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AP Intermediate 2nd Year Solutions — practice questions

Explore 53 free Solutions questions in AP Intermediate 2nd Year 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 1–30 of 53.

Colligative properties of a dilute solution depend on:Read the answer and worked solution →$36$ g of glucose ($M = 180$ g/mol) is dissolved in $200$ g of water. The molality of the solution is:Read the answer and worked solution →The mole fraction of urea ($M = 60\,\text{g/mol}$) in an aqueous solution containing $6\,\text{g}$ of urea in $180\,\text{g}$ of water is approximately:Read the answer and worked solution →For an ideal solution containing two volatile liquids A and B, Raoult's law gives the total vapour pressure as:Read the answer and worked solution →Osmotic pressure of a dilute solution is expressed by van't Hoff's equation as:Read the answer and worked solution →Two solutions are said to be **isotonic** if they:Read the answer and worked solution →If $\mathrm{NaCl}$ undergoes complete dissociation in water, the van't Hoff factor $i$ is:Read the answer and worked solution →Desalination of sea water is best carried out by:Read the answer and worked solution →With increase in temperature, the solubility of most gases in water:Read the answer and worked solution →The MOLARITY of a solution containing 58.5 g NaCl dissolved in 1 L of solution is:Read the answer and worked solution →HENRY'S LAW states that at constant temperature:Read the answer and worked solution →A MINIMUM-BOILING azeotrope arises from:Read the answer and worked solution →Which of these is NOT a colligative property?Read the answer and worked solution →Salt is sprinkled on icy roads in cold countries to:Read the answer and worked solution →The van't Hoff factor (i) for sodium chloride (NaCl) in water is approximately:Read the answer and worked solution →NEET · Chemistry · Colligative PropertiesRead 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 →HENRY'S LAW states that at constant temperature:Read the answer and worked solution →Salt is sprinkled on icy roads in cold countries to:Read the answer and worked solution →

Worked practice questions

Colligative properties of a dilute solution depend on:

  1. The pressure only
  2. The temperature only
  3. The number of solute particles, not their nature
  4. The chemical nature of the solute
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Correct answer: C. The number of solute particles, not their nature

By definition, colligative properties (relative lowering of vapour pressure, boiling-point elevation, freezing-point depression, osmotic pressure) depend on how many solute particles are dissolved, not what those particles are. One mole of glucose and one mole of urea cause the same boiling-point elevation in 1 kg of water. With electrolytes like NaCl that dissociate into 2 ions, the effective particle count is multiplied by the van't Hoff factor $i$ (close to 2 for NaCl in dilute solution).

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$36$ g of glucose ($M = 180$ g/mol) is dissolved in $200$ g of water. The molality of the solution is:

  1. $0.5$ mol/kg
  2. $2.0$ mol/kg
  3. $0.1$ mol/kg
  4. $1.0$ mol/kg
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Correct answer: D. $1.0$ mol/kg

Moles of glucose: $\dfrac{36}{180} = 0.2$ mol. Mass of solvent in kilograms: $\dfrac{200}{1000} = 0.2$ kg. Molality: $m = \dfrac{0.2}{0.2} = 1.0$ mol/kg. Note the use of solvent mass (not solution mass) in the denominator: that distinction separates molality from molarity. For very dilute aqueous solutions the two are numerically close, but they diverge for concentrated solutions.

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The mole fraction of urea ($M = 60\,\text{g/mol}$) in an aqueous solution containing $6\,\text{g}$ of urea in $180\,\text{g}$ of water is approximately:

  1. $0.010$
  2. $0.005$
  3. $0.100$
  4. $0.050$
Show answer and solution

Correct answer: A. $0.010$

Moles of urea $= 6/60 = 0.10$. Moles of water $= 180/18 = 10.0$. Mole fraction of urea $= 0.10/(0.10 + 10.0) = 0.10/10.10 \approx 0.0099 \approx 0.010$.

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