Solutions: Physical Properties and Types
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What does the term 'mole fraction' represent?

  • The total number of atoms present in a compound
  • The ratio of the number of moles of a component to the total number of moles in a mixture (correct)
  • The number of moles of a substance per liter of solution
  • The mass of solute in kilograms divided by the volume of solvent in liters

    • In a redox reaction, what does 'a' represent when dealing with the reaction of $C_{2}O_{4}^{2-} → CO_{2}$?

  • The molarity of the reactants involved
  • The mass ratio of the products to reactants
  • The total number of electrons gained or lost during the reaction (correct)
  • The concentration of the oxidizing agent

    • What is the unit of measurement for molality?

  • moles per liter
  • grams per liter
  • moles per kilogram (correct)
  • equivalents per liter

    • Which statement is true regarding molarity (M) and normality (N)?

    <p>M relates to the amount of solute in liters while N relates to equivalents</p> Signup and view all the answers

    For the compound Ca(NO3)2, what is the total equivalent (a) value when considering its ions in solution?

    <p>2 eq/mol</p> Signup and view all the answers

    What describes a saturated solution?

    <p>It contains the maximum amount of solute the solvent can dissolve.</p> Signup and view all the answers

    Which of the following accurately defines a supersaturated solution?

    <p>A solution that contains more solute than the solubility allows.</p> Signup and view all the answers

    What characterizes an unsaturated solution?

    <p>It can still dissolve additional solute.</p> Signup and view all the answers

    Which statement correctly describes nonelectrolytes?

    <p>They do not dissociate into ions.</p> Signup and view all the answers

    When a solute dissolves in a solvent, which of the following events does NOT occur?

    <p>Solvent particles combine with solute atoms.</p> Signup and view all the answers

    What distinguishes organic compounds from inorganic compounds?

    <p>Organic compounds contain carbon, while inorganic do not.</p> Signup and view all the answers

    Which of the following statements is true regarding the solubility process?

    <p>Both solute and solvent particles must separate from each other.</p> Signup and view all the answers

    Why is a supersaturated solution considered unstable?

    <p>It exceeds the solubility limit, which can lead to precipitation.</p> Signup and view all the answers

    What occurs to the concentration of a solution when it is diluted by adding more solvent?

    <p>It decreases.</p> Signup and view all the answers

    Using the dilution formula $M_1V_1 = M_2V_2$, if you have a 0.50 M solution and dilute it to 750 mL, what can be inferred about the initial concentration?

    <p>It is greater than 0.50 M.</p> Signup and view all the answers

    If the normality of K2Cr2O7 is given as 0.200 N, what does this indicate about the equivalent relationships?

    <p>0.200 equivalents per liter of solution.</p> Signup and view all the answers

    How would you calculate the volume of a 12.0 M HCl solution needed to prepare 300 mL of a 3.00 M solution?

    <p>$V_1 = (3.00)(300)/(12.0)$</p> Signup and view all the answers

    What is the direct conversion relationship between Normality (N) and Molarity (M) for H2SO4, given that

    <p>N = 2M.</p> Signup and view all the answers

    If 15.0 g of CuSO4 is converted to a 0.125 N solution, how would you determine the volume of the solution prepared?

    <p>Convert mass to moles and then use $N = (number of equivalents)/(L of solution)$</p> Signup and view all the answers

    What is the molality of a solution created by dissolving 36.5 g of naphthalene in 420 g of toluene?

    <p>0.87 m.</p> Signup and view all the answers

    Which equation describes the relationship between molarity (M) and normality (N)?

    <p>N = M × number of equivalents per mole.</p> Signup and view all the answers

    What is the percentage by weight of NaCl in a solution containing 15.0 g of NaCl in 100 g of water?

    <p>15.0%</p> Signup and view all the answers

    How much vinegar is needed to obtain 80.0 g of acetic acid if the vinegar is 5.00% acetic acid by weight?

    <p>2000 g</p> Signup and view all the answers

    What is the mass of sodium hypochlorite (NaOCl) in a 2.50 g bleaching solution that contains 3.62 mass % sodium hypochlorite?

    <p>0.0905 g</p> Signup and view all the answers

    What is the molality of a solution containing 0.850 g of ammonia (NH3) dissolved in 125.0 g of water?

    <p>0.063 mol/kg</p> Signup and view all the answers

    Calculate the molality of an aqueous solution of NaCl if 0.250 kg of the solution contains 40.0 g of NaCl.

    <p>0.150 mol/kg</p> Signup and view all the answers

    How do you calculate the molarity of a solution prepared by dissolving 0.827 g NaCl in enough solvent to make 250 mL of solution?

    <p>Molarity = moles of solute / liters of solution</p> Signup and view all the answers

    Given a concentrated sulfuric acid solution with a density of 1.84 g/mL and 98.3% H2SO4 by weight, what is the molarity of this acid?

    <p>19.5 M</p> Signup and view all the answers

    Which factor affects the solubility of gases according to the principles of solubility?

    <p>Increasing temperature</p> Signup and view all the answers

    What happens to the boiling point of a solution compared to that of the pure solvent?

    <p>It is higher than the boiling point of the pure solvent.</p> Signup and view all the answers

    According to Raoult’s Law, what is the relationship between boiling point elevation and molality?

    <p>Boiling point elevation is directly proportional to molality.</p> Signup and view all the answers

    What occurs to the vapor pressure of a solution when a nonvolatile solute is added?

    <p>It decreases compared to the pure solvent.</p> Signup and view all the answers

    Which of the following is true regarding colligative properties?

    <p>They depend solely on the concentration of solute particles.</p> Signup and view all the answers

    What is the formula for calculating boiling point elevation?

    <p>ΔTb = Kb·m</p> Signup and view all the answers

    The term 'vapor pressure lowering' is best described as which of the following?

    <p>The decrease in vapor pressure of a solvent caused by a solute.</p> Signup and view all the answers

    Which type of solutions does Raoult’s Law apply to?

    <p>Non-volatile and non-electrolytic solutions.</p> Signup and view all the answers

    How does temperature affect the vapor pressure of a liquid?

    <p>Higher temperature results in higher vapor pressure.</p> Signup and view all the answers

    What does Raoult's Law predict regarding the vapor pressure of solutions?

    <p>It is lower than that of the solvent.</p> Signup and view all the answers

    What is the formula for calculating freezing point depression according to Raoult's Law?

    <p>Tf' - Tf = Kfm</p> Signup and view all the answers

    Which component does NOT affect the freezing point of an ideal solution?

    <p>Vapor pressure of the solute</p> Signup and view all the answers

    Which statement is true regarding the behavior of ideal solutions?

    <p>They follow Raoult's Law at low solute concentrations.</p> Signup and view all the answers

    What happens to the freezing point of a solution as its molality increases?

    <p>It decreases.</p> Signup and view all the answers

    Which substance has the highest freezing point according to the constants provided?

    <p>Water</p> Signup and view all the answers

    In a solution with components A and B, how can the total vapor pressure be calculated?

    <p>PTOTAL = PA + PB</p> Signup and view all the answers

    Under which condition does reverse osmosis occur?

    <p>When applied pressure is greater than osmotic pressure.</p> Signup and view all the answers

    What does the cryoscopic constant (Kf) indicate for a particular solvent?

    <p>The freezing point depression per molal concentration.</p> Signup and view all the answers

    Which of the following best describes an ideal solution?

    <p>It exhibits lower vapor pressure than each pure component.</p> Signup and view all the answers

    Study Notes

    Solutions: Physical Properties

    • A solution is a homogenous mixture of two or more components, adjustable in composition.
    • The solvent is the component present in the largest amount.
    • The solute is the other component(s) dissolved in the solvent.
    • Aqueous solutions have water as the solvent.
    • Solvation is the interaction between solute and solvent molecules, driven by intermolecular forces (IMFs). For example, Na⁺ and Cl⁻ ions are surrounded by water molecules.
    • Hydration refers to solvation when the solvent is water.

    Types of Solutions

    • Dilute solutions have a low solute concentration.
    • Concentrated solutions have a high solute concentration.
    • Solubility is the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature.
    • A saturated solution contains the maximum amount of solute that can dissolve at a given temperature; adding more solute will not dissolve.
    • An unsaturated solution contains less solute than the maximum possible at a given temperature; more solute can dissolve.
    • A supersaturated solution contains more solute than the maximum possible at a given temperature; it is unstable, and excess solute will precipitate out.

    Electrolytes and Nonelectrolytes

    • Strong electrolytes completely dissociate into ions in solution, resulting in good electrical conductivity. Examples include salts (NaCl), strong acids (HCl), and strong bases (NaOH).
    • Weak electrolytes partially dissociate into ions in solution, leading to weaker electrical conductivity. Examples include weak acids (CH₃COOH) and weak bases.
    • Nonelectrolytes do not dissociate into ions in solution, and therefore their solutions are non-conducting. Most molecular compounds are nonelectrolytes.

    The Solution Process

    • For a substance to dissolve in another, solute particles must separate from each other, solvent particles must separate from each other, and then both solute and solvent particles must mix.
    • The separating processes require overcoming intermolecular forces.
    • The mixing process involves attractive forces between solute and solvent particles.

    Ways of Expressing Concentration

    • Mass percentage: (mass of component/total mass of solution) x 100%
    • Volume percentage: (volume of component/total volume of solution) x 100%
    • Parts per million (ppm): (mass of component/total mass of solution) x 10⁶
    • Parts per billion (ppb): (mass of component/total mass of solution) x 10⁹
    • Mole fraction (X): (moles of component/total moles of all components)
    • Molality (m): (moles of solute/kilograms of solvent) - independent of temperature.
    • Molarity (M): (moles of solute/litres of solution) - dependent on temperature.
    • Normality (N): (equivalents of solute/litres of solution).

    Factors Affecting Solubility

    • Temperature: Increasing temperature typically increases solubility of solids in liquids but decreases solubility of gases in liquids.
    • Nature of solute and solvent: "Like dissolves like." Polar solvents dissolve polar solutes, and nonpolar solvents dissolve nonpolar solutes.
    • Pressure: Increasing pressure increases solubility of gases in liquids.

    Colligative Properties

    • Colligative properties depend only on the concentration of solute particles, not their nature. These properties are observed in non-volatile and non-electrolyte solutions.
    • Vapor pressure lowering: The vapor pressure of a solution is lower than the vapor pressure of the pure solvent.
    • Boiling point elevation: The boiling point of a solution is higher than the boiling point of the pure solvent.
    • Freezing point depression: The freezing point of a solution is lower than the freezing point of the pure solvent.
    • Osmotic pressure: The pressure required to prevent the net flow of solvent across a semipermeable membrane.

    Other concepts

    • Dilution formula: M₁V₁ = M₂V₂
    • Relationships of Molarity and Normality: N = M * a

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    Description

    This quiz covers the physical properties of solutions and their types, including definitions of solute, solvent, and concepts like dilution, concentration, and solubility. Explore relationship dynamics like solvation and hydration, as well as the characteristics of saturated and unsaturated solutions.

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