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KCET Solutions — practice questions — page 2

Explore 63 free Solutions questions in KCET 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 31–60 of 63.

Molality m is defined as:Read the answer and worked solution →Henry's law states partial pressure of a gas above liquid is proportional to:Read the answer and worked solution →Raoult's law for ideal solution states vapor pressure of solvent:Read the answer and worked solution →For dilute solutions, lowering of vapor pressure of solvent ΔP / P°_A =Read the answer and worked solution →Elevation in boiling point ΔT_b for solution of non-volatile solute:Read the answer and worked solution →Depression in freezing point ΔT_f for non-electrolyte solute:Read the answer and worked solution →Osmotic pressure π for dilute solution:Read the answer and worked solution →For NaCl in water (assumes complete dissociation), van't Hoff factor i =Read the answer and worked solution →For 0.1 M urea in water, freezing point depression (K_f = 1.86):Read the answer and worked solution →Mass percent of solute = (mass of solute / mass of solution) × 100. For 5 g NaCl in 95 g water:Read the answer and worked solution →Two volatile liquids A (P°_A = 100) and B (P°_B = 200) form ideal solution. For x_A = 0.4, total vapor pressure:Read the answer and worked solution →Osmotic pressure of 0.01 M sucrose solution at 27°C (R = 0.0821 L atm/mol K):Read the answer and worked solution →For solution of urea (M_w = 60 g/mol) with 6 g in 100 g water, molality:Read the answer and worked solution →For 0.1 M acetic acid (Ka = 1.8 × 10⁻⁵), van't Hoff factor i is:Read the answer and worked solution →For salt CaCl₂ (assume full dissociation), i =Read the answer and worked solution →For a 1 m glucose aqueous solution (i = 1), boiling point:Read the answer and worked solution →Freezing-point depression and elevation are colligative properties: depend on:Read the answer and worked solution →Match each concentration termRead the answer and worked solution →Knock out the temperature mythsRead the answer and worked solution →Catch the concentration termsRead the answer and worked solution →Key in the solution numbersRead 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 →

Worked practice questions

Molality m is defined as:

  1. Mass per kg
  2. Moles of solute per kg of SOLVENT (temperature independent)
  3. Moles of solute per liter of solution
  4. Same as molarity
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Correct answer: B. Moles of solute per kg of SOLVENT (temperature independent)

m = moles solute / kg solvent. T-independent (mass doesn't change with T). Preferred in colligative property calculations (involve temperature).

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Henry's law states partial pressure of a gas above liquid is proportional to:

  1. Temperature
  2. Density
  3. Volume
  4. Solute mole fraction × Henry's constant: p = K_H × x
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Correct answer: D. Solute mole fraction × Henry's constant: p = K_H × x

**Henry's law:** p_gas = K_H × x_gas-in-solution. Used in carbonated drinks (CO₂ solubility), respiration (O₂ in blood). K_H depends on gas, solvent, T.

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Raoult's law for ideal solution states vapor pressure of solvent:

  1. P_A = P°_A × x_A (mole fraction in solution)
  2. P_A = x_B × P°_A
  3. P_A = K_H × x_A
  4. P_A = P°_A always
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Correct answer: A. P_A = P°_A × x_A (mole fraction in solution)

**Raoult's law:** vapor pressure of each component in ideal solution = its pure-state vapor pressure × mole fraction. P_total = P°_A x_A + P°_B x_B. Foundation of distillation.

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More Chemistry topics

Chemical EquilibriumElectrochemistryCoordination CompoundsElectrochemical SeriesIdeal and Non-Ideal SolutionsIdeal SolutionsNon-Ideal SolutionsReactions in Aqueous Solution