Solubility Unit Quiz
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Questions and Answers

What occurs when ionic compounds are separated into their individual ions?

  • Dissociation (correct)
  • Precipitation
  • Solvation
  • Hydration

    • Which statement accurately describes a saturated solution?

  • It is at equilibrium with the solute and solvent. (correct)
  • It contains no undissolved solute.
  • It contains more solute than can usually dissolve.
  • It is unable to dissolve any solute.

    • Which factor does NOT affect the solubility of a solute in a solvent?

  • Temperature of the solution
  • Size of the solute particles (correct)
  • Nature of the solute and solvent
  • Pressure of the environment

    • What happens to the solubility of most solid solutes as temperature increases?

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

    Which of the following is an example of a covalent solid dissolving in water?

    <p>C6H12O6 (s) → C6H12O6 (aq)</p> Signup and view all the answers

    What is the definition of 'hydration' in the context of solubility?

    <p>The process by which solute molecules are surrounded by solvent molecules.</p> Signup and view all the answers

    What is true regarding the solubility of gases in liquids as temperature increases?

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

    What characterizes the particles in a colloid compared to those in a suspension?

    <p>Colloid particles are smaller and do not settle out.</p> Signup and view all the answers

    What does 'like dissolves like' refer to in the context of solubility?

    <p>Similar types of substances tend to dissolve well together.</p> Signup and view all the answers

    In a dissociation equation, what are the products generated when a chemical dissolves?

    <p>Ions only</p> Signup and view all the answers

    What is the molarity of a solution if 0.75 moles of CaCl are dissolved in 2.5 liters of solution?

    <p>0.3 M</p> Signup and view all the answers

    How many grams of KCl are needed to create a 0.2 M solution in 1.8 L of water?

    <p>30 g</p> Signup and view all the answers

    If you need to dilute 18 M H2SO4 to create 2 M H2SO4, how much of the concentrated solution is required for 1.5 L of the diluted solution?

    <p>0.167 L</p> Signup and view all the answers

    To what volume does 10 g of NaCl increase the molarity of an existing 180 mL solution to get the new molarity?

    <p>230 mL</p> Signup and view all the answers

    What does Henry's law state regarding the solubility of gases?

    <p>Solubility is directly proportional to the pressure of the gas above the liquid.</p> Signup and view all the answers

    What is the relationship between molarity (M) and concentration?

    <p>Molarity is a measure of concentration in moles per liter.</p> Signup and view all the answers

    Which of the following is NOT a factor affecting the rate of dissolving?

    <p>Pressure of the gas above the liquid</p> Signup and view all the answers

    What does a chemical need to be classified as an electrolyte?

    <p>It must dissolve in water and produce ions.</p> Signup and view all the answers

    What characterizes an undersaturated solution?

    <p>It is below the solubility curve.</p> Signup and view all the answers

    Which colligative property relates to the need for more heat to boil a solution?

    <p>Boiling point elevation</p> Signup and view all the answers

    How does the presence of a solute in a solution affect vapor pressure?

    <p>It reduces the vapor pressure due to interference with vaporization.</p> Signup and view all the answers

    What is a key characteristic of a suspension?

    <p>It settles out if left undisturbed.</p> Signup and view all the answers

    What happens to the freezing point of water when a solute is added?

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

    What differentiates a solution from a mixture?

    <p>Solutions are uniform in composition with a single phase.</p> Signup and view all the answers

    What is the molarity of the new solution after adding 10g of NaCl to the original 0.18L solution?

    <p>2.44M</p> Signup and view all the answers

    How many moles of HCl are present in 1.5L of a 3.5M solution?

    <p>5.25 mol</p> Signup and view all the answers

    Using reaction stoichiometry, how many moles of Mg are required to react with 5.25 moles of HCl?

    <p>2.625 mol</p> Signup and view all the answers

    What is the molarity of the solution when 150 ml of a 2M solution is mixed with 550 ml of a 3.5M solution?

    <p>3.17M</p> Signup and view all the answers

    What is the final mass of Na2SO4 formed when 500ml of a 4.5M solution of H2SO4 is mixed with excess NaOH?

    <p>126.5g</p> Signup and view all the answers

    How many grams of magnesium (Mg) are needed to react with 5.25 moles of HCl?

    <p>63.85g</p> Signup and view all the answers

    Which balanced equation correctly represents the reaction between sulfuric acid and sodium hydroxide?

    <p>H2SO4 + 2NaOH -&gt; Na2SO4 + H2O</p> Signup and view all the answers

    What is the total volume of the resulting solution when 150 ml of a 2M solution is mixed with 550 ml of a 3.5M solution?

    <p>700 ml</p> Signup and view all the answers

    What is the term used when solvent molecules surround solute molecules?

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

    What happens to the solubility of gases in liquids at higher temperatures?

    <p>Solubility decreases</p> Signup and view all the answers

    Which of the following best describes a saturated solution?

    <p>At equilibrium with crystallization</p> Signup and view all the answers

    What does the term 'crystallization' refer to in the context of solutions?

    <p>Formation of solid solute from a saturated solution</p> Signup and view all the answers

    What characteristic best illustrates the phrase 'like dissolves like'?

    <p>Polar solvents dissolve polar solutes</p> Signup and view all the answers

    Which condition is required for a solution to be classified as super-saturated?

    <p>Contains more solute than maximum without crystallization</p> Signup and view all the answers

    In which scenario would you expect an increase in the solubility of a solid solute?

    <p>Increase in temperature</p> Signup and view all the answers

    What is the primary factor that affects the rate of dissolving an ionic solid in water?

    <p>Temperature of the water</p> Signup and view all the answers

    What is the molarity of a solution that contains 50g of sodium chloride (NaCl) dissolved in 1L of water? (Molar mass of NaCl = 58.44 g/mol)

    <p>1.0 M</p> Signup and view all the answers

    How many grams of potassium chloride (KCl) are in a 0.5 M solution with a total volume of 3 L? (Molar mass of KCl = 74.55 g/mol)

    <p>222.65 g</p> Signup and view all the answers

    What is the final concentration of sodium chloride after mixing 100 mL of a 3M solution with 400 mL of a 1.5M solution?

    <p>2.25 M</p> Signup and view all the answers

    What volume of water is needed to dilute 500 mL of a 5M solution of HCl to a 1M solution?

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

    To create a 0.5 M solution, how many moles of solute are needed in 1.5 L of solution?

    <p>0.75 moles</p> Signup and view all the answers

    What final concentration results from combining 250 mL of a 2M solution and 750 mL of a 4M solution?

    <p>3.0 M</p> Signup and view all the answers

    If 10g of NaCl are added to 500 mL of a solution already at 1 M, what will be the new molarity? (NaCl = 58.44 g/mol)

    <p>1.5 M</p> Signup and view all the answers

    What is the number of moles in 2 L of a 2.5M solution?

    <p>5.0 moles</p> Signup and view all the answers

    What effect does increasing the surface area of a solute have on its rate of dissolving?

    <p>It increases the rate of dissolution.</p> Signup and view all the answers

    How does the presence of a solute affect the boiling point of a solution compared to pure solvent?

    <p>It raises the boiling point and requires more heat to boil.</p> Signup and view all the answers

    Which of the following correctly describes an undersaturated solution?

    <p>It has not reached its maximum solubility and can dissolve more solute.</p> Signup and view all the answers

    What happens to the freezing point of a solution when a solute is added?

    <p>It decreases, requiring more energy removal to solidify.</p> Signup and view all the answers

    Which of the following is NOT a colligative property?

    <p>Melting point elevation</p> Signup and view all the answers

    What is the relationship described by Henry's law?

    <p>The solubility of a gas in a liquid is directly proportional to the pressure of the gas above it.</p> Signup and view all the answers

    What characterizes a suspension compared to a colloid?

    <p>A suspension will settle out if left undisturbed.</p> Signup and view all the answers

    What is indicated by a high vapor pressure in a liquid?

    <p>The liquid is likely to evaporate quickly.</p> Signup and view all the answers

    What is the final molarity of the new solution after adding 10g of NaCl to the original 0.18L solution with a molarity of 1.5M?

    <p>2.44M</p> Signup and view all the answers

    How many moles of magnesium (Mg) are needed to react with 5.25 moles of hydrochloric acid (HCl)?

    <p>2.625 moles</p> Signup and view all the answers

    What is the total volume of the resulting solution when mixing 150 mL of a 2M solution with 550 mL of a 3.5M solution?

    <p>700 mL</p> Signup and view all the answers

    How many grams of Na2SO4 are produced when 500 mL of a 4.5M solution of H2SO4 is reacted with excess NaOH?

    <p>110.5 g</p> Signup and view all the answers

    Given the molar masses of Na (22.989 g/mol) and Cl (35.457 g/mol), what is the total mass of NaCl produced from 0.17 moles?

    <p>10.03 g</p> Signup and view all the answers

    What is the molarity of HCl if 1.5L of 3.5M solution provides how many moles of HCl?

    <p>5.25 moles</p> Signup and view all the answers

    What stoichiometric relationship can be established from the reaction between Mg and HCl?

    <p>1 mole of Mg reacts with 2 moles of HCl</p> Signup and view all the answers

    When diluting a solution, what would be the correct formula to calculate molarity after mixing different volumes?

    <p>($M_1V_1$ + $M_2V_2$) / ($V_1 + V_2$) = $M_f$</p> Signup and view all the answers

    Study Notes

    Solubility Unit

    • Ionic compounds arrange themselves to increase attractive forces between ions and decrease repulsive forces. This arrangement is known as a crystal structure or lattice.
    • Polar solvent molecules surround each ion.
    • Separation of ions is called dissociation.
    • Solvation is when solute molecules are surrounded by solvent molecules.
    • Hydration is solvation when the solvent is water.
    • Covalent molecules are held together by weak intermolecular forces.
    • During solvation, each molecule is surrounded by solvent molecules.
    • Solvents do not appear in dissolving equations.
    • Ionic solids separate into ions (e.g., NH₄NO₃ → NH₄⁺(aq) + NO₃⁻(aq)).
    • Covalent solids just separate between molecules (e.g., C₆H₁₂O₆(s) → C₆H₁₂O₆(aq)).

    Definitions

    • Undersaturated: A solution containing less than the maximum amount of solute that can be dissolved (dissolving > crystallization).
    • Saturated: A solution containing the maximum amount of solute that can be dissolved (dissolving = crystallization).
    • Supersaturated: A solution containing more than the maximum amount of solute under special conditions, but crystallization does not occur.

    Factors Affecting Solubility

    • Nature of Solute and Solvent ("Like Dissolves Like"):
      • Substances with similar intermolecular forces dissolve each other more readily.
      • Polar substances dissolve polar substances, and nonpolar substances dissolve nonpolar substances.
    • Temperature:
      • Generally, the solubility of a solid or liquid solute increases with temperature. (e.g., sugar in hot tea vs. cold tea).
      • Solubility of gases decreases with increasing temperature.
      • Particles with more kinetic energy can escape the solution more quickly (e.g., cold pop vs. warm pop).
    • Pressure:
      • Only applies to solutions of gases in liquids.
      • Henry's Law: The solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.

    Rate of Dissolving

    • Surface Area: Increasing surface area increases solute-solvent collisions, leading to faster dissolving (e.g., dissolving a cube of sugar vs. a teaspoon of sugar).
    • Amount of Solute Already Dissolved: As a solution approaches saturation, dissolving becomes slower.
    • Equilibrium: Dissolving and crystallization occur at the same rate in a saturated solution. This is called equilibrium.
    • Solubility: The maximum amount of a solute that can dissolve in a given amount of solvent at a specific temperature.

    Colligative Properties

    • Colligative properties depend on the concentration of solute particles (number), not the type of solute.
    • Vapor Pressure Reduction: Solute particles interfere with evaporation, lowering the vapor pressure of a solution.
    • Boiling Point Elevation: Increased pressure requires a higher temperature for boiling.
    • Freezing Point Depression: Solute particles disrupt the formation of the solid phase, lowering the freezing point of a solution.

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    Solubility Unit PDF

    Description

    Test your knowledge on the solubility unit, covering key concepts such as ionic and covalent solvation, dissociation, and hydration. This quiz will challenge your understanding of how different types of compounds interact with solvents and the definitions of supersaturated, saturated, and undersaturated solutions.

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