Chemistry Quiz: Acid-Base Theories
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Questions and Answers

Which of the following best describes a Bronsted-Lowry acid?

  • Proton acceptor
  • Electron pair donor
  • Electron pair acceptor
  • Proton donor (correct)

How do weak electrolytes differ from strong electrolytes?

  • They produce no ions in solution.
  • They partially dissociate in solution. (correct)
  • They fully dissociate in solution.
  • They completely combine with water.

According to the Lewis definition, what function do Lewis bases serve?

  • Electron pair donor (correct)
  • Electron pair acceptor
  • Proton donor
  • Proton acceptor

Which of the following compounds is considered a strong electrolyte?

<p>Sodium hydroxide (NaOH) (B)</p> Signup and view all the answers

In the reaction NH3 + HCl → NH4+ + Cl−, what is identified as the Bronsted-Lowry base?

<p>NH3 (A)</p> Signup and view all the answers

What is the defining characteristic of a non-electrolyte?

<p>Does not produce ions in solution (D)</p> Signup and view all the answers

Which statement most accurately describes a Bronsted-Lowry base?

<p>Accepts protons from acids (D)</p> Signup and view all the answers

What do strong acids and bases have in common regarding their behavior in solution?

<p>Both create a high concentration of ions. (B)</p> Signup and view all the answers

What attracts the cation in water?

<p>The partially negative O (D)</p> Signup and view all the answers

What happens to the solubility of solids with increasing temperature?

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

How does pressure affect the solubility of gases in liquids?

<p>It increases solubility (A)</p> Signup and view all the answers

What characterizes a saturated solution?

<p>It contains as much dissolved solute as possible at a given temperature (A)</p> Signup and view all the answers

What is true about supersaturated solutions?

<p>They are unstable and can precipitate excess solute (A)</p> Signup and view all the answers

Which factor does NOT influence the rate of dissolution of a solid?

<p>Color of the solute (A)</p> Signup and view all the answers

What type of solution contains less solute than needed for saturation?

<p>Unsaturated solution (D)</p> Signup and view all the answers

What causes smaller crystals to dissolve faster than larger crystals?

<p>Larger surface to volume ratio (D)</p> Signup and view all the answers

What is the primary determinant of colligative properties in a solution?

<p>Concentration of the solute particles (A)</p> Signup and view all the answers

When diluting a solution, which statement is true?

<p>The quantity of solute remains unchanged. (D)</p> Signup and view all the answers

Which equation represents the relationship between volume and molarity during dilution?

<p>V1 × M1 = V2 × M2 (B)</p> Signup and view all the answers

What effect does stirring have on the solute in a solution?

<p>It eliminates the saturation at the surface of the solid (D)</p> Signup and view all the answers

What is the effect of nonvolatile solutes on the vapor pressure of a solution?

<p>Decreases the vapor pressure (C)</p> Signup and view all the answers

Which factor is most likely to increase the solubility of a solid in water?

<p>Grinding the solid to increase its surface area (C)</p> Signup and view all the answers

What is the molarity of a solution containing 5.85 g of NaCl in 200 mL of solution?

<p>0.50 M (D)</p> Signup and view all the answers

What does a concentrated solution contain?

<p>A relatively large amount of dissolved solute (D)</p> Signup and view all the answers

How does the boiling point of a solution compare to that of the pure solvent?

<p>It is higher than that of the pure solvent. (C)</p> Signup and view all the answers

What is defined as the product of the mole fraction of the solvent times the vapor pressure of the pure solvent?

<p>Vapor pressure of the solution (D)</p> Signup and view all the answers

How is molarity calculated?

<p>Moles of solute divided by the volume of the solution in liters (B)</p> Signup and view all the answers

What is the mass of NaCl required to prepare a 0.90 m/v % solution in 50 mL?

<p>1.80 g (A)</p> Signup and view all the answers

What is the mass percent of a solution made by dissolving 1.00 g of ethanol in 100.0 g of water?

<p>1.00% (B)</p> Signup and view all the answers

What is a dilute solution defined as?

<p>A solution with a relatively small amount of dissolved solute (B)</p> Signup and view all the answers

How would you calculate the mass percent of NaCl in a solution made by dissolving 50 g NaCl in 150 g H2O?

<p>Divide 50 g by 200 g and multiply by 100 (D)</p> Signup and view all the answers

If 200 mL of CH3CH2OH is contained in a solution that is 6.0 % by volume alcohol, what volume of the solution is needed?

<p>3,333 mL (D)</p> Signup and view all the answers

What does Psoln represent in the context of solutions?

<p>Observed vapor pressure of solution (B)</p> Signup and view all the answers

What is the significance of Raoult's Law in ideal solutions?

<p>It relates the vapor pressure of the solution to the mole fractions of its components. (A)</p> Signup and view all the answers

In the context of ideal solutions, what happens to the boiling point when a solute is dissolved?

<p>The boiling point is raised. (C)</p> Signup and view all the answers

Which equation represents the relationship between boiling point elevation and molality?

<p>Δtb = mKb (C)</p> Signup and view all the answers

For a solution to behave ideally, how do the vapor pressures of the components compare?

<p>The total vapor pressure must be less than the sum of the individual vapor pressures. (C)</p> Signup and view all the answers

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

<p>The freezing point is lowered. (B)</p> Signup and view all the answers

Given equal concentrations, which factor contributes most significantly to vapor pressure lowering in solutions?

<p>Nature of the solute-solvent interactions (B)</p> Signup and view all the answers

What is the typical effect of solute particles on the vapor pressure of a solution?

<p>They lower the vapor pressure of the solution. (C)</p> Signup and view all the answers

What is the normal freezing point of water?

<p>0.0°C (A)</p> Signup and view all the answers

What is the van’t Hoff factor for sodium chloride (NaCl) when it dissociates in solution?

<p>2 (B)</p> Signup and view all the answers

If the temperature of a solution increases, what happens to the freezing point?

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

What is the molar mass of the molecular solid glucose if 18.00 g dissolves in 150 g water to give a boiling point of 100.34°C?

<p>180.0 g/mol (A)</p> Signup and view all the answers

To freeze a solution at -10.0°F, which property is being manipulated?

<p>Freezing point depression (C)</p> Signup and view all the answers

What does the term 'osmotic pressure' refer to in relation to colligative properties?

<p>The pressure needed to stop the movement of solvent. (B)</p> Signup and view all the answers

When two solutions have the same osmotic pressure, what is the consequence?

<p>No osmosis will occur. (D)</p> Signup and view all the answers

Which of the following substances can form semipermeable membranes?

<p>Certain polymers (D)</p> Signup and view all the answers

Flashcards

Electrolyte

A substance that, when dissolved in a solvent, produces ions, allowing the solution to conduct electricity.

Strong Electrolyte

A substance that dissociates completely in solution, generating a high concentration of ions. Examples include strong acids, strong bases, and salts.

Weak Electrolyte

A substance that only partially dissociates in solution, generating fewer ions. Examples include weak acids and weak bases.

Non-Electrolyte

A substance that does not produce ions in solution, and thus, does not conduct electricity. Examples include sugars and alcohols.

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Brønsted-Lowry Acid

A substance that donates a proton (H+) in a chemical reaction.

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Brønsted-Lowry Base

A substance that accepts a proton (H+) in a chemical reaction.

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Lewis Acid

A substance that accepts an electron pair in a chemical reaction.

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Lewis Base

A substance that donates an electron pair in a chemical reaction.

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Cation attraction in water

The attraction between a cation and the partially negative oxygen atom in water.

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Anion attraction in water

The attraction between an anion and the partially positive hydrogen atoms in water.

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Solubility of solids and temperature

The solubility of most solids increases as the temperature increases.

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Solubility of gases and temperature

The solubility of all gases decreases as the temperature increases.

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Solubility of gases and pressure

The solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.

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Saturated solution

A solution that contains the maximum amount of solute that can dissolve at a given temperature.

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Unsaturated solution

A solution that contains less solute than the maximum amount that can dissolve at a given temperature.

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Supersaturated solution

A solution that contains more solute than the maximum amount that can dissolve at a given temperature. These solutions are unstable and excess solute will precipitate out upon disturbance.

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Surface Area and Dissolving

The process of dissolving a solid in a liquid is faster when the surface area of the solid is increased.

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Stirring and Dissolving

Stirring a solution helps to dissolve a solid by moving dissolved solute away from the surface, allowing more solvent to interact with the solid.

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Dilute Solution

A dilute solution contains a relatively small amount of dissolved solute.

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Concentrated Solution

A concentrated solution contains a relatively large amount of dissolved solute.

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Mass Percent Concentration

Mass percent is the mass of the solute divided by the total mass of the solution, multiplied by 100%.

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Volume Percent Concentration

Volume percent is the volume of the solute divided by the total volume of the solution, multiplied by 100%.

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Molarity (M)

Molarity is the moles of solute dissolved in 1 liter of solution.

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Temperature and Solubility

The solubility of a solid in a liquid is generally increased by increasing the temperature.

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What is a solution?

A solution is a homogeneous mixture of two or more substances. The substance present in the largest amount is called the solvent, and the other substances are called solutes.

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What is Molarity?

Molarity (M) is a unit of concentration that expresses the number of moles of solute per liter of solution.

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What is Molality?

Molality (m) is a unit of concentration that expresses the number of moles of solute per kilogram of solvent.

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What is Dilution?

The process of adding solvent to a concentrated solution to make a more dilute solution.

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What is a colligative property?

A property of a solution that depends only on the number of solute particles present, not on their identity.

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Why does a solution have a lower vapor pressure than the pure solvent?

The vapor pressure of a solution is lower than that of the pure solvent because the solute molecules interfere with the evaporation of the solvent molecules.

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Why does a solution have a higher boiling point than the pure solvent?

The boiling point of a solution is higher than that of the pure solvent because the solute molecules interfere with the vaporization of the solvent molecules.

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Why does a solution have a lower freezing point than the pure solvent?

The freezing point of a solution is lower than that of the pure solvent because the solute molecules interfere with the formation of the solvent's crystal lattice.

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Raoult's Law

The vapor pressure of a solution is directly proportional to the mole fraction of the solvent in the solution.

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Vapor pressure

A pressure exerted by a vapor in equilibrium with its condensed phase (liquid or solid).

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Ideal solution

A solution where the vapor pressure of the solution is equal to the predicted vapor pressure based on Raoult's Law.

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Total vapor pressure (PTOTAL)

The sum of the partial pressures of each component in a mixture.

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Vapor pressure of pure solvent (P°solv)

The vapor pressure of a pure solvent at a given temperature.

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Boiling Point Elevation (tb)

The change in boiling point of a solution compared to the pure solvent. It is directly proportional to the molality of the solution.

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Boiling point constant (Kb)

A constant specific to a solvent that relates the molality of a solution to its boiling point elevation.

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Mole fraction (χ)

The ratio of moles of a component in a mixture to the total moles of all components in the mixture.

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Freezing Point Depression

The change in freezing point of a solution is directly proportional to the molality of the solute. This change is calculated using the freezing point depression constant (Kf) for the solvent, which is a property specific to the solvent.

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Boiling Point Elevation

The change in boiling point of a solution is directly proportional to the molality of the solute. This change is calculated using the boiling point elevation constant (Kb) for the solvent, which is a property specific to the solvent.

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Van't Hoff Factor (i)

The van't Hoff factor (i) represents the number of particles a solute dissociates into when dissolved in a solvent. For example, NaCl dissociates into two particles (Na+ and Cl-), so i = 2 for NaCl.

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Colligative Property

A colligative property depends solely on the concentration of solute particles in a solution, not their specific identity. Examples include freezing point depression, boiling point elevation, osmotic pressure, and vapor pressure lowering.

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Osmosis

Osmosis is the movement of solvent molecules across a semipermeable membrane from a region of high solvent concentration (low solute concentration) to a region of low solvent concentration (high solute concentration).

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Osmotic Pressure

Osmotic pressure is the pressure that must be applied to a solution to prevent the inward flow of water across a semipermeable membrane. This pressure is directly proportional to the molar concentration of the solute.

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Semipermeable Membrane

A semipermeable membrane allows some particles to pass through while blocking others. This selectivity is based on size, charge, and other factors.

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Dialysis

Dialysis is a separation process in which a semipermeable membrane is used to separate molecules of different sizes. Smaller molecules can pass through the membrane, while larger molecules are retained.

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Study Notes

Solutions

  • Solutions are homogeneous mixtures of one or more solutes and a solvent.
  • A solute is the substance being dissolved.
  • A solvent is the dissolving agent, usually the most abundant substance.

Classification of Compounds

  • Organic Compounds: Compounds primarily consisting of carbon, excluding carbonates, cyanides, carbides, and oxides. Often derived from living organisms. Tend to be soluble in organic solvents and usually flammable. Structures are complex, often in chains or rings.

  • Inorganic Compounds: Compounds that do not primarily consist of carbon. Includes oxides, bases, acids, and salts. Often derived from minerals or non-living sources. Typically soluble in water (especially ionic compounds) and are not flammable. Structures are simple and often crystalline.

Acids, Bases, and Salts

  • Acids: Substances that taste sour, turn blue litmus paper red, and corrode metals, producing H2 gas.
  • Bases: Substances that taste bitter, turn red litmus paper blue, and have a slippery feel.
  • Salts: Formed when acids and bases react, neutralizing each other and producing a salt along with water.

Acid and Base Definitions

  • Arrhenius Definition: An acid produces H+ ions in aqueous solution; a base produces OH- ions. Free H+ ions don't exist alone in solution, they combine with water to form H3O+ ions. This theory assumes all bases contain OH-.

  • Brønsted-Lowry Definition: An acid is a proton donor, and a base is a proton acceptor. The product that gains an H+ is the conjugate acid of the base. The product that loses an H+ is the conjugate base of the acid.

  • Lewis Definition: A broader definition. An acid is an electron pair acceptor; a base is an electron pair donor.

Electrolytes

  • Electrolytes are substances that, when dissolved in water or other solvents, produce ions allowing the solution to conduct electricity.
  • Electrolytes are essential in both chemistry and biology for activities like conducting electrical signals and maintaining homeostasis.
  • Strong Electrolytes: Dissociate completely in solution, producing a high concentration of ions. Examples include strong acids (HCI, H2SO4), strong bases (NaOH, KOH), and most salts (NaCl, KNO3).
  • Weak Electrolytes: Partially dissociate in solution, producing fewer ions. Examples include weak acids (CH3COOH), and weak bases (NH3).
  • Non-Electrolytes: Do not produce ions in solution; therefore, they do not conduct electricity. Examples include sugars (glucose, sucrose) and alcohols (ethanol).

Nature of Solutions

  • Solutions are homogeneous mixtures of a solute and solvent.
  • The concentration of solute in a solution dictates how much solute dissolves.
  • What dissolves depends on characteristics of both solute and solvent.

Properties of a True Solution

  • A homogeneous mixture of two or more components.
  • A solute is molecular or ionic in size (less than 1 nm).
  • Generally colorless or transparent.
  • The solute will not separate out of the solution.
  • The solute can be separated from the solvent by physical methods.

Solubility

  • Solubility describes the amount of a substance that can dissolve in a specific amount of solvent at a particular temperature.
  • Miscible liquids dissolve in each other.
  • Immiscible liquids do not dissolve in each other.
  • Ionic compound solubility rules predict whether substances will dissolve.
  • "Like dissolves like": Polar substances dissolve in polar solvents; nonpolar substances dissolve in nonpolar solvents.
  • Temperature changes affect solubility of solids and gases differently.
  • Pressure affects the solubility of gases.
  • The rate of dissolving solids depends on the particle size, temperature, agitation, and concentration of the solution.

Saturated, Unsaturated, and Supersaturated Solutions

  • Saturated solution: Contains the maximum amount of a solute that can dissolve in a given amount of solvent at a particular temperature. It is in equilibrium with undissolved solute.
  • Unsaturated solution: Contains less solute than the maximum amount that can dissolve.
  • Supersaturated solution: Contains more solute than the maximum amount that can dissolve under normal conditions. The excess solute will precipitate out if conditions change (like temperature).

Concentration of Solutions

  • Qualitative: Dilute or concentrated solutions are described by how much solute is dissolved.
  • Quantitative: Various units are used to measure the specific concentration of a solution, such as mass percent, mass/volume percent, volume percent, molarity, and molality.

Solution Stoichiometry

  • Calculations to find specific amounts of reactants and products in solutions involving chemical reactions.

Dilution of Solutions

  • Adding a solvent to a concentrated solution makes it less concentrated (more dilute).
  • Moles of solute remain constant in a dilution.
  • V₁M₁ = V₂M₂ A key equation.

Colligative Properties of Solutions

  • Solution properties which depend only on the number of solute particles, not the type of solute.
  • Some colligative properties include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.

Osmotic Pressure

  • Pressure required to stop osmosis (the net movement of solvent from a lower to a higher concentration).
  • Osmotic pressure is a colligative property.
  • The formula relates osmotic pressure to molarity, the ideal gas constant, and temperature: π = iMRT

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Test your knowledge of Bronsted-Lowry and Lewis acid-base theories with this quiz. Explore the differences between strong and weak electrolytes, as well as the characteristics of non-electrolytes. Perfect for students preparing for exams in chemistry.

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