Introduction to Solubility Equilibria - AP Chemistry
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How does $K_{sp}$ change with temperature for exothermic reactions?
How does $K_{sp}$ change with temperature for exothermic reactions?
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$K_{sp}$ decreases with temperature. Lower temperature favors exothermic dissolution process.
$K_{sp}$ decreases with temperature. Lower temperature favors exothermic dissolution process.
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Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.
Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.
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$K_{sp} = 4x^3$. Substitute equilibrium concentrations: $(2x)^2(x) = 4x^3$.
$K_{sp} = 4x^3$. Substitute equilibrium concentrations: $(2x)^2(x) = 4x^3$.
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How does $K_{sp}$ change with temperature for exothermic reactions?
How does $K_{sp}$ change with temperature for exothermic reactions?
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$K_{sp}$ decreases with temperature. Lower temperature favors exothermic dissolution process.
$K_{sp}$ decreases with temperature. Lower temperature favors exothermic dissolution process.
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What is the relationship between $K_{sp}$ and $Q_{sp}$?
What is the relationship between $K_{sp}$ and $Q_{sp}$?
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Precipitation occurs if $Q_{sp} > K_{sp}$. $Q_{sp}$ compares current ion concentrations to equilibrium values.
Precipitation occurs if $Q_{sp} > K_{sp}$. $Q_{sp}$ compares current ion concentrations to equilibrium values.
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What does a large $K_{sp}$ value indicate about solubility?
What does a large $K_{sp}$ value indicate about solubility?
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Compound is more soluble. Higher $K_{sp}$ means more ions can dissolve at equilibrium.
Compound is more soluble. Higher $K_{sp}$ means more ions can dissolve at equilibrium.
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What is the effect of adding $NH_3$ to $AgCl$ solubility?
What is the effect of adding $NH_3$ to $AgCl$ solubility?
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Increases due to complexation. $NH_3$ forms $[Ag(NH_3)_2]^+$ complex, removing $Ag^+$ ions.
Increases due to complexation. $NH_3$ forms $[Ag(NH_3)_2]^+$ complex, removing $Ag^+$ ions.
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What is the effect of $pH$ on the solubility of $Mg(OH)_2$?
What is the effect of $pH$ on the solubility of $Mg(OH)_2$?
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Solubility decreases at higher $pH$. Higher $pH$ increases $[OH^-]$, shifting equilibrium toward solid.
Solubility decreases at higher $pH$. Higher $pH$ increases $[OH^-]$, shifting equilibrium toward solid.
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Identify the $K_{sp}$ expression for $Ca_3(PO_4)_2$.
Identify the $K_{sp}$ expression for $Ca_3(PO_4)_2$.
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$K_{sp} = [Ca^{2+}]^3[PO_4^{3-}]^2$. Stoichiometry: 3 $Ca^{2+}$ and 2 $PO_4^{3-}$ per formula unit.
$K_{sp} = [Ca^{2+}]^3[PO_4^{3-}]^2$. Stoichiometry: 3 $Ca^{2+}$ and 2 $PO_4^{3-}$ per formula unit.
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How does the presence of a common ion affect solubility?
How does the presence of a common ion affect solubility?
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Decreases solubility. Le Chatelier's principle: excess ion shifts equilibrium toward solid.
Decreases solubility. Le Chatelier's principle: excess ion shifts equilibrium toward solid.
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What is the $K_{sp}$ expression for $Al(OH)_3$?
What is the $K_{sp}$ expression for $Al(OH)_3$?
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$K_{sp} = [Al^{3+}][OH^-]^3$. Aluminum hydroxide: 1 $Al^{3+}$ and 3 $OH^-$ ions.
$K_{sp} = [Al^{3+}][OH^-]^3$. Aluminum hydroxide: 1 $Al^{3+}$ and 3 $OH^-$ ions.
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Identify the $K_{sp}$ expression for $BaSO_4$.
Identify the $K_{sp}$ expression for $BaSO_4$.
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$K_{sp} = [Ba^{2+}][SO_4^{2-}]$. 1:1 stoichiometry gives simple product of ion concentrations.
$K_{sp} = [Ba^{2+}][SO_4^{2-}]$. 1:1 stoichiometry gives simple product of ion concentrations.
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What is the solubility product constant ($K_{sp}$) expression for $AgCl$?
What is the solubility product constant ($K_{sp}$) expression for $AgCl$?
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$K_{sp} = [Ag^+][Cl^-]$. Product of ion concentrations at equilibrium for the saturated solution.
$K_{sp} = [Ag^+][Cl^-]$. Product of ion concentrations at equilibrium for the saturated solution.
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Identify the $K_{sp}$ expression for $CuS$.
Identify the $K_{sp}$ expression for $CuS$.
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$K_{sp} = [Cu^{2+}][S^{2-}]$. 1:1 stoichiometry for copper(II) sulfide dissolution.
$K_{sp} = [Cu^{2+}][S^{2-}]$. 1:1 stoichiometry for copper(II) sulfide dissolution.
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How does complex ion formation affect solubility?
How does complex ion formation affect solubility?
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Increases solubility. Complex formation removes free metal ions from solution.
Increases solubility. Complex formation removes free metal ions from solution.
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Identify the $K_{sp}$ expression for $PbSO_4$.
Identify the $K_{sp}$ expression for $PbSO_4$.
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$K_{sp} = [Pb^{2+}][SO_4^{2-}]$. 1:1 stoichiometry for lead(II) sulfate dissolution.
$K_{sp} = [Pb^{2+}][SO_4^{2-}]$. 1:1 stoichiometry for lead(II) sulfate dissolution.
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Which has higher solubility: $BaSO_4$ or $SrSO_4$?
Which has higher solubility: $BaSO_4$ or $SrSO_4$?
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$SrSO_4$ (higher $K_{sp}$ value). Compare $K_{sp}$ values; larger value indicates higher solubility.
$SrSO_4$ (higher $K_{sp}$ value). Compare $K_{sp}$ values; larger value indicates higher solubility.
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Which compound will precipitate first: $AgCl$ or $AgBr$?
Which compound will precipitate first: $AgCl$ or $AgBr$?
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$AgBr$ (lower $K_{sp}$ value). Lower $K_{sp}$ means less soluble, so precipitates first.
$AgBr$ (lower $K_{sp}$ value). Lower $K_{sp}$ means less soluble, so precipitates first.
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State the formula to calculate $Q_{sp}$.
State the formula to calculate $Q_{sp}$.
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$Q_{sp} = [cation]^m[anion]^n$. Same form as $K_{sp}$ but uses current concentrations, not equilibrium.
$Q_{sp} = [cation]^m[anion]^n$. Same form as $K_{sp}$ but uses current concentrations, not equilibrium.
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What is the $K_{sp}$ expression for $Fe(OH)_3$?
What is the $K_{sp}$ expression for $Fe(OH)_3$?
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$K_{sp} = [Fe^{3+}][OH^-]^3$. Stoichiometry: 1 $Fe^{3+}$ and 3 $OH^-$ ions per formula unit.
$K_{sp} = [Fe^{3+}][OH^-]^3$. Stoichiometry: 1 $Fe^{3+}$ and 3 $OH^-$ ions per formula unit.
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Identify the $K_{sp}$ expression for $Hg_2Cl_2$.
Identify the $K_{sp}$ expression for $Hg_2Cl_2$.
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$K_{sp} = [Hg_2^{2+}][Cl^-]^2$. Dimeric mercury(I) ion has +2 charge with two chlorides.
$K_{sp} = [Hg_2^{2+}][Cl^-]^2$. Dimeric mercury(I) ion has +2 charge with two chlorides.
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Identify the effect of temperature on $K_{sp}$ for endothermic dissolution.
Identify the effect of temperature on $K_{sp}$ for endothermic dissolution.
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$K_{sp}$ increases with temperature. Higher temperature favors endothermic dissolution process.
$K_{sp}$ increases with temperature. Higher temperature favors endothermic dissolution process.
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How does $pH$ affect solubility of compounds containing basic anions?
How does $pH$ affect solubility of compounds containing basic anions?
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Increases solubility at lower $pH$. Acidic conditions protonate basic anions, reducing their concentration.
Increases solubility at lower $pH$. Acidic conditions protonate basic anions, reducing their concentration.
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Which compound is more soluble: $CaF_2$ or $SrF_2$?
Which compound is more soluble: $CaF_2$ or $SrF_2$?
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$SrF_2$ (higher $K_{sp}$ value). Compare $K_{sp}$ values directly for same formula type.
$SrF_2$ (higher $K_{sp}$ value). Compare $K_{sp}$ values directly for same formula type.
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What is $K_{sp}$ for $PbCl_2$ given solubility $s$?
What is $K_{sp}$ for $PbCl_2$ given solubility $s$?
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$K_{sp} = 4s^3$. For $PbCl_2$: $K_{sp} = s(2s)^2 = 4s^3$.
$K_{sp} = 4s^3$. For $PbCl_2$: $K_{sp} = s(2s)^2 = 4s^3$.
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Identify the common ion effect in solubility equilibria.
Identify the common ion effect in solubility equilibria.
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Reduction in solubility due to a common ion. Adding an ion already present shifts equilibrium toward solid formation.
Reduction in solubility due to a common ion. Adding an ion already present shifts equilibrium toward solid formation.
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Calculate $K_{sp}$ for $Ag_2S$ with $[Ag^+] = 2x$ and $[S^{2-}] = x$.
Calculate $K_{sp}$ for $Ag_2S$ with $[Ag^+] = 2x$ and $[S^{2-}] = x$.
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$K_{sp} = 4x^3$. For $Ag_2S$: $K_{sp} = [Ag^+]^2[S^{2-}] = (2x)^2(x) = 4x^3$.
$K_{sp} = 4x^3$. For $Ag_2S$: $K_{sp} = [Ag^+]^2[S^{2-}] = (2x)^2(x) = 4x^3$.
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Identify the $K_{sp}$ expression for $CdS$.
Identify the $K_{sp}$ expression for $CdS$.
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$K_{sp} = [Cd^{2+}][S^{2-}]$. 1:1 stoichiometry for cadmium sulfide dissolution.
$K_{sp} = [Cd^{2+}][S^{2-}]$. 1:1 stoichiometry for cadmium sulfide dissolution.
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Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.
Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.
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$K_{sp} = 4x^3$. Substitute equilibrium concentrations: $(2x)^2(x) = 4x^3$.
$K_{sp} = 4x^3$. Substitute equilibrium concentrations: $(2x)^2(x) = 4x^3$.
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Identify the $K_{sp}$ expression for $CdS$.
Identify the $K_{sp}$ expression for $CdS$.
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$K_{sp} = [Cd^{2+}][S^{2-}]$. 1:1 stoichiometry for cadmium sulfide dissolution.
$K_{sp} = [Cd^{2+}][S^{2-}]$. 1:1 stoichiometry for cadmium sulfide dissolution.
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What is the unit of $K_{sp}$ for $CaF_2$?
What is the unit of $K_{sp}$ for $CaF_2$?
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mol^3/L^3. Units from $[Ca^{2+}][F^-]^2$ concentration terms.
mol^3/L^3. Units from $[Ca^{2+}][F^-]^2$ concentration terms.
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