Characteristics of Solutions and Solubility
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Questions and Answers

What generally happens to the solubility of solids in water as temperature increases?

  • Solubility increases (correct)
  • Solubility decreases
  • Solubility remains constant
  • Solubility fluctuates randomly

How does the temperature affect the solubility of gases in water?

  • Has no impact
  • Increases with temperature
  • Decreases with temperature (correct)
  • Fluctuates with pressure changes

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

  • Pressure has a variable effect depending on the substance
  • Pressure significantly increases solubility
  • Pressure has a minimal effect on solubility (correct)
  • Pressure decreases solubility

What does Henry's Law state about gas solubility in a liquid?

<p>Solubility is directly proportional to the partial pressure of the gas (B)</p> Signup and view all the answers

What happens to the solubility of gases when their pressure above the liquid is increased?

<p>Solubility increases (D)</p> Signup and view all the answers

Which of the following statements is NOT true regarding the effect of temperature on solubility?

<p>All solids are soluble at any temperature (A)</p> Signup and view all the answers

Which type of compounds does pressure primarily affect in terms of solubility?

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

Which of the following is true regarding the effect of temperature and pressure on solubility?

<p>Gas solubility decreases with temperature, but increases with pressure (A)</p> Signup and view all the answers

What describes osmosis accurately?

<p>Water moves from high concentration of water to low concentration of water. (D)</p> Signup and view all the answers

What is osmotic pressure?

<p>The pressure required to stop water flow from higher to lower solute concentration. (D)</p> Signup and view all the answers

Which of the following best characterizes tonicity?

<p>The ability of a solution to change cell volume by affecting water movement. (C)</p> Signup and view all the answers

In which type of solution does water move into a cell?

<p>Hypotonic solution (C)</p> Signup and view all the answers

What outcome occurs in a hypertonic solution?

<p>Water moves out of the cell, causing it to shrink. (C)</p> Signup and view all the answers

Which statement correctly describes the direction of water movement during osmosis?

<p>Water moves toward regions of higher solute concentration. (A)</p> Signup and view all the answers

What is the primary factor influencing the net flow of solvent during osmosis?

<p>The concentration gradient of solute. (A)</p> Signup and view all the answers

How does a semipermeable membrane function in osmosis?

<p>It allows only certain sizes of molecules to pass through. (D)</p> Signup and view all the answers

What is the formula for calculating percent by mass concentration?

<p>mass of solute × 100 / mass of solution (D)</p> Signup and view all the answers

If a solution has a mass percent concentration of 10%, how much solute is present in 100 g of solution?

<p>10 g of solute (C)</p> Signup and view all the answers

What components make up the mass of a solution?

<p>The solute and solvent combined (D)</p> Signup and view all the answers

In a solution with 5.5 g of glucose and 78.2 g of water, what is the total mass of the solution?

<p>83.7 g (B)</p> Signup and view all the answers

How would you describe a mass–volume percent concentration?

<p>It represents the mass of solute per unit volume of solution. (B)</p> Signup and view all the answers

What is the correct amount of sodium hydroxide to prepare 200 mL of a 0.8 M solution?

<p>64 g (D)</p> Signup and view all the answers

What does a mass percent concentration of 10% imply regarding the solute and solvent mass?

<p>The solute makes up 10% of the total solution mass. (B)</p> Signup and view all the answers

Identify the solute and solvent in a solution made by dissolving sodium hydroxide in water.

<p>The solute is sodium hydroxide, and the solvent is water. (A)</p> Signup and view all the answers

What is the molar mass of sodium hydroxide used to calculate the solution's concentration?

<p>40 g/mole (D)</p> Signup and view all the answers

In the context of percent concentrations, which statement is false?

<p>Solvent is sometimes included in calculating mass percent. (D)</p> Signup and view all the answers

What is the percent by mass concentration of glucose in the solution with 5.5 g of glucose dissolved in 78.2 g of water?

<p>6.6% (A)</p> Signup and view all the answers

Which option incorrectly states the amount of sodium hydroxide required for the solution?

<p>6.4 g of sodium hydroxide is needed. (B), 32 g of sodium hydroxide is needed. (C)</p> Signup and view all the answers

If one wanted to prepare a 1.6 M solution, how would the amount of sodium hydroxide change?

<p>It would double to 128 g. (B)</p> Signup and view all the answers

How is the relationship between moles, volume, and molarity expressed mathematically?

<p>Molarity = moles / volume. (D)</p> Signup and view all the answers

What is the primary purpose of adding solvent to a solution during the dilution process?

<p>To lower the concentration of the solution (C)</p> Signup and view all the answers

What would happen if 64 g of sodium hydroxide were added to 300 mL of water instead of 200 mL?

<p>The molarity would decrease. (B)</p> Signup and view all the answers

Which equation correctly represents the dilution process?

<p>Cd × Vd = Cs × Vs (C)</p> Signup and view all the answers

Which option represents a molarity equation correctly?

<p>$M = \frac{moles}{liters}$ (B)</p> Signup and view all the answers

How would one prepare 100 mL of a 0.9% saline solution using a 10% saline solution?

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

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

<p>Pouring some of the solution down the sink (B), Adding water to the solution (C)</p> Signup and view all the answers

What is the minimum volume of a 2.00 M NaOH solution necessary to prepare 150.0 mL of a 0.800 M NaOH solution?

<p>60.0 mL (A)</p> Signup and view all the answers

What characterizes an unsaturated solution?

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

Which statement is true about a saturated solution?

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

What will happen if you leave a concentrated salt solution exposed to air for too long?

<p>The concentration will increase (C)</p> Signup and view all the answers

What defines a supersaturated solution?

<p>It is characterized by an unstable solute arrangement. (D)</p> Signup and view all the answers

If you want to decrease the concentration of an already diluted salt solution, what should you avoid doing?

<p>Adding more salt (D)</p> Signup and view all the answers

How does a concentrated solution differ from a dilute solution?

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

In a dilution calculation, if you know the concentration and volume of the stock solution, which variable do you need to determine for the diluted solution?

<p>The concentration of the diluted solution (D)</p> Signup and view all the answers

Which of the following describes a characteristic of a dilute solution?

<p>It is always unsaturated. (B)</p> Signup and view all the answers

What happens when a supersaturated solution is allowed to sit?

<p>It can form crystals as excess solute precipitates out. (A)</p> Signup and view all the answers

Which of the following best describes a key difference between saturated and unsaturated solutions?

<p>Saturated solutions contain maximum solute; unsaturated solutions contain less solute. (B)</p> Signup and view all the answers

If a solution is described as concentrated, which of the following might also be accurate?

<p>It has reached the threshold where additional solute cannot dissolve. (B)</p> Signup and view all the answers

Flashcards

Solubility of solids in water

The amount of solid that can dissolve in a given amount of water at a specific temperature.

Effect of Temperature on Solid Solubility

Most solids become more soluble in water as the temperature increases.

Solubility of gases in water

The amount of gas that can dissolve in a given amount of water at a specific temperature and pressure.

Effect of Temperature on Gas Solubility

Gas solubilities in water decrease as the temperature increases.

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Effect of Pressure on Solid/Liquid Solubility

Pressure has little effect on the solubility of solids and liquids in water.

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Effect of Pressure on Gas Solubility

Pressure has a major effect on the solubility of gases in water.

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Henry's Law

The amount of gas that dissolves in a liquid is directly proportional to the partial pressure of the gas above the liquid.

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Henry's Law in Practice

As the pressure of a gas above a liquid increases, the solubility of the gas increases, and vice versa.

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Dilution

Adding more solvent to a solution, decreasing its concentration.

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Dilution Equation

The formula used to calculate the volumes and concentrations of solutions before and after dilution. Cs × Vs = Cd × Vd

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What is the effect of dilution on concentration?

Dilution decreases the concentration of a solution by increasing the volume of the solvent.

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How to prepare a diluted solution?

Calculate the required volumes of the stock solution and solvent using the dilution equation and then mix them carefully.

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How to decrease the concentration of a salt solution?

Add water to the solution.

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What is the minimum volume of a stock solution needed for dilution?

Use the dilution equation to calculate the volume of the stock solution needed to achieve the desired concentration and volume of the diluted solution.

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How to prepare 100 mL of 0.9% saline solution from 10% saline solution?

Calculate the required volume of the 10% saline solution using the dilution equation and then add water to make the final volume 100 mL.

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What is the relationship between volume and concentration in dilution?

As volume increases, concentration decreases and vice versa. The product of concentration and volume remains constant.

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Unsaturated Solution

A solution that has room for more solute to dissolve. It contains less solute than the maximum possible at the given conditions.

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Saturated Solution

A solution that contains the maximum amount of solute that can dissolve at the given conditions. Any more solute added will not dissolve.

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Supersaturated Solution

A solution that has more solute dissolved than it normally can hold at the given conditions. This is very unstable and will eventually return to a saturated solution by crystallizing excess solute.

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Concentrated Solution

A solution with a relatively large amount of solute compared to the amount that could dissolve.

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Dilute Solution

A solution with a relatively small amount of solute compared to the amount that could dissolve.

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What's the main difference between a saturated and an unsaturated solution?

A saturated solution has reached its maximum solute capacity, while an unsaturated solution can still dissolve more solute.

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What's the key characteristic of a supersaturated solution?

It contains more dissolved solute than a saturated solution at the given conditions, making it unstable and likely to crystallize out excess solute.

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What's the difference between a concentrated and dilute solution?

A concentrated solution has a high amount of solute for the given volume while a dilute solution has a low amount of solute.

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Percent Concentration

A way to express the amount of solute present in a solution, often expressed as a percentage.

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Percent by Mass (m/m%)

The mass of solute divided by the total mass of the solution, multiplied by 100. It expresses the concentration in terms of grams of solute per 100 grams of solution.

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Mass of Solution

The total mass of the solution, which includes both the mass of the solute and the mass of the solvent.

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10% Solution

A solution that contains 10 grams of solute per 100 grams of solution.

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Calculate Percent by Mass

The formula is (mass of solute / mass of solution) * 100

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What is the percent by mass (m/m) concentration of glucose in a solution made by dissolving 5.5 g of glucose in 78.2 g of water?

To find the percent by mass, first calculate the mass of the solution: 5.5 g (glucose) + 78.2 g (water) = 83.7 g (solution). Then, apply the formula: (5.5 g / 83.7 g) * 100 = 6.56%. Therefore, the concentration is 6.56% by mass.

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Solute

The substance being dissolved in a solution. It's the component that gets mixed in.

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Solvent

The substance that dissolves the solute. It's the dominant component of the solution.

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Molarity

A measure of the concentration of a solution, defined as the number of moles of solute per liter of solution.

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How to prepare a solution

To make a solution with a specific molarity, you need to calculate the mass of solute required and dissolve it in a specific volume of solvent.

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What is a solution?

A homogeneous mixture that consists of a uniformly dissolved solute in a solvent.

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What is the formula for Molarity?

Molarity = moles of solute / liters of solution

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What are the units of Molarity?

Molarity is expressed in moles per liter (mol/L) or M.

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Osmosis

The movement of water across a semipermeable membrane from an area of high water concentration (low solute concentration) to an area of low water concentration (high solute concentration).

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Osmotic Pressure

The pressure that needs to be applied to a solution to prevent the inward flow of water across a semipermeable membrane. It's essentially the pressure required to stop osmosis.

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Hypotonic Solution

A solution with a lower solute concentration than the cell. Water moves into the cell, causing it to swell.

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Hypertonic Solution

A solution with a higher solute concentration than the cell. Water moves out of the cell, causing it to shrink.

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Isotonic Solution

A solution with the same solute concentration as the cell. There is no net movement of water across the membrane.

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Tonicity

The ability of a solution to cause water to move into or out of a cell by osmosis.

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What happens to a cell placed in a hypotonic solution?

The cell will swell as water moves into it from the solution, as the solution has a lower solute concentration than the cell.

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What happens to a cell placed in a hypertonic solution?

The cell will shrink as water moves out of it into the solution, as the solution has a higher solute concentration than the cell.

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Study Notes

Characteristics of Solutions

  • A solution is a homogeneous mixture of two or more substances.
  • Each substance in a solution retains its own chemical identity.
  • Components of a solution include:
    • Solvent: The component present in the greatest amount.
    • Solute: The component present in a lesser amount. The substance being dissolved in the solution.

Solubility

  • Solubility is the maximum amount of solute that will dissolve in a given amount of solvent under a given set of conditions.
  • Temperature affects solubility:
    • Most solids become more soluble in water with increasing temperature.
    • Gas solubility in water decreases with increasing temperature.
  • Pressure affects solubility:
    • Pressure has little effect on the solubility of solids and liquids
    • Pressure has a major effect on the solubility of gases
  • Henry's Law: The amount of gas that will dissolve in a liquid at a given temperature is directly proportional to the partial pressure of the gas above the liquid. As gas pressure increases, solubility increases

Types of Solutions

  • Unsaturated solutions: Contain less than the maximum amount of solute that can dissolve under the existing conditions.
  • Saturated solutions: Contain the maximum amount of solute that can dissolve under the existing conditions.
  • Supersaturated solutions: Contain more dissolved solute than is present in a saturated solution under the existing conditions. These are unstable.

Concentration Units

  • Percent concentration of a solution
    • Percentage by mass (m/m): (mass of solute/mass of solution) *100%
    • Percentage by volume (v/v): (volume of solute/volume of solution) *100%
    • Percentage by mass/volume (m/v): (mass of solute/volume of solution) *100%
  • Molarity: Moles of solute per liter of solution (M).
  • Molality: Moles of solute per kilogram of solvent (m)

Dilution

  • Dilution is the process of reducing the concentration of a solution by adding more solvent.
  • C₁V₁ = C₂V₂ (Molarity equation for dilution)

Osmosis

  • Osmosis is the movement of solvent (usually water) from a region of high solvent concentration to a region of low solvent concentration across a semipermeable membrane until equilibrium is reached.

  • A semipermeable membrane allows certain types of molecules to pass through it but prevents the passage of other types of molecules.

  • Osmotic Pressure: The pressure that must be applied to prevent the net flow of solvent through a semipermeable membrane from a solution of lower solute concentration to a solution of higher solute concentration.

Osmolarity

  • Osmolarity: is the product of a solution's molarity and the number of particles produced per formula unit. A measure of the total concentration of solute particles in a solution. This concentration is proportional to the osmotic pressure. (Osmolarity= Molarity X i, where i is the number of particles produced for each solute molecule).

Tonicity

  • Tonicity refers to the ability of a solution to cause a cell to gain or lose water.

    • Hypotonic solution: A solution with a lower concentration of solutes than inside the cell results in the cell gaining water.
    • Hypertonic solution: A solution with a higher concentration of solutes than inside the cell resulting in the cell losing water.
    • Isotonic solution: A solution with an equal concentration of solutes as inside the cell. Results in no net flow of water.

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Explore the key concepts of solutions and solubility in this quiz. Learn about the components of a solution, factors affecting solubility, and Henry's Law. Perfect for students looking to deepen their understanding of this fundamental chemistry topic.

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