Chemistry: Solutions and Solubility
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Questions and Answers

Which component of a solution is present in the greatest amount?

  • Mixture
  • Colloidal substance
  • Solute
  • Solvent (correct)

    • What defines solubility in a solution?

  • The maximum amount of solute that can dissolve in a given amount of solvent (correct)
  • The process of a solute returning to its original state
  • The ability of the solute to affect the solvent's properties
  • The temperature at which a solution becomes saturated

    • Which statement about solutions is true?

  • Solutions are always composed of liquid solvents.
  • The solvent is always a gas.
  • A solution is a homogeneous mixture of substances. (correct)
  • Solutes alter their chemical identity when dissolved.

    • Which factor is likely to influence solubility?

    <p>The size of the solute particles</p> Signup and view all the answers

    Which of the following correctly identifies a solute?

    <p>A component present in a lesser amount</p> Signup and view all the answers

    What happens to a solute when it dissolves in a solvent?

    <p>It retains its chemical identity while becoming part of the solution.</p> Signup and view all the answers

    The term 'homogeneous mixture' most closely describes which characteristic?

    <p>All components are uniform and indistinguishable.</p> Signup and view all the answers

    Which scenario would likely decrease the solubility of a solute in a solvent?

    <p>Decreasing the surface area of the solute</p> Signup and view all the answers

    How does temperature generally affect the solubility of solids in water?

    <p>Increases solubility with increasing temperature</p> Signup and view all the answers

    What is the effect of pressure on the solubility of solids and liquids in water?

    <p>Pressure has little effect on solubility</p> Signup and view all the answers

    How does temperature affect the solubility of gases in water?

    <p>Decreases solubility with increasing temperature</p> Signup and view all the answers

    According to Henry's Law, what happens to the amount of gas dissolved in a liquid if the partial pressure of that gas is increased?

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

    What is primarily true about the solubility of gases compared to that of solids?

    <p>Gas solubility is significantly affected by temperature and pressure</p> Signup and view all the answers

    Which of the following best describes the relationship between partial pressure and gas solubility as indicated by Henry's Law?

    <p>Direct relationship</p> Signup and view all the answers

    What effect does increasing temperature have on the solubility of most solids in water?

    <p>It enhances solubility</p> Signup and view all the answers

    Which statement regarding solubility changes with pressure is correct?

    <p>Pressure significantly affects the solubility of gases</p> Signup and view all the answers

    What is defined as a solution in which water is the solvent?

    <p>Aqueous solution</p> Signup and view all the answers

    Which interparticle attraction must be overcome for a solute to dissolve in a solvent?

    <p>Attractions between solute–solute particles</p> Signup and view all the answers

    What generally happens when there is a greater difference in solute–solvent polarity?

    <p>The solute is less likely to dissolve</p> Signup and view all the answers

    What does the phrase 'like dissolves like' imply about solubility?

    <p>Similar polarities enhance solubility</p> Signup and view all the answers

    Which of the following is NOT a method for expressing concentration?

    <p>Mass concentration</p> Signup and view all the answers

    What type of attraction arises from solute and solvent interacting?

    <p>Solute–solvent attraction</p> Signup and view all the answers

    In which situation would you expect a solute to be less soluble?

    <p>When the solute and solvent are of different polarities</p> Signup and view all the answers

    What concept does the term 'percent concentration' refer to?

    <p>The amount of solute in a specified amount of solution</p> Signup and view all the answers

    What defines an unsaturated solution?

    <p>It contains less than the maximum amount of solute that can be dissolved.</p> Signup and view all the answers

    Which statement accurately describes a saturated solution?

    <p>It contains the maximum amount of solute that can be dissolved.</p> Signup and view all the answers

    What is a characteristic of a supersaturated solution?

    <p>It temporarily contains more dissolved solute than that present in a saturated solution.</p> Signup and view all the answers

    How is a concentrated solution defined?

    <p>It contains a large amount of solute relative to the amount that could dissolve.</p> Signup and view all the answers

    What is the primary difference between a concentrated solution and a dilute solution?

    <p>A concentrated solution has a larger amount of solute relative to what could dissolve.</p> Signup and view all the answers

    What occurs over time in a supersaturated solution?

    <p>Excess solute will crystallize out, leading to saturation.</p> Signup and view all the answers

    Which of the following solutions is considered most commonly encountered?

    <p>Unsaturated solutions are the most common type of solution.</p> Signup and view all the answers

    In which scenario would you typically find a concentrated solution?

    <p>In scenarios where a large amount of solute is present relative to the solvent.</p> Signup and view all the answers

    How many grams of sodium chloride are required to create 150 mL of a 0.9% (m/v) solution?

    <p>1.35 g</p> Signup and view all the answers

    What is the molarity of a solution containing 1.00 mol of sugar in 125.0 mL?

    <p>8.0 M</p> Signup and view all the answers

    If you have a 10.0 M sugar solution, what volume do you need to obtain 2.00 mol of sugar?

    <p>0.2 L</p> Signup and view all the answers

    What is the formula for calculating molarity?

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

    How would you express a 0.9% (m/v) solution in terms of grams per 100 mL?

    <p>0.9 g</p> Signup and view all the answers

    Which of the following statements is true regarding a 10.0 M solution?

    <p>It contains 10 moles of solute in 1000 mL.</p> Signup and view all the answers

    What is the effect of increasing the volume of solvent on the molarity of a solution?

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

    What would be the molarity of 0.5 mol of sodium chloride dissolved in 250 mL?

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

    What is the definition of dilution?

    <p>The process of adding more solvent to a solution to lower its concentration.</p> Signup and view all the answers

    To prepare a 100 mL of 0.9% saline solution from a 10% saline solution, which combination is correct?

    <p>9 mL of 10% saline solution + 91 mL of water</p> Signup and view all the answers

    Which action would decrease the concentration of a 0.50 M sodium chloride solution?

    <p>Add water to the solution.</p> Signup and view all the answers

    Using the dilution formula, Cs × Vs = Cd × Vd, what do 'Cs' and 'Vs' represent?

    <p>Concentration and volume of the stock solution.</p> Signup and view all the answers

    How can you calculate the minimum volume of a 2.00 M NaOH solution needed to make 150.0 mL of a 0.800 M NaOH solution?

    <p>Using the formula Cs × Vs = Cd × Vd.</p> Signup and view all the answers

    When diluting solutions, which factor must remain consistent to ensure accuracy?

    <p>The initial concentration of the solute.</p> Signup and view all the answers

    In what scenario would the concentration of a salt solution increase?

    <p>Adding more sodium chloride to the solution.</p> Signup and view all the answers

    If 60.0 mL of a 2.00 M NaOH solution is used to make a 0.800 M solution, what will be the total volume of the resulting solution?

    <p>150.0 mL</p> Signup and view all the answers

    Study Notes

    • Solutions are homogeneous mixtures of two or more substances, where each substance retains its own chemical identity.
    • A solution comprises a solvent (the component present in the greatest amount) and a solute (the component present in a lesser amount).
    • Solubility is the maximum amount of solute that can dissolve in a given amount of solvent under specific conditions.
    • Solubility of solids generally increases with temperature, while gas solubility decreases with temperature.
    • Pressure has little effect on the solubility of solids and liquids in water, but significantly impacts the solubility of gases (Henry's Law). The solubility of a gas is directly proportional to the partial pressure of the gas above the liquid.
    • Solutions can be unsaturated (more solute can dissolve), saturated (no more solute can dissolve), or supersaturated (more solute is dissolved than should be possible at the given conditions).
    • Concentrated solutions contain a large amount of solute relative to the amount that could dissolve, while dilute solutions contain a small amount of solute relative to the maximum possible amount in a given amount of solvent.
    • Aqueous solutions have water as the solvent, while non-aqueous solutions have a solvent other than water.
    • For a solute to dissolve in a solvent, two types of interparticle attractions must be broken: solute-solute and solvent-solvent attractions. A new type of attraction, solute-solvent, forms.
    • "Like dissolves like" is a general rule—substances with similar polarities tend to be more soluble in each other.
    • Concentration can be expressed using different units: percent concentration (by mass, by volume, or mass-volume), molarity, and molality.
    • Molarity is the moles of solute per liter of solution, while molality is the moles of solute per kilogram of solvent.
    • Dilutions involve adding more solvent to a solution to decrease its concentration.
    • Osmolarity is a measure of osmotic pressure based on the number of solute particles in a solution.
    • Osmosis is the movement of solvent (like water) across a semi-permeable membrane from a region of higher solvent concentration to a region of lower solvent concentration.
    • Osmotic pressure is the pressure required to prevent osmosis across a semipermeable membrane.
    • Tonicity refers to the ability of an extracellular solution to cause water movement into or out of a cell. There are three types of tonicity: hypotonic (lower solute concentration than the cell), hypertonic (higher solute concentration than the cell), and isotonic (equal solute concentration to the cell).
    • IV fluid types are an example of isotonic, hypertonic or hypotonic solutions.

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    Description

    Test your knowledge on solutions and solubility concepts in chemistry. This quiz covers topics such as solute and solvent interactions, factors affecting solubility, and the impact of temperature and pressure. Perfect for students looking to reinforce their understanding of solution chemistry.

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