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Questions and Answers
What is a solution?
What is a solution?
What drives the dissolution process when a solid dissolves into a liquid?
What drives the dissolution process when a solid dissolves into a liquid?
Why do we need to understand water as a medium and how drugs behave in aqueous solutions?
Why do we need to understand water as a medium and how drugs behave in aqueous solutions?
What are weak acids or bases called when they dissociate partially into ions when dissolved in water?
What are weak acids or bases called when they dissociate partially into ions when dissolved in water?
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What type of intermolecular force is involved when ions are surrounded by water molecules?
What type of intermolecular force is involved when ions are surrounded by water molecules?
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What does the solubility constant, $K_s$, determine in a solution?
What does the solubility constant, $K_s$, determine in a solution?
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What does the common ion effect, based on Le Chatelier's principle, state?
What does the common ion effect, based on Le Chatelier's principle, state?
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What is the autoprotolysis constant of water, Kw, equal to?
What is the autoprotolysis constant of water, Kw, equal to?
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What does the pH scale measure?
What does the pH scale measure?
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What can a buffer solution withstand without much change in pH?
What can a buffer solution withstand without much change in pH?
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What does the Henderson-Hasselbalch equation relate?
What does the Henderson-Hasselbalch equation relate?
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What determines the ratio of [A-] to [HA] in a solution according to the Henderson-Hasselbalch equation?
What determines the ratio of [A-] to [HA] in a solution according to the Henderson-Hasselbalch equation?
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What type of substances tend to dissolve in nonpolar solvents according to the axiom 'like dissolves like'?
What type of substances tend to dissolve in nonpolar solvents according to the axiom 'like dissolves like'?
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What determines whether a solution is unsaturated or saturated?
What determines whether a solution is unsaturated or saturated?
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What occurs with each interaction broken or formed during the process of dissolving an ionic solid in water?
What occurs with each interaction broken or formed during the process of dissolving an ionic solid in water?
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What generally happens to the solubility of solid solutes in liquid solvents with increasing temperature?
What generally happens to the solubility of solid solutes in liquid solvents with increasing temperature?
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What is the term for the extent of ionization of a weak acid or base at different pH values?
What is the term for the extent of ionization of a weak acid or base at different pH values?
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What is the term for the homogeneous mixtures of two or more pure substances?
What is the term for the homogeneous mixtures of two or more pure substances?
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What drives the dissolution process when a solid dissolves into a liquid?
What drives the dissolution process when a solid dissolves into a liquid?
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What determines the ratio of [A-] to [HA] in a solution according to the Henderson-Hasselbalch equation?
What determines the ratio of [A-] to [HA] in a solution according to the Henderson-Hasselbalch equation?
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What is the term for the equilibrium term between solid and saturated solution?
What is the term for the equilibrium term between solid and saturated solution?
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What does the solubility constant, $K_s$, determine in a solution?
What does the solubility constant, $K_s$, determine in a solution?
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What does the Henderson-Hasselbalch equation relate?
What does the Henderson-Hasselbalch equation relate?
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What is the autoprotolysis constant of water, $K_w$, equal to?
What is the autoprotolysis constant of water, $K_w$, equal to?
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What generally happens to the solubility of solid solutes in liquid solvents with increasing temperature?
What generally happens to the solubility of solid solutes in liquid solvents with increasing temperature?
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What drives the dissolution process when a solid dissolves into a liquid?
What drives the dissolution process when a solid dissolves into a liquid?
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What does the common ion effect, based on Le Chatelier's principle, state?
What does the common ion effect, based on Le Chatelier's principle, state?
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What type of intermolecular force is involved when ions are surrounded by water molecules?
What type of intermolecular force is involved when ions are surrounded by water molecules?
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What determines whether a solution is unsaturated or saturated?
What determines whether a solution is unsaturated or saturated?
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What does the pH scale measure?
What does the pH scale measure?
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What is the term for the homogeneous mixtures of two or more pure substances?
What is the term for the homogeneous mixtures of two or more pure substances?
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What occurs with each interaction broken or formed during the process of dissolving an ionic solid in water?
What occurs with each interaction broken or formed during the process of dissolving an ionic solid in water?
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What drives the dissolution process when a solid dissolves into a liquid?
What drives the dissolution process when a solid dissolves into a liquid?
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What determines the extent of ionization of a weak acid or base at different pH values?
What determines the extent of ionization of a weak acid or base at different pH values?
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What is the term for the equilibrium term between solid and saturated solution?
What is the term for the equilibrium term between solid and saturated solution?
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What does the common ion effect, based on Le Chatelier's principle, state?
What does the common ion effect, based on Le Chatelier's principle, state?
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What is the term for the equilibrium term between solid and saturated solution?
What is the term for the equilibrium term between solid and saturated solution?
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What is the autoprotolysis constant of water, $K_w$, equal to?
What is the autoprotolysis constant of water, $K_w$, equal to?
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What type of substances tend to dissolve in nonpolar solvents according to the axiom 'like dissolves like'?
What type of substances tend to dissolve in nonpolar solvents according to the axiom 'like dissolves like'?
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What generally happens to the solubility of solid solutes in liquid solvents with increasing temperature?
What generally happens to the solubility of solid solutes in liquid solvents with increasing temperature?
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What does the common ion effect, based on Le Chatelier's principle, state?
What does the common ion effect, based on Le Chatelier's principle, state?
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What drives the dissolution process when a solid dissolves into a liquid?
What drives the dissolution process when a solid dissolves into a liquid?
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What determines whether a solution is unsaturated or saturated?
What determines whether a solution is unsaturated or saturated?
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What does the solubility constant, $K_s$, determine in a solution?
What does the solubility constant, $K_s$, determine in a solution?
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What occurs with each interaction broken or formed during the process of dissolving an ionic solid in water?
What occurs with each interaction broken or formed during the process of dissolving an ionic solid in water?
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Study Notes
Solubility and Dissociation in Chemistry
- Solvent molecules are attracted to surface ions, and each ion is surrounded by solvent molecules.
- Enthalpy changes (∆H) occur with each interaction broken or formed during the process of dissolving an ionic solid in water.
- The ions are solvated when surrounded by solvent, and if the solvent is water, the ions are hydrated, with ion-dipole intermolecular force.
- The enthalpy of solution, DHsoln, can be positive or negative and is only one side of the story (entropy).
- The degree of saturation determines whether a solution is unsaturated or saturated, and solubility is an equilibrium term between solid and saturated solution.
- For dissolution to happen, chemists use the axiom “like dissolves like,” where polar substances tend to dissolve in polar solvents and nonpolar substances tend to dissolve in nonpolar solvents.
- The solubility constant, Ks, is used to determine the equilibrium in a solution, and generally, the solubility of solid solutes in liquid solvents increases with increasing temperature.
- The common ion effect, based on Le Chatelier's principle, states that adding ions will affect the equilibrium constant.
- Water dissociates into ions, and the autoprotolysis constant of water is Kw = 10^-14.
- The pH scale measures the acidity or basicity of a solution, and a buffer solution can withstand small additions of acid or base without much change in pH.
- The dissociation of acids and bases is governed by equilibrium constants, and the Henderson-Hasselbalch equation relates pH, pKa, and ionization.
- The ratio of [A-] to [HA] in a solution can be determined using the Henderson-Hasselbalch equation, with practical applications in pharmaceuticals.
Solubility and Dissociation in Chemistry
- Solvent molecules are attracted to surface ions, and each ion is surrounded by solvent molecules.
- Enthalpy changes (∆H) occur with each interaction broken or formed during the process of dissolving an ionic solid in water.
- The ions are solvated when surrounded by solvent, and if the solvent is water, the ions are hydrated, with ion-dipole intermolecular force.
- The enthalpy of solution, DHsoln, can be positive or negative and is only one side of the story (entropy).
- The degree of saturation determines whether a solution is unsaturated or saturated, and solubility is an equilibrium term between solid and saturated solution.
- For dissolution to happen, chemists use the axiom “like dissolves like,” where polar substances tend to dissolve in polar solvents and nonpolar substances tend to dissolve in nonpolar solvents.
- The solubility constant, Ks, is used to determine the equilibrium in a solution, and generally, the solubility of solid solutes in liquid solvents increases with increasing temperature.
- The common ion effect, based on Le Chatelier's principle, states that adding ions will affect the equilibrium constant.
- Water dissociates into ions, and the autoprotolysis constant of water is Kw = 10^-14.
- The pH scale measures the acidity or basicity of a solution, and a buffer solution can withstand small additions of acid or base without much change in pH.
- The dissociation of acids and bases is governed by equilibrium constants, and the Henderson-Hasselbalch equation relates pH, pKa, and ionization.
- The ratio of [A-] to [HA] in a solution can be determined using the Henderson-Hasselbalch equation, with practical applications in pharmaceuticals.
Solubility and Dissociation in Chemistry
- Solvent molecules are attracted to surface ions, and each ion is surrounded by solvent molecules.
- Enthalpy changes (∆H) occur with each interaction broken or formed during the process of dissolving an ionic solid in water.
- The ions are solvated when surrounded by solvent, and if the solvent is water, the ions are hydrated, with ion-dipole intermolecular force.
- The enthalpy of solution, DHsoln, can be positive or negative and is only one side of the story (entropy).
- The degree of saturation determines whether a solution is unsaturated or saturated, and solubility is an equilibrium term between solid and saturated solution.
- For dissolution to happen, chemists use the axiom “like dissolves like,” where polar substances tend to dissolve in polar solvents and nonpolar substances tend to dissolve in nonpolar solvents.
- The solubility constant, Ks, is used to determine the equilibrium in a solution, and generally, the solubility of solid solutes in liquid solvents increases with increasing temperature.
- The common ion effect, based on Le Chatelier's principle, states that adding ions will affect the equilibrium constant.
- Water dissociates into ions, and the autoprotolysis constant of water is Kw = 10^-14.
- The pH scale measures the acidity or basicity of a solution, and a buffer solution can withstand small additions of acid or base without much change in pH.
- The dissociation of acids and bases is governed by equilibrium constants, and the Henderson-Hasselbalch equation relates pH, pKa, and ionization.
- The ratio of [A-] to [HA] in a solution can be determined using the Henderson-Hasselbalch equation, with practical applications in pharmaceuticals.
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Description
This quiz covers definitions related to solutions, solubility, solubility constant, common ion effect, pKw, Ka, Kb, pH, pOH, Henderson-Hasselbalch equation, ionization of weak acids and bases, and buffer solutions.
