Composition of Mixtures - AP Chemistry
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What is the technique called that separates mixtures based on differences in density?
What is the technique called that separates mixtures based on differences in density?
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Centrifugation. High-speed spinning separates components by density differences.
Centrifugation. High-speed spinning separates components by density differences.
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What is the key distinction between a colloid and a true solution?
What is the key distinction between a colloid and a true solution?
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Colloids have larger particles than true solutions. Colloid particles are larger but still small enough to remain dispersed.
Colloids have larger particles than true solutions. Colloid particles are larger but still small enough to remain dispersed.
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Which law relates the solubility of a gas in a liquid to the pressure of the gas above the liquid?
Which law relates the solubility of a gas in a liquid to the pressure of the gas above the liquid?
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Henry's Law. Gas solubility is directly proportional to partial pressure above liquid.
Henry's Law. Gas solubility is directly proportional to partial pressure above liquid.
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What term is used for the maximum amount of solute that can dissolve in a solvent at a given temperature?
What term is used for the maximum amount of solute that can dissolve in a solvent at a given temperature?
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Saturated solution. Equilibrium state where no more solute can dissolve.
Saturated solution. Equilibrium state where no more solute can dissolve.
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What is the term for a solution with a pH greater than 7?
What is the term for a solution with a pH greater than 7?
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Basic (or alkaline) solution. Low hydrogen ion concentration creates basic conditions.
Basic (or alkaline) solution. Low hydrogen ion concentration creates basic conditions.
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Which term describes a mixture where particles are dispersed throughout but not dissolved?
Which term describes a mixture where particles are dispersed throughout but not dissolved?
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Colloid. Intermediate between solution and suspension with dispersed particles.
Colloid. Intermediate between solution and suspension with dispersed particles.
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How do you express parts per million (ppm) in terms of mass?
How do you express parts per million (ppm) in terms of mass?
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ppm = $\frac{\text{mass of solute}}{\text{mass of solution}} \times 10^6$. Expresses very small concentrations as parts per million by mass ratio.
ppm = $\frac{\text{mass of solute}}{\text{mass of solution}} \times 10^6$. Expresses very small concentrations as parts per million by mass ratio.
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What is the term for the layer that forms in a heterogeneous mixture of immiscible liquids?
What is the term for the layer that forms in a heterogeneous mixture of immiscible liquids?
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Interface. Boundary between two immiscible liquid phases in mixture.
Interface. Boundary between two immiscible liquid phases in mixture.
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Identify the principal distinction between a homogeneous and a heterogeneous mixture.
Identify the principal distinction between a homogeneous and a heterogeneous mixture.
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Homogeneous mixtures have uniform composition; heterogeneous do not. Homogeneous means uniform throughout; heterogeneous has visible distinct phases.
Homogeneous mixtures have uniform composition; heterogeneous do not. Homogeneous means uniform throughout; heterogeneous has visible distinct phases.
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Which process involves the separation of a mixture by passing it through a medium where components move at different rates?
Which process involves the separation of a mixture by passing it through a medium where components move at different rates?
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Chromatography. Components move through medium at different rates enabling separation.
Chromatography. Components move through medium at different rates enabling separation.
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Which term denotes the concentration of a solution in terms of mole fraction?
Which term denotes the concentration of a solution in terms of mole fraction?
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Mole fraction. Ratio of component moles to total moles in mixture.
Mole fraction. Ratio of component moles to total moles in mixture.
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Identify the property that describes how much solute can dissolve in a solvent at a given temperature.
Identify the property that describes how much solute can dissolve in a solvent at a given temperature.
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Solubility. Maximum amount of solute that dissolves at equilibrium conditions.
Solubility. Maximum amount of solute that dissolves at equilibrium conditions.
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What defines a solution with equal concentrations of solute and solvent on either side of a membrane?
What defines a solution with equal concentrations of solute and solvent on either side of a membrane?
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Isotonic solution. Equal solute concentrations prevent net water movement across membrane.
Isotonic solution. Equal solute concentrations prevent net water movement across membrane.
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What effect does the addition of a solute have on the vapor pressure of a solvent?
What effect does the addition of a solute have on the vapor pressure of a solvent?
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Vapor pressure reduction. Solute particles decrease vapor pressure below pure solvent value.
Vapor pressure reduction. Solute particles decrease vapor pressure below pure solvent value.
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What is the formula for parts per billion (ppb) in terms of mass?
What is the formula for parts per billion (ppb) in terms of mass?
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ppb = $\frac{\text{mass of solute}}{\text{mass of solution}} \times 10^9$. Even smaller concentrations expressed as parts per billion by mass.
ppb = $\frac{\text{mass of solute}}{\text{mass of solution}} \times 10^9$. Even smaller concentrations expressed as parts per billion by mass.
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What is the result of adding a non-volatile solute to a solvent in terms of boiling point?
What is the result of adding a non-volatile solute to a solvent in terms of boiling point?
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Boiling point elevation. Solute particles increase the boiling point above pure solvent.
Boiling point elevation. Solute particles increase the boiling point above pure solvent.
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What is the effect of increasing temperature on the solubility of gases in liquids?
What is the effect of increasing temperature on the solubility of gases in liquids?
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Solubility of gases decreases with increasing temperature. Higher temperature reduces gas-liquid attractive forces and solubility.
Solubility of gases decreases with increasing temperature. Higher temperature reduces gas-liquid attractive forces and solubility.
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What is the term for the process of separating a mixture into its components based on boiling points?
What is the term for the process of separating a mixture into its components based on boiling points?
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Distillation. Separation technique exploiting different boiling points of components.
Distillation. Separation technique exploiting different boiling points of components.
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What is the formula for molality of a solution?
What is the formula for molality of a solution?
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Molality = $\frac{\text{moles of solute}}{\text{kilograms of solvent}}$. Temperature-independent concentration based on solvent mass, not volume.
Molality = $\frac{\text{moles of solute}}{\text{kilograms of solvent}}$. Temperature-independent concentration based on solvent mass, not volume.
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What is a common method for separating a solid from a liquid in a heterogeneous mixture?
What is a common method for separating a solid from a liquid in a heterogeneous mixture?
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Filtration. Physical separation using porous barrier to retain solid particles.
Filtration. Physical separation using porous barrier to retain solid particles.
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Which type of mixture displays the Tyndall effect?
Which type of mixture displays the Tyndall effect?
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Colloid. Light scattering distinguishes colloids from true solutions.
Colloid. Light scattering distinguishes colloids from true solutions.
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How do you express parts per million (ppm) in terms of mass?
How do you express parts per million (ppm) in terms of mass?
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ppm = $\frac{\text{mass of solute}}{\text{mass of solution}} \times 10^6$. Expresses very small concentrations as parts per million by mass ratio.
ppm = $\frac{\text{mass of solute}}{\text{mass of solution}} \times 10^6$. Expresses very small concentrations as parts per million by mass ratio.
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What is the usual effect of pressure on the solubility of solids in liquids?
What is the usual effect of pressure on the solubility of solids in liquids?
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Little to no effect. Solid solubility typically independent of pressure changes.
Little to no effect. Solid solubility typically independent of pressure changes.
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What is the term for a solution that has a pH less than 7?
What is the term for a solution that has a pH less than 7?
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Acidic solution. High hydrogen ion concentration creates acidic conditions.
Acidic solution. High hydrogen ion concentration creates acidic conditions.
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Identify the effect of a solute on the freezing point of a solvent.
Identify the effect of a solute on the freezing point of a solvent.
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Freezing point depression. Solute particles lower the freezing point below pure solvent.
Freezing point depression. Solute particles lower the freezing point below pure solvent.
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Which technique uses a semi-permeable membrane to separate small particles from large ones?
Which technique uses a semi-permeable membrane to separate small particles from large ones?
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Dialysis. Membrane separation based on particle size differences.
Dialysis. Membrane separation based on particle size differences.
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Which rule determines the solubility of ionic compounds in water?
Which rule determines the solubility of ionic compounds in water?
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Solubility rules. Empirical guidelines that predict which ionic compounds dissolve in water.
Solubility rules. Empirical guidelines that predict which ionic compounds dissolve in water.
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What is the key feature of a suspension compared to a solution?
What is the key feature of a suspension compared to a solution?
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Particles in a suspension are larger and settle over time. Large particles settle due to gravity, unlike dissolved solutions.
Particles in a suspension are larger and settle over time. Large particles settle due to gravity, unlike dissolved solutions.
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What is the formula for calculating the mole fraction of a component in a mixture?
What is the formula for calculating the mole fraction of a component in a mixture?
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Mole fraction = $\frac{\text{moles of component}}{\text{total moles of all components}}$. Expresses relative amount of each component in molar terms.
Mole fraction = $\frac{\text{moles of component}}{\text{total moles of all components}}$. Expresses relative amount of each component in molar terms.
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What is the term for the layer that forms in a heterogeneous mixture of immiscible liquids?
What is the term for the layer that forms in a heterogeneous mixture of immiscible liquids?
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Interface. Boundary between two immiscible liquid phases in mixture.
Interface. Boundary between two immiscible liquid phases in mixture.
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