AP Chemistry Flashcards: Representations Of Solutions

What this deck covers

This deck focuses on Representations Of Solutions, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

Flashcard 1: What is Raoult's Law formula?

Answer: $P_A = X_A P^0_A$, where $P_A$ is vapor pressure of component $A$. Law relates vapor pressure to mole fraction in ideal solutions.

Flashcard 2: Identify the property of a colligative property.

Answer: Depends on the number of solute particles, not their identity. Properties determined by particle count, not chemical identity.

Flashcard 3: What is the effect of a solute on freezing point of a solution?

Answer: Lowers the freezing point. Solute particles interfere with crystal formation at normal freezing point.

Flashcard 4: What is an unsaturated solution?

Answer: A solution that can dissolve more solute at a given temperature. Solution can still accept additional solute below saturation point.

Flashcard 5: Find the new concentration after dilution: $M_1 = 6$, $V_1 = 1$, $V_2 = 3$.

Answer: New concentration is 2 M. Apply dilution equation: $6 \times 1 = M_2 \times 3$, so $M_2 = 2$.

Flashcard 6: What is a supersaturated solution?

Answer: A solution that contains more solute than can dissolve at the current temperature. Metastable state containing excess solute that can crystallize out.

Flashcard 7: What is the principle of Le Chatelier's?

Answer: System at equilibrium will adjust to counteract disturbances. Fundamental principle describing system response to external changes.

Flashcard 8: What is the definition of molarity?

Answer: Molarity is the number of moles of solute per liter of solution. This is the fundamental concentration unit relating solute amount to solution volume.

Flashcard 9: Find the new concentration after dilution: $M_1 = 6$, $V_1 = 1$, $V_2 = 3$.

Answer: New concentration is 2 M. Apply dilution equation: $6 \times 1 = M_2 \times 3$, so $M_2 = 2$.

Flashcard 10: Which equation represents the dilution of solutions?

Answer: $M_1V_1 = M_2V_2$, where $M$ is molarity and $V$ is volume. Conservation equation for dilutions where moles remain constant.

Flashcard 11: Which formula represents freezing point depression?

Answer: $\Delta T_f = iK_f m$, where $i$ is van't Hoff factor. Formula accounts for number of particles formed when solute dissolves.

Flashcard 12: What is osmotic pressure?

Answer: Pressure required to stop osmosis. External pressure needed to prevent solvent flow across membrane.

Flashcard 13: How is molality defined in a solution?

Answer: Molality is the number of moles of solute per kilogram of solvent. Uses solvent mass instead of solution volume, making it temperature-independent.

Flashcard 14: What is the effect of pressure on gas solubility in liquids?

Answer: Increased pressure increases gas solubility. Henry's Law: higher pressure forces more gas molecules into solution.

Flashcard 15: Find the new concentration after dilution: $M_1 = 6$, $V_1 = 1$, $V_2 = 3$.

Answer: New concentration is 2 M. Apply dilution equation: $6 \times 1 = M_2 \times 3$, so $M_2 = 2$.

Flashcard 16: Identify the property of a colligative property.

Answer: Depends on the number of solute particles, not their identity. Properties determined by particle count, not chemical identity.

Flashcard 17: Determine the freezing point depression: $i = 3$, $K_f = 1$, $m = 0.2$.

Answer: Freezing point depression is 0.6°C. Apply formula: $\Delta T_f = 3 \times 1 \times 0.2 = 0.6$.

Flashcard 18: What is the effect of a solute on boiling point of a solution?

Answer: Raises the boiling point. Solute particles disrupt solvent vaporization, requiring higher temperature.

Flashcard 19: What describes a hypotonic solution?

Answer: Solution with lower solute concentration than another. Comparative term indicating lesser solute concentration relative to reference.

Flashcard 20: What is the formula for calculating molality?

Answer: $m = \frac{n}{m_{\text{solvent}}}$, where $n$ is moles of solute and $m_{\text{solvent}}$ is kg of solvent. Formula uses kilograms of solvent in the denominator.

Flashcard 21: What is the principle of Le Chatelier's?

Answer: System at equilibrium will adjust to counteract disturbances. Fundamental principle describing system response to external changes.

Flashcard 22: How is molality defined in a solution?

Answer: Molality is the number of moles of solute per kilogram of solvent. Uses solvent mass instead of solution volume, making it temperature-independent.

Flashcard 23: What is the effect of pressure on gas solubility in liquids?

Answer: Increased pressure increases gas solubility. Henry's Law: higher pressure forces more gas molecules into solution.

Flashcard 24: What is a saturated solution?

Answer: A solution in which no more solute can dissolve at a given temperature. Maximum solubility reached at equilibrium for given conditions.

Flashcard 25: State Henry's Law formula.

Answer: $C = kP$, where $C$ is solubility and $P$ is pressure. Linear relationship where $k$ is Henry's law constant.

Flashcard 26: What is the formula for mole fraction?

Answer: $X_A = \frac{n_A}{n_{\text{total}}}$, where $n_A$ is moles of component $A$. Ratio formula where all mole fractions sum to 1.

Flashcard 27: How is molality defined in a solution?

Answer: Molality is the number of moles of solute per kilogram of solvent. Uses solvent mass instead of solution volume, making it temperature-independent.

Flashcard 28: Calculate osmotic pressure: $i = 1$, $M = 0.5$, $R = 0.0821$, $T = 300$.

Answer: Osmotic pressure is 12.315 atm. Apply formula: $\pi = 1 \times 0.5 \times 0.0821 \times 300$.

Flashcard 29: Which formula represents boiling point elevation?

Answer: $\Delta T_b = iK_b m$, where $i$ is van't Hoff factor. Formula includes van't Hoff factor for ionic dissociation effects.

Flashcard 30: What is Henry's Law?

Answer: Solubility of gas in liquid is proportional to the pressure of gas above the liquid. Direct proportionality between gas pressure and dissolution concentration.

Flashcard 31: Identify the property of a colligative property.

Answer: Depends on the number of solute particles, not their identity. Properties determined by particle count, not chemical identity.

Flashcard 32: What is the principle of Le Chatelier's?

Answer: System at equilibrium will adjust to counteract disturbances. Fundamental principle describing system response to external changes.

Flashcard 33: What is a saturated solution?

Answer: A solution in which no more solute can dissolve at a given temperature. Maximum solubility reached at equilibrium for given conditions.

Flashcard 34: Identify the property of a colligative property.

Answer: Depends on the number of solute particles, not their identity. Properties determined by particle count, not chemical identity.

Flashcard 35: Find the new concentration after dilution: $M_1 = 6$, $V_1 = 1$, $V_2 = 3$.

Answer: New concentration is 2 M. Apply dilution equation: $6 \times 1 = M_2 \times 3$, so $M_2 = 2$.

Flashcard 36: Determine the boiling point elevation: $i = 2$, $K_b = 0.5$, $m = 1$.

Answer: Boiling point elevation is 1°C. Apply formula: $\Delta T_b = 2 \times 0.5 \times 1 = 1$.

Flashcard 37: Determine the boiling point elevation: $i = 2$, $K_b = 0.5$, $m = 1$.

Answer: Boiling point elevation is 1°C. Apply formula: $\Delta T_b = 2 \times 0.5 \times 1 = 1$.

Flashcard 38: What describes an isotonic solution?

Answer: Solutions with equal solute concentrations. No net osmotic pressure difference exists between the solutions.

Flashcard 39: State the formula for calculating molarity.

Answer: $M = \frac{n}{V}$, where $n$ is moles of solute and $V$ is volume in liters. Standard formula relating moles of solute to liters of solution.

Flashcard 40: Define mole fraction.

Answer: Mole fraction is the ratio of moles of one component to the total moles in the mixture. Represents the fraction of total moles contributed by one component.

Flashcard 41: Determine the boiling point elevation: $i = 2$, $K_b = 0.5$, $m = 1$.

Answer: Boiling point elevation is 1°C. Apply formula: $\Delta T_b = 2 \times 0.5 \times 1 = 1$.

Flashcard 42: What is a saturated solution?

Answer: A solution in which no more solute can dissolve at a given temperature. Maximum solubility reached at equilibrium for given conditions.

Flashcard 43: What is the principle of Le Chatelier's?

Answer: System at equilibrium will adjust to counteract disturbances. Fundamental principle describing system response to external changes.

Flashcard 44: What happens to vapor pressure when a non-volatile solute is added?

Answer: Vapor pressure decreases. Raoult's Law: solute particles reduce solvent's tendency to vaporize.

Flashcard 45: What is the unit of molality?

Answer: Moles per kilogram (mol/kg). Units reflect moles of solute per mass of solvent.

Flashcard 46: Which formula represents freezing point depression?

Answer: $\Delta T_f = iK_f m$, where $i$ is van't Hoff factor. Formula accounts for number of particles formed when solute dissolves.

Flashcard 47: What is a saturated solution?

Answer: A solution in which no more solute can dissolve at a given temperature. Maximum solubility reached at equilibrium for given conditions.

Flashcard 48: How is molality defined in a solution?

Answer: Molality is the number of moles of solute per kilogram of solvent. Uses solvent mass instead of solution volume, making it temperature-independent.

Flashcard 49: Determine the boiling point elevation: $i = 2$, $K_b = 0.5$, $m = 1$.

Answer: Boiling point elevation is 1°C. Apply formula: $\Delta T_b = 2 \times 0.5 \times 1 = 1$.

Flashcard 50: Which formula represents freezing point depression?

Answer: $\Delta T_f = iK_f m$, where $i$ is van't Hoff factor. Formula accounts for number of particles formed when solute dissolves.

Flashcard 51: Identify the formula for percent mass.

Answer: Percent mass = $\frac{\text{mass of solute}}{\text{mass of solution}} \times 100\%$. Mass percentage formula multiplied by 100 for percentage.

Flashcard 52: Describe the common ion effect.

Answer: Decrease in solubility of an ionic compound by adding a common ion. Added common ions shift equilibrium, reducing compound solubility.

Flashcard 53: Which formula represents freezing point depression?

Answer: $\Delta T_f = iK_f m$, where $i$ is van't Hoff factor. Formula accounts for number of particles formed when solute dissolves.

Flashcard 54: What is the definition of molarity?

Answer: Molarity is the number of moles of solute per liter of solution. This is the fundamental concentration unit relating solute amount to solution volume.

Flashcard 55: Calculate molality: 3 moles solute in 2 kg solvent.

Answer: 1.5 mol/kg. Divide moles by solvent mass: $3 \div 2 = 1.5$.

Flashcard 56: How do you calculate the van't Hoff factor, $i$?

Answer: $i$ is the number of particles the solute dissociates into. Represents degree of dissociation for ionic compounds in solution.

Flashcard 57: What describes a hypertonic solution?

Answer: Solution with higher solute concentration than another. Comparative term indicating greater solute concentration relative to reference.

Flashcard 58: Find the molarity: 2 moles solute in 4 L solution.

Answer: 0.5 mol/L. Divide moles by volume: $2 \div 4 = 0.5$.

Flashcard 59: What is the unit of molarity?

Answer: Moles per liter (mol/L). Standard SI unit for concentration in chemistry.

Flashcard 60: Identify the solution type: 1 M NaCl inside, 0.5 M NaCl outside.

Answer: Hypertonic inside, hypotonic outside. Higher concentration inside makes it hypertonic relative to outside.

Flashcard 61: What is the formula for osmotic pressure?

Answer: $\pi = iMRT$, where $\pi$ is osmotic pressure. Van't Hoff equation incorporating gas law principles for osmosis.

Flashcard 62: Compute the mole fraction: 2 moles $A$, 3 moles $B$.

Answer: Mole fraction of $A$ is 0.4. Divide component moles by total: $2 \div (2+3) = 0.4$.