value, especially at higher concentrations. At dilute $0.01$ M the assumption of complete dissociation is reasonable, and the experimental $i$ is close to $1.9$. The question asks for the theoretical value assuming complete dissociation, so 2 is the cleanest answer. Compare with $\mathrm{CaCl_2}$: dissociates into 3 ions, so $i = 3$ (option D) — common trap.

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What is the molarity of a solution containing 5.85 g of NaCl (M.W. = 58.5) in 250 mL of solution?

  1. 0.2 M
  2. 0.1 M
  3. 0.4 M
  4. 1 M
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Correct answer: C. 0.4 M

Moles of NaCl = 5.85/58.5 = 0.1 mol. Volume = 0.25 L. Molarity = 0.1/0.25 = 0.4 M.

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For 0.5 m solutions of NaCl, KCl, and BaCl2, which gives largest ΔT_f?

  1. NaCl (i=2)
  2. KCl (i=2)
  3. All equal
  4. BaCl2 (i=3)
Show answer and solution

Correct answer: D. BaCl2 (i=3)

ΔT_f ∝ i × m. BaCl2 has highest i = 3, so largest ΔT_f. ΔT_f = 1.86 × 3 × 0.5 = 2.79 K for BaCl2; 1.86 K for NaCl/KCl.

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