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AP Chemistry Flashcards: Introduction To Solubility Equilibria

Study Introduction To Solubility Equilibria in AP Chemistry with focused flashcards that help you recognize the idea, recall the key rule, and apply it in practice-style prompts.

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What this deck covers

This deck focuses on Introduction To Solubility Equilibria, 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.

AP Chemistry Flashcards: Introduction To Solubility Equilibria

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QUESTION

How does $K_{sp}$ change with temperature for exothermic reactions?

Tap or drag to reveal answer

ANSWER

$K_{sp}$ decreases with temperature. Lower temperature favors exothermic dissolution process.

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All flashcards

Flashcard 1: How does $K_{sp}$ change with temperature for exothermic reactions?

Answer: $K_{sp}$ decreases with temperature. Lower temperature favors exothermic dissolution process.

Flashcard 2: Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.

Answer: $K_{sp} = 4x^3$ . Substitute equilibrium concentrations: $(2x)^2(x) = 4x^3$ .

Flashcard 3: How does $K_{sp}$ change with temperature for exothermic reactions?

Answer: $K_{sp}$ decreases with temperature. Lower temperature favors exothermic dissolution process.

Flashcard 4: What is the relationship between $K_{sp}$ and $Q_{sp}$ ?

Answer: Precipitation occurs if $Q_{sp} > K_{sp}$ . $Q_{sp}$ compares current ion concentrations to equilibrium values.

Flashcard 5: What does a large $K_{sp}$ value indicate about solubility?

Answer: Compound is more soluble. Higher $K_{sp}$ means more ions can dissolve at equilibrium.

Flashcard 6: What is the effect of adding $NH_3$ to $AgCl$ solubility?

Answer: Increases due to complexation. $NH_3$ forms $[Ag(NH_3)_2]^+$ complex, removing $Ag^+$ ions.

Flashcard 7: What is the effect of $pH$ on the solubility of $Mg(OH)_2$ ?

Answer: Solubility decreases at higher $pH$ . Higher $pH$ increases $[OH^-]$ , shifting equilibrium toward solid.

Flashcard 8: Identify the $K_{sp}$ expression for $Ca_3(PO_4)_2$ .

Answer: $K_{sp} = [Ca^{2+}]^3[PO_4^{3-}]^2$ . Stoichiometry: 3 $Ca^{2+}$ and 2 $PO_4^{3-}$ per formula unit.

Flashcard 9: How does the presence of a common ion affect solubility?

Answer: Decreases solubility. Le Chatelier's principle: excess ion shifts equilibrium toward solid.

Flashcard 10: What is the $K_{sp}$ expression for $Al(OH)_3$ ?

Answer: $K_{sp} = [Al^{3+}][OH^-]^3$ . Aluminum hydroxide: 1 $Al^{3+}$ and 3 $OH^-$ ions.

Flashcard 11: Identify the $K_{sp}$ expression for $BaSO_4$ .

Answer: $K_{sp} = [Ba^{2+}][SO_4^{2-}]$ . 1:1 stoichiometry gives simple product of ion concentrations.

Flashcard 12: What is the solubility product constant ( $K_{sp}$ ) expression for $AgCl$ ?

Answer: $K_{sp} = [Ag^+][Cl^-]$ . Product of ion concentrations at equilibrium for the saturated solution.

Flashcard 13: Identify the $K_{sp}$ expression for $CuS$ .

Answer: $K_{sp} = [Cu^{2+}][S^{2-}]$ . 1:1 stoichiometry for copper(II) sulfide dissolution.

Flashcard 14: How does complex ion formation affect solubility?

Answer: Increases solubility. Complex formation removes free metal ions from solution.

Flashcard 15: Identify the $K_{sp}$ expression for $PbSO_4$ .

Answer: $K_{sp} = [Pb^{2+}][SO_4^{2-}]$ . 1:1 stoichiometry for lead(II) sulfate dissolution.

Flashcard 16: Which has higher solubility: $BaSO_4$ or $SrSO_4$ ?

Answer: $SrSO_4$ (higher $K_{sp}$ value). Compare $K_{sp}$ values; larger value indicates higher solubility.

Flashcard 17: Which compound will precipitate first: $AgCl$ or $AgBr$ ?

Answer: $AgBr$ (lower $K_{sp}$ value). Lower $K_{sp}$ means less soluble, so precipitates first.

Flashcard 18: State the formula to calculate $Q_{sp}$ .

Answer: $Q_{sp} = [cation]^m[anion]^n$ . Same form as $K_{sp}$ but uses current concentrations, not equilibrium.

Flashcard 19: What is the $K_{sp}$ expression for $Fe(OH)_3$ ?

Answer: $K_{sp} = [Fe^{3+}][OH^-]^3$ . Stoichiometry: 1 $Fe^{3+}$ and 3 $OH^-$ ions per formula unit.

Flashcard 20: Identify the $K_{sp}$ expression for $Hg_2Cl_2$ .

Answer: $K_{sp} = [Hg_2^{2+}][Cl^-]^2$ . Dimeric mercury(I) ion has +2 charge with two chlorides.

Flashcard 21: Identify the effect of temperature on $K_{sp}$ for endothermic dissolution.

Answer: $K_{sp}$ increases with temperature. Higher temperature favors endothermic dissolution process.

Flashcard 22: How does $pH$ affect solubility of compounds containing basic anions?

Answer: Increases solubility at lower $pH$ . Acidic conditions protonate basic anions, reducing their concentration.

Flashcard 23: Which compound is more soluble: $CaF_2$ or $SrF_2$ ?

Answer: $SrF_2$ (higher $K_{sp}$ value). Compare $K_{sp}$ values directly for same formula type.

Flashcard 24: What is $K_{sp}$ for $PbCl_2$ given solubility $s$ ?

Answer: $K_{sp} = 4s^3$ . For $PbCl_2$ : $K_{sp} = s(2s)^2 = 4s^3$ .

Flashcard 25: Identify the common ion effect in solubility equilibria.

Answer: Reduction in solubility due to a common ion. Adding an ion already present shifts equilibrium toward solid formation.

Flashcard 26: Calculate $K_{sp}$ for $Ag_2S$ with $[Ag^+] = 2x$ and $[S^{2-}] = x$ .

Answer: $K_{sp} = 4x^3$ . For $Ag_2S$ : $K_{sp} = [Ag^+]^2[S^{2-}] = (2x)^2(x) = 4x^3$ .

Flashcard 27: Identify the $K_{sp}$ expression for $CdS$ .

Answer: $K_{sp} = [Cd^{2+}][S^{2-}]$ . 1:1 stoichiometry for cadmium sulfide dissolution.

Flashcard 28: Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.

Answer: $K_{sp} = 4x^3$ . Substitute equilibrium concentrations: $(2x)^2(x) = 4x^3$ .

Flashcard 29: Identify the $K_{sp}$ expression for $CdS$ .

Answer: $K_{sp} = [Cd^{2+}][S^{2-}]$ . 1:1 stoichiometry for cadmium sulfide dissolution.

Flashcard 30: What is the unit of $K_{sp}$ for $CaF_2$ ?

Answer: mol^3/L^3. Units from $[Ca^{2+}][F^-]^2$ concentration terms.

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AP Chemistry Flashcards: Introduction To Solubility Equilibria

Study Introduction To Solubility Equilibria in AP Chemistry with focused flashcards that help you recognize the idea, recall the key rule, and apply it in practice-style prompts.

← Back to flashcard decks

What this deck covers

This deck focuses on Introduction To Solubility Equilibria, 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.

AP Chemistry Flashcards: Introduction To Solubility Equilibria

/ 30

0 reviewed

0% Complete

0 reviewing

QUESTION

How does $K_{sp}$ change with temperature for exothermic reactions?

Tap or drag to reveal answer

ANSWER

$K_{sp}$ decreases with temperature. Lower temperature favors exothermic dissolution process.

Swipe Right = I Know It! 🎉

Swipe Left = Still Learning

All flashcards

Flashcard 1: How does $K_{sp}$ change with temperature for exothermic reactions?

Answer: $K_{sp}$ decreases with temperature. Lower temperature favors exothermic dissolution process.

Flashcard 2: Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.

Answer: $K_{sp} = 4x^3$ . Substitute equilibrium concentrations: $(2x)^2(x) = 4x^3$ .

Flashcard 3: How does $K_{sp}$ change with temperature for exothermic reactions?

Answer: $K_{sp}$ decreases with temperature. Lower temperature favors exothermic dissolution process.

Flashcard 4: What is the relationship between $K_{sp}$ and $Q_{sp}$ ?

Answer: Precipitation occurs if $Q_{sp} > K_{sp}$ . $Q_{sp}$ compares current ion concentrations to equilibrium values.

Flashcard 5: What does a large $K_{sp}$ value indicate about solubility?

Answer: Compound is more soluble. Higher $K_{sp}$ means more ions can dissolve at equilibrium.

Flashcard 6: What is the effect of adding $NH_3$ to $AgCl$ solubility?

Answer: Increases due to complexation. $NH_3$ forms $[Ag(NH_3)_2]^+$ complex, removing $Ag^+$ ions.

Flashcard 7: What is the effect of $pH$ on the solubility of $Mg(OH)_2$ ?

Answer: Solubility decreases at higher $pH$ . Higher $pH$ increases $[OH^-]$ , shifting equilibrium toward solid.

Flashcard 8: Identify the $K_{sp}$ expression for $Ca_3(PO_4)_2$ .

Answer: $K_{sp} = [Ca^{2+}]^3[PO_4^{3-}]^2$ . Stoichiometry: 3 $Ca^{2+}$ and 2 $PO_4^{3-}$ per formula unit.

Flashcard 9: How does the presence of a common ion affect solubility?

Answer: Decreases solubility. Le Chatelier's principle: excess ion shifts equilibrium toward solid.

Flashcard 10: What is the $K_{sp}$ expression for $Al(OH)_3$ ?

Answer: $K_{sp} = [Al^{3+}][OH^-]^3$ . Aluminum hydroxide: 1 $Al^{3+}$ and 3 $OH^-$ ions.

Flashcard 11: Identify the $K_{sp}$ expression for $BaSO_4$ .

Answer: $K_{sp} = [Ba^{2+}][SO_4^{2-}]$ . 1:1 stoichiometry gives simple product of ion concentrations.

Flashcard 12: What is the solubility product constant ( $K_{sp}$ ) expression for $AgCl$ ?

Answer: $K_{sp} = [Ag^+][Cl^-]$ . Product of ion concentrations at equilibrium for the saturated solution.

Flashcard 13: Identify the $K_{sp}$ expression for $CuS$ .

Answer: $K_{sp} = [Cu^{2+}][S^{2-}]$ . 1:1 stoichiometry for copper(II) sulfide dissolution.

Flashcard 14: How does complex ion formation affect solubility?

Answer: Increases solubility. Complex formation removes free metal ions from solution.

Flashcard 15: Identify the $K_{sp}$ expression for $PbSO_4$ .

Answer: $K_{sp} = [Pb^{2+}][SO_4^{2-}]$ . 1:1 stoichiometry for lead(II) sulfate dissolution.

Flashcard 16: Which has higher solubility: $BaSO_4$ or $SrSO_4$ ?

Answer: $SrSO_4$ (higher $K_{sp}$ value). Compare $K_{sp}$ values; larger value indicates higher solubility.

Flashcard 17: Which compound will precipitate first: $AgCl$ or $AgBr$ ?

Answer: $AgBr$ (lower $K_{sp}$ value). Lower $K_{sp}$ means less soluble, so precipitates first.

Flashcard 18: State the formula to calculate $Q_{sp}$ .

Answer: $Q_{sp} = [cation]^m[anion]^n$ . Same form as $K_{sp}$ but uses current concentrations, not equilibrium.

Flashcard 19: What is the $K_{sp}$ expression for $Fe(OH)_3$ ?

Answer: $K_{sp} = [Fe^{3+}][OH^-]^3$ . Stoichiometry: 1 $Fe^{3+}$ and 3 $OH^-$ ions per formula unit.

Flashcard 20: Identify the $K_{sp}$ expression for $Hg_2Cl_2$ .

Answer: $K_{sp} = [Hg_2^{2+}][Cl^-]^2$ . Dimeric mercury(I) ion has +2 charge with two chlorides.

Flashcard 21: Identify the effect of temperature on $K_{sp}$ for endothermic dissolution.

Answer: $K_{sp}$ increases with temperature. Higher temperature favors endothermic dissolution process.

Flashcard 22: How does $pH$ affect solubility of compounds containing basic anions?

Answer: Increases solubility at lower $pH$ . Acidic conditions protonate basic anions, reducing their concentration.

Flashcard 23: Which compound is more soluble: $CaF_2$ or $SrF_2$ ?

Answer: $SrF_2$ (higher $K_{sp}$ value). Compare $K_{sp}$ values directly for same formula type.

Flashcard 24: What is $K_{sp}$ for $PbCl_2$ given solubility $s$ ?

Answer: $K_{sp} = 4s^3$ . For $PbCl_2$ : $K_{sp} = s(2s)^2 = 4s^3$ .

Flashcard 25: Identify the common ion effect in solubility equilibria.

Answer: Reduction in solubility due to a common ion. Adding an ion already present shifts equilibrium toward solid formation.

Flashcard 26: Calculate $K_{sp}$ for $Ag_2S$ with $[Ag^+] = 2x$ and $[S^{2-}] = x$ .

Answer: $K_{sp} = 4x^3$ . For $Ag_2S$ : $K_{sp} = [Ag^+]^2[S^{2-}] = (2x)^2(x) = 4x^3$ .

Flashcard 27: Identify the $K_{sp}$ expression for $CdS$ .

Answer: $K_{sp} = [Cd^{2+}][S^{2-}]$ . 1:1 stoichiometry for cadmium sulfide dissolution.

Flashcard 28: Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.

Answer: $K_{sp} = 4x^3$ . Substitute equilibrium concentrations: $(2x)^2(x) = 4x^3$ .

Flashcard 29: Identify the $K_{sp}$ expression for $CdS$ .

Answer: $K_{sp} = [Cd^{2+}][S^{2-}]$ . 1:1 stoichiometry for cadmium sulfide dissolution.

Flashcard 30: What is the unit of $K_{sp}$ for $CaF_2$ ?

Answer: mol^3/L^3. Units from $[Ca^{2+}][F^-]^2$ concentration terms.

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AP Chemistry Flashcards: Introduction To Solubility Equilibria

What this deck covers

How to use these flashcards

AP Chemistry Flashcards: Introduction To Solubility Equilibria

All flashcards

Flashcard 1: How does KspK_{sp}Ksp​ change with temperature for exothermic reactions?

Flashcard 2: Determine KspK_{sp}Ksp​ for Ag2SAg_2SAg2​S if [Ag+]=2x[Ag^+] = 2x[Ag+]=2x and [S2−]=x[S^{2-}] = x[S2−]=x at equilibrium.

Flashcard 3: How does KspK_{sp}Ksp​ change with temperature for exothermic reactions?

Flashcard 4: What is the relationship between KspK_{sp}Ksp​ and QspQ_{sp}Qsp​?

Flashcard 5: What does a large KspK_{sp}Ksp​ value indicate about solubility?

Flashcard 6: What is the effect of adding NH3NH_3NH3​ to AgClAgClAgCl solubility?

Flashcard 7: What is the effect of pHpHpH on the solubility of Mg(OH)2Mg(OH)_2Mg(OH)2​?

Flashcard 8: Identify the KspK_{sp}Ksp​ expression for Ca3(PO4)2Ca_3(PO_4)_2Ca3​(PO4​)2​.

Flashcard 9: How does the presence of a common ion affect solubility?

Flashcard 10: What is the KspK_{sp}Ksp​ expression for Al(OH)3Al(OH)_3Al(OH)3​?

Flashcard 11: Identify the KspK_{sp}Ksp​ expression for BaSO4BaSO_4BaSO4​.

Flashcard 12: What is the solubility product constant (KspK_{sp}Ksp​) expression for AgClAgClAgCl?

Flashcard 13: Identify the KspK_{sp}Ksp​ expression for CuSCuSCuS.

Flashcard 14: How does complex ion formation affect solubility?

Flashcard 15: Identify the KspK_{sp}Ksp​ expression for PbSO4PbSO_4PbSO4​.

Flashcard 16: Which has higher solubility: BaSO4BaSO_4BaSO4​ or SrSO4SrSO_4SrSO4​?

Flashcard 17: Which compound will precipitate first: AgClAgClAgCl or AgBrAgBrAgBr?

Flashcard 18: State the formula to calculate QspQ_{sp}Qsp​.

Flashcard 19: What is the KspK_{sp}Ksp​ expression for Fe(OH)3Fe(OH)_3Fe(OH)3​?

Flashcard 20: Identify the KspK_{sp}Ksp​ expression for Hg2Cl2Hg_2Cl_2Hg2​Cl2​.

Flashcard 21: Identify the effect of temperature on KspK_{sp}Ksp​ for endothermic dissolution.

Flashcard 22: How does pHpHpH affect solubility of compounds containing basic anions?

Flashcard 23: Which compound is more soluble: CaF2CaF_2CaF2​ or SrF2SrF_2SrF2​?

Flashcard 24: What is KspK_{sp}Ksp​ for PbCl2PbCl_2PbCl2​ given solubility sss?

Flashcard 25: Identify the common ion effect in solubility equilibria.

Flashcard 26: Calculate KspK_{sp}Ksp​ for Ag2SAg_2SAg2​S with [Ag+]=2x[Ag^+] = 2x[Ag+]=2x and [S2−]=x[S^{2-}] = x[S2−]=x.

Flashcard 27: Identify the KspK_{sp}Ksp​ expression for CdSCdSCdS.

Flashcard 28: Determine KspK_{sp}Ksp​ for Ag2SAg_2SAg2​S if [Ag+]=2x[Ag^+] = 2x[Ag+]=2x and [S2−]=x[S^{2-}] = x[S2−]=x at equilibrium.

Flashcard 29: Identify the KspK_{sp}Ksp​ expression for CdSCdSCdS.

Flashcard 30: What is the unit of KspK_{sp}Ksp​ for CaF2CaF_2CaF2​?

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AP Chemistry Flashcards: Introduction To Solubility Equilibria

What this deck covers

How to use these flashcards

AP Chemistry Flashcards: Introduction To Solubility Equilibria

All flashcards

Flashcard 1: How does KspK_{sp}Ksp​ change with temperature for exothermic reactions?

Flashcard 2: Determine KspK_{sp}Ksp​ for Ag2SAg_2SAg2​S if [Ag+]=2x[Ag^+] = 2x[Ag+]=2x and [S2−]=x[S^{2-}] = x[S2−]=x at equilibrium.

Flashcard 3: How does KspK_{sp}Ksp​ change with temperature for exothermic reactions?

Flashcard 4: What is the relationship between KspK_{sp}Ksp​ and QspQ_{sp}Qsp​?

Flashcard 5: What does a large KspK_{sp}Ksp​ value indicate about solubility?

Flashcard 6: What is the effect of adding NH3NH_3NH3​ to AgClAgClAgCl solubility?

Flashcard 7: What is the effect of pHpHpH on the solubility of Mg(OH)2Mg(OH)_2Mg(OH)2​?

Flashcard 8: Identify the KspK_{sp}Ksp​ expression for Ca3(PO4)2Ca_3(PO_4)_2Ca3​(PO4​)2​.

Flashcard 9: How does the presence of a common ion affect solubility?

Flashcard 10: What is the KspK_{sp}Ksp​ expression for Al(OH)3Al(OH)_3Al(OH)3​?

Flashcard 11: Identify the KspK_{sp}Ksp​ expression for BaSO4BaSO_4BaSO4​.

Flashcard 12: What is the solubility product constant (KspK_{sp}Ksp​) expression for AgClAgClAgCl?

Flashcard 13: Identify the KspK_{sp}Ksp​ expression for CuSCuSCuS.

Flashcard 14: How does complex ion formation affect solubility?

Flashcard 15: Identify the KspK_{sp}Ksp​ expression for PbSO4PbSO_4PbSO4​.

Flashcard 16: Which has higher solubility: BaSO4BaSO_4BaSO4​ or SrSO4SrSO_4SrSO4​?

Flashcard 17: Which compound will precipitate first: AgClAgClAgCl or AgBrAgBrAgBr?

Flashcard 18: State the formula to calculate QspQ_{sp}Qsp​.

Flashcard 19: What is the KspK_{sp}Ksp​ expression for Fe(OH)3Fe(OH)_3Fe(OH)3​?

Flashcard 20: Identify the KspK_{sp}Ksp​ expression for Hg2Cl2Hg_2Cl_2Hg2​Cl2​.

Flashcard 21: Identify the effect of temperature on KspK_{sp}Ksp​ for endothermic dissolution.

Flashcard 22: How does pHpHpH affect solubility of compounds containing basic anions?

Flashcard 23: Which compound is more soluble: CaF2CaF_2CaF2​ or SrF2SrF_2SrF2​?

Flashcard 24: What is KspK_{sp}Ksp​ for PbCl2PbCl_2PbCl2​ given solubility sss?

Flashcard 25: Identify the common ion effect in solubility equilibria.

Flashcard 26: Calculate KspK_{sp}Ksp​ for Ag2SAg_2SAg2​S with [Ag+]=2x[Ag^+] = 2x[Ag+]=2x and [S2−]=x[S^{2-}] = x[S2−]=x.

Flashcard 27: Identify the KspK_{sp}Ksp​ expression for CdSCdSCdS.

Flashcard 28: Determine KspK_{sp}Ksp​ for Ag2SAg_2SAg2​S if [Ag+]=2x[Ag^+] = 2x[Ag+]=2x and [S2−]=x[S^{2-}] = x[S2−]=x at equilibrium.

Flashcard 29: Identify the KspK_{sp}Ksp​ expression for CdSCdSCdS.

Flashcard 30: What is the unit of KspK_{sp}Ksp​ for CaF2CaF_2CaF2​?

Flashcard 1: How does $K_{sp}$ change with temperature for exothermic reactions?

Flashcard 2: Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.

Flashcard 3: How does $K_{sp}$ change with temperature for exothermic reactions?

Flashcard 4: What is the relationship between $K_{sp}$ and $Q_{sp}$ ?

Flashcard 5: What does a large $K_{sp}$ value indicate about solubility?

Flashcard 6: What is the effect of adding $NH_3$ to $AgCl$ solubility?

Flashcard 7: What is the effect of $pH$ on the solubility of $Mg(OH)_2$ ?

Flashcard 8: Identify the $K_{sp}$ expression for $Ca_3(PO_4)_2$ .

Flashcard 10: What is the $K_{sp}$ expression for $Al(OH)_3$ ?

Flashcard 11: Identify the $K_{sp}$ expression for $BaSO_4$ .

Flashcard 12: What is the solubility product constant ( $K_{sp}$ ) expression for $AgCl$ ?

Flashcard 13: Identify the $K_{sp}$ expression for $CuS$ .

Flashcard 15: Identify the $K_{sp}$ expression for $PbSO_4$ .

Flashcard 16: Which has higher solubility: $BaSO_4$ or $SrSO_4$ ?

Flashcard 17: Which compound will precipitate first: $AgCl$ or $AgBr$ ?

Flashcard 18: State the formula to calculate $Q_{sp}$ .

Flashcard 19: What is the $K_{sp}$ expression for $Fe(OH)_3$ ?

Flashcard 20: Identify the $K_{sp}$ expression for $Hg_2Cl_2$ .

Flashcard 21: Identify the effect of temperature on $K_{sp}$ for endothermic dissolution.

Flashcard 22: How does $pH$ affect solubility of compounds containing basic anions?

Flashcard 23: Which compound is more soluble: $CaF_2$ or $SrF_2$ ?

Flashcard 24: What is $K_{sp}$ for $PbCl_2$ given solubility $s$ ?

Flashcard 26: Calculate $K_{sp}$ for $Ag_2S$ with $[Ag^+] = 2x$ and $[S^{2-}] = x$ .

Flashcard 27: Identify the $K_{sp}$ expression for $CdS$ .

Flashcard 28: Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.

Flashcard 29: Identify the $K_{sp}$ expression for $CdS$ .

Flashcard 30: What is the unit of $K_{sp}$ for $CaF_2$ ?

Flashcard 1: How does $K_{sp}$ change with temperature for exothermic reactions?

Flashcard 2: Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.

Flashcard 3: How does $K_{sp}$ change with temperature for exothermic reactions?

Flashcard 4: What is the relationship between $K_{sp}$ and $Q_{sp}$ ?

Flashcard 5: What does a large $K_{sp}$ value indicate about solubility?

Flashcard 6: What is the effect of adding $NH_3$ to $AgCl$ solubility?

Flashcard 7: What is the effect of $pH$ on the solubility of $Mg(OH)_2$ ?

Flashcard 8: Identify the $K_{sp}$ expression for $Ca_3(PO_4)_2$ .

Flashcard 10: What is the $K_{sp}$ expression for $Al(OH)_3$ ?

Flashcard 11: Identify the $K_{sp}$ expression for $BaSO_4$ .

Flashcard 12: What is the solubility product constant ( $K_{sp}$ ) expression for $AgCl$ ?

Flashcard 13: Identify the $K_{sp}$ expression for $CuS$ .

Flashcard 15: Identify the $K_{sp}$ expression for $PbSO_4$ .

Flashcard 16: Which has higher solubility: $BaSO_4$ or $SrSO_4$ ?

Flashcard 17: Which compound will precipitate first: $AgCl$ or $AgBr$ ?

Flashcard 18: State the formula to calculate $Q_{sp}$ .

Flashcard 19: What is the $K_{sp}$ expression for $Fe(OH)_3$ ?

Flashcard 20: Identify the $K_{sp}$ expression for $Hg_2Cl_2$ .

Flashcard 21: Identify the effect of temperature on $K_{sp}$ for endothermic dissolution.

Flashcard 22: How does $pH$ affect solubility of compounds containing basic anions?

Flashcard 23: Which compound is more soluble: $CaF_2$ or $SrF_2$ ?

Flashcard 24: What is $K_{sp}$ for $PbCl_2$ given solubility $s$ ?

Flashcard 26: Calculate $K_{sp}$ for $Ag_2S$ with $[Ag^+] = 2x$ and $[S^{2-}] = x$ .

Flashcard 27: Identify the $K_{sp}$ expression for $CdS$ .

Flashcard 28: Determine $K_{sp}$ for $Ag_2S$ if $[Ag^+] = 2x$ and $[S^{2-}] = x$ at equilibrium.

Flashcard 29: Identify the $K_{sp}$ expression for $CdS$ .

Flashcard 30: What is the unit of $K_{sp}$ for $CaF_2$ ?