Chemistry Solutions and Properties Quiz
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Questions and Answers

What is the formula to calculate normality?

  • N = Molarity / n
  • N = grams/L
  • N = Molarity x concentration
  • N = Molarity x n (correct)

If you dissolve 50g of H2SO4 in 15 L of solution, what is its normality?

  • 1.00 N
  • 0.10 N
  • 0.068 N (correct)
  • 0.034 N

Which colligative property describes the lowering of a solvent's vapor pressure due to the presence of a solute?

  • Freezing-point depression
  • Vapor-pressure lowering (correct)
  • Boiling-point elevation
  • Osmotic pressure

What primarily determines colligative properties?

<p>The number of solute particles in solution (D)</p> Signup and view all the answers

What relationship does freezing-point depression have with the number of solute particles in a solution?

<p>It is directly proportional to the number of solute particles. (D)</p> Signup and view all the answers

What is the PPM concentration of NaCl when 4mg is dissolved in 8 kg of water?

<p>0.5 PPM (B)</p> Signup and view all the answers

Given 5m of NaCl, what is the calculated freezing-point depression?

<p>-3.72 °C (C)</p> Signup and view all the answers

In the context of colligative properties, what does a decrease in vapor pressure indicate?

<p>Presence of a non-volatile solute (D)</p> Signup and view all the answers

Which formula correctly represents the relationship for boiling-point elevation?

<p>ΔT = Kb x m x i (A)</p> Signup and view all the answers

Why is normality important in chemical reactions?

<p>It reflects the reactivity based on concentration of reactive units. (A)</p> Signup and view all the answers

For a solution of 10m KCl, what is the expected boiling-point elevation?

<p>10.2 °C (D)</p> Signup and view all the answers

Which of the following is NOT a colligative property?

<p>Density of the solution (A)</p> Signup and view all the answers

What does the constant Kf represent in the freezing-point depression formula?

<p>The freezing-point depression constant (C)</p> Signup and view all the answers

If the boiling-point elevation for a solvent is Kb = 0.51, what is the boiling-point elevation when 5m KI is dissolved in the solvent?

<p>5.1 °C (C)</p> Signup and view all the answers

What factor does NOT affect freezing-point depression?

<p>The identity of the solute (B)</p> Signup and view all the answers

How much would the boiling point increase if 2 moles of CaCl2 are dissolved in 1 kg of water with Kb = 0.512?

<p>5.12 °C (B)</p> Signup and view all the answers

Flashcards

Colligative property

A property of a solution that depends only on the number of solute particles present, not their identity. It is a colligative property because it is affected by the concentration of the solution.

Vapor-pressure lowering

The decrease in the vapor pressure of a solvent when a non-volatile solute is added. This is because the solute molecules occupy some of the surface of the solution, reducing the number of solvent molecules that can escape into the vapor phase.

Vapor-pressure lowering

The difference in the vapor pressure of a pure solvent and a solution. It is directly proportional to the molal concentration of the solute.

Boiling-point elevation

The temperature at which the vapor pressure of a liquid equals the external pressure. The boiling point of a solution is higher than that of the pure solvent due to the vapor-pressure lowering effect.

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Freezing-point depression

The difference between the freezing point of the pure solvent and that of the solution. It is directly proportional to the molal concentration of the solute.

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Freezing-point depression

The temperature at which a liquid changes to a solid. The freezing point of a solution is lower than that of the pure solvent due to the vapor-pressure lowering effect.

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Normality

A unit of concentration that expresses the number of equivalents of a solute per liter of solution. Normality is mainly used in acid-base chemistry.

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Parts per million (ppm)

A way to express the concentration of a solute in a solution. It is defined as the mass of solute per million units of mass of solution. It is often used for very dilute solutions.

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Freezing-Point Depression Constant (Kf)

A constant that represents the amount of freezing-point depression caused by 1 molal solution of a non-volatile solute in a particular solvent.

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Freezing Point of a Solution

The freezing point of a solution is lower than the freezing point of the pure solvent.

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Boiling-Point Elevation Constant (Kb)

A constant that represents the amount of boiling-point elevation caused by 1 molal solution of a non-volatile solute in a particular solvent.

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Boiling Point of a Solution

The boiling point of a solution is higher than the boiling point of the pure solvent.

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Molality (m)

The number of moles of solute dissolved in 1 kg of solvent.

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Van't Hoff Factor (i)

The number of particles a solute dissociates into when dissolved in a solvent.

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Study Notes

Chemical Composition of Water

  • Water's chemical composition is H₂O

Colligative Properties of Solutions

  • Colligative properties depend on the number of solute particles, not their identity.
  • Important colligative properties include vapor-pressure lowering, boiling-point elevation, and freezing-point depression.

Normality

  • Normality (N) is the equivalent concentration.
  • N = Molarity (M) x n
  • n represents the number of protons/hydrogen ions.
  • Calculations for normality (N) are shown for HCl, H₂SO₄, NaOH, and Ba(OH)₂.

Parts Per Million (PPM)

  • PPM = (grams of solute /grams of solution ) x 10⁶
  • An example calculation for finding the concentration of NaCl (4mg) in 8 kg of water is provided.

Freezing-Point Depression

  • The freezing point of a solution is lower than the freezing point of the pure solvent.
  • The magnitude of the freezing-point depression is proportional to the number of solute particles.
  • Calculations for freezing-point depression (ΔT) using the formula ΔT = Kf × m × i are shown for examples with NaCl, 5m NaCl, and 5m AlCl₃.

Boiling-Point Elevation

  • The boiling point of a solution is higher than the boiling point of the pure solvent.
  • The magnitude of the boiling-point elevation is proportional to the number of solute particles.
  • Boiling point elevation is calculated using the formula ΔT =Kb × m × i, showing examples with NaCl, 5m KI, and 10m KCl.

Assessment: Boiling Point Elevation Calculation

  • Calculate the boiling-point elevation for a solution of 2 moles of CaCl₂ in 1 kg of water, given the boiling-point elevation constant (Kb) for water is 0.512.

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Description

Test your knowledge on the chemical composition of water and the colligative properties of solutions. Explore concepts like normality, parts per million, and the effects of solute particles on freezing-point depression. Perfect for chemistry enthusiasts!

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