45 Questions
What is a solution?
A homogeneous mixture of two or more pure substances
What drives the dissolution process when a solid dissolves into a liquid?
Increase in temperature
Why do we need to understand water as a medium and how drugs behave in aqueous solutions?
Because all reactions in the body occur in aqueous solutions
What are weak acids or bases called when they dissociate partially into ions when dissolved in water?
Ionized drugs
What type of intermolecular force is involved when ions are surrounded by water molecules?
Dipole-dipole interaction
What does the solubility constant, $K_s$, determine in a solution?
The equilibrium in a solution
What does the common ion effect, based on Le Chatelier's principle, state?
Adding ions will affect the equilibrium constant
What is the autoprotolysis constant of water, Kw, equal to?
$10^{-14}$
What does the pH scale measure?
Acidity or basicity of a solution
What can a buffer solution withstand without much change in pH?
Small additions of acid or base
What does the Henderson-Hasselbalch equation relate?
pH, pKa, and ionization
What determines the ratio of [A-] to [HA] in a solution according to the Henderson-Hasselbalch equation?
pH and pKa values
What type of substances tend to dissolve in nonpolar solvents according to the axiom 'like dissolves like'?
Nonpolar substances
What determines whether a solution is unsaturated or saturated?
Degree of saturation
What occurs with each interaction broken or formed during the process of dissolving an ionic solid in water?
Enthalpy changes (∆H)
What generally happens to the solubility of solid solutes in liquid solvents with increasing temperature?
Increases
What is the term for the extent of ionization of a weak acid or base at different pH values?
Henderson-Hasselbalch equation
What is the term for the homogeneous mixtures of two or more pure substances?
Solution
What drives the dissolution process when a solid dissolves into a liquid?
Increase in entropy
What determines the ratio of [A-] to [HA] in a solution according to the Henderson-Hasselbalch equation?
$K_a$ (acid dissociation constant)
What is the term for the equilibrium term between solid and saturated solution?
Solubility
What does the solubility constant, $K_s$, determine in a solution?
Maximum solute concentration
What does the Henderson-Hasselbalch equation relate?
$pH$ and $pKa$
What is the autoprotolysis constant of water, $K_w$, equal to?
$10^{-14}$
What generally happens to the solubility of solid solutes in liquid solvents with increasing temperature?
Increases
What drives the dissolution process when a solid dissolves into a liquid?
$ riangle H$ and $ riangle S$
What does the common ion effect, based on Le Chatelier's principle, state?
Addition of ions affects equilibrium position.
What type of intermolecular force is involved when ions are surrounded by water molecules?
Dipole-dipole interaction
What determines whether a solution is unsaturated or saturated?
Degree of saturation
What does the pH scale measure?
Acidity or basicity of a solution
What is the term for the homogeneous mixtures of two or more pure substances?
Solution
What occurs with each interaction broken or formed during the process of dissolving an ionic solid in water?
Enthalpy changes
What drives the dissolution process when a solid dissolves into a liquid?
Decrease in enthalpy and increase in entropy
What determines the extent of ionization of a weak acid or base at different pH values?
Henderson-Hasselbalch equation
What is the term for the equilibrium term between solid and saturated solution?
$K_s$ (solubility constant)
What does the common ion effect, based on Le Chatelier's principle, state?
It reduces the solubility of a slightly soluble salt when a common ion is added.
What is the term for the equilibrium term between solid and saturated solution?
Solubility
What is the autoprotolysis constant of water, $K_w$, equal to?
$10^{-14}$
What type of substances tend to dissolve in nonpolar solvents according to the axiom 'like dissolves like'?
Nonpolar substances
What generally happens to the solubility of solid solutes in liquid solvents with increasing temperature?
Increases
What does the common ion effect, based on Le Chatelier's principle, state?
Adding ions will affect the equilibrium constant
What drives the dissolution process when a solid dissolves into a liquid?
$\text{Free energy changes} (\triangle G)$
What determines whether a solution is unsaturated or saturated?
The degree of saturation
What does the solubility constant, $K_s$, determine in a solution?
The maximum amount of solute that can dissolve at a specific temperature
What occurs with each interaction broken or formed during the process of dissolving an ionic solid in water?
Free energy changes ($\triangle G$)
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.
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.
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