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AP Chemistry Flashcards: Common Ion Effect

Study Common Ion Effect 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 Common Ion Effect, 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: Common Ion Effect

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QUESTION

State the equilibrium expression for a weak acid $HA$ with $K_a$ .

Tap or drag to reveal answer

ANSWER

$K_a=\frac{[H^+][A^-]}{[HA]}$ . Products over reactants for weak acid dissociation equilibrium.

Swipe Right = I Know It! 🎉

Swipe Left = Still Learning

All flashcards

Flashcard 1: State the equilibrium expression for a weak acid $HA$ with $K_a$ .

Answer: $K_a=\frac{[H^+][A^-]}{[HA]}$ . Products over reactants for weak acid dissociation equilibrium.

Flashcard 2: What happens to $[H^+]$ when a strong acid is added to a weak acid solution?

Answer: $[H^+]$ increases; weak acid ionization decreases. Strong acid fully dissociates, suppressing weak acid's partial ionization.

Flashcard 3: What is the common-ion effect in aqueous equilibrium systems?

Answer: Added common ion shifts equilibrium left, reducing dissociation/solubility. Excess product ions drive equilibrium backward per Le Châtelier's principle.

Flashcard 4: For $AgCl(s)$ , what happens to solubility when $NaCl(aq)$ is added?

Answer: Solubility decreases (common ion $Cl^-$ ). Added chloride shifts dissolution equilibrium left.

Flashcard 5: What happens to $pH$ when $A^-$ (the conjugate base) is added to a buffer of $HA/A^-$ ?

Answer: $pH$ increases. More conjugate base consumes $H^+$ , raising pH.

Flashcard 6: For $CaF_2(s)$ , what happens to solubility when $NaF(aq)$ is added?

Answer: Solubility decreases (common ion $F^-$ ). Added fluoride shifts dissolution equilibrium left.

Flashcard 7: Identify the direction of shift when $NaOH$ is added to $NH_3(aq)$ .

Answer: Shift left; $NH_3$ forms less $NH_4^+$ . Added $OH^-$ shifts ammonia-water equilibrium left.

Flashcard 8: Identify the direction of shift when $CH_3COONa$ is added to $CH_3COOH(aq)$ .

Answer: Shift left; $CH_3COOH$ ionizes less. Added acetate ion suppresses acetic acid dissociation.

Flashcard 9: Which ion is the common ion when $NH_4Cl$ is added to a solution containing $NH_3$ ?

Answer: $NH_4^+$ . Both $NH_4Cl$ and protonated $NH_3$ contain ammonium ion.

Flashcard 10: Which ion is the common ion when $NaF$ is added to a solution containing $HF$ ?

Answer: $F^-$ . Both $NaF$ and $HF$ contain fluoride ion in solution.

Flashcard 11: What is the effect on molar solubility when a common ion is added to a sparingly soluble salt?

Answer: Molar solubility decreases. Common ion shifts dissolution equilibrium left, reducing dissolved ions.

Flashcard 12: Which relationship is correct for a conjugate pair: $K_a$ and $K_b$ at $25^\circ C$ ?

Answer: $K_aK_b=K_w=1.0\times 10^{-14}$ . Conjugate acid-base pairs multiply to water's ion product.

Flashcard 13: What is the solubility product expression for $M(OH)_2(s)\rightleftharpoons M^{2+}+2OH^-$ ?

Answer: $K_{sp}=[M^{2+}][OH^-]^2$ . Includes squared $[OH^-]$ due to stoichiometry coefficient of 2.

Flashcard 14: What is the solubility product expression for $MX(s)\rightleftharpoons M^+ + X^-$ ?

Answer: $K_{sp}=[M^+][X^-]$ . Product of ion concentrations for 1:1 salt dissolution.

Flashcard 15: What is the net ionic equation for common-ion suppression of $B$ by adding $BH^+$ ?

Answer: $B(aq)+H_2O(l)\rightleftharpoons BH^+(aq)+OH^-(aq)$ shifts left. Added $BH^+$ drives equilibrium toward unprotonated $B$ .

Flashcard 16: What is the net ionic equation for common-ion suppression of $HA$ by adding $A^-$ ?

Answer: $HA(aq)\rightleftharpoons H^+(aq)+A^-(aq)$ shifts left. Added $A^-$ drives equilibrium toward undissociated $HA$ .

Flashcard 17: State the equilibrium expression for a weak base $B$ with $K_b$ .

Answer: $K_b=\frac{[BH^+][OH^-]}{[B]}$ . Products over reactants for weak base protonation equilibrium.

Flashcard 18: What happens to $[OH^-]$ when a strong base is added to a weak base solution?

Answer: $[OH^-]$ increases; weak base ionization decreases. Strong base fully dissociates, suppressing weak base's partial ionization.

Flashcard 19: What is the equilibrium expression for a weak acid $\text{HA}$ : $\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-$ ?

Answer: $K_a=\frac{[\text{H}^+][\text{A}^-]}{[\text{HA}]}$ . Products over reactants for weak acid dissociation.

Flashcard 20: What is the common-ion effect in aqueous equilibrium systems?

Answer: Adding a shared ion shifts equilibrium left, reducing ionization/solubility. Le Châtelier's principle: system responds to minimize disturbance.

Flashcard 21: What is the molar solubility $s$ of $\text{CaF}_2$ in pure water in terms of $K_{sp}$ ?

Answer: $s=\left(\frac{K_{sp}}{4}\right)^{\frac{1}{3}}$ . For 1:2 salt, $K_{sp}=s(2s)^2=4s^3$ .

Flashcard 22: Assuming $[\text{F}^-]_{\text{initial}} \gg 2s$ , what is $s$ for $\text{CaF}_2$ in $[\text{F}^-]$ using $K_{sp}$ ?

Answer: $s\approx\frac{K_{sp}}{[\text{F}^-]^2}$ . When common ion dominates, solve $K_{sp}$ for cation concentration.

Flashcard 23: What is the molar solubility $s$ of $\text{AgCl}$ in pure water in terms of $K_{sp}$ ?

Answer: $s=\sqrt{K_{sp}}$ . For 1:1 salt, $K_{sp}=s^2$ where $s$ is molar solubility.

Flashcard 24: Which direction does $\text{B}+\text{H}_2\text{O} \rightleftharpoons \text{BH}^+ + \text{OH}^-$ shift when $[\text{BH}^+]$ is increased?

Answer: Left (toward $\text{B}$ ). Excess product drives equilibrium toward reactants.

Flashcard 25: Assuming $[\text{Cl}^-]_{\text{initial}} \gg s$ , what is $s$ for $\text{AgCl}$ in $[\text{Cl}^-]$ using $K_{sp}$ ?

Answer: $s\approx\frac{K_{sp}}{[\text{Cl}^-]}$ . When common ion dominates, solve $K_{sp}$ for remaining ion.

Flashcard 26: In $\text{AgCl}(s) \rightleftharpoons \text{Ag}^+ + \text{Cl}^-$ , what happens to $[\text{Ag}^+]$ when $[\text{Cl}^-]$ is increased?

Answer: $[\text{Ag}^+]$ decreases. To maintain constant $K_{sp}$ , $[\text{Ag}^+]$ must decrease.

Flashcard 27: Which direction does $\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-$ shift when $[\text{A}^-]$ is increased?

Answer: Left (toward $\text{HA}$ ). Excess product drives equilibrium toward reactants.

Flashcard 28: What is the buffer relationship between conjugate pairs: $\text{HA}$ and $\text{A}^-$ , in terms of the common-ion effect?

Answer: $\text{A}^-$ suppresses ionization of $\text{HA}$ . Conjugate base reduces conjugate acid ionization.

Flashcard 29: Identify the common ion when $\text{BaSO}_4(s)$ is placed in a solution of $\text{Na}_2\text{SO}_4(aq)$ .

Answer: $\text{SO}_4^{2-}$ . Sulfate ion is present in both the solid and added salt.

Flashcard 30: Identify the common ion when $\text{CaF}_2(s)$ is placed in a solution of $\text{NaF}(aq)$ .

Answer: $\text{F}^-$ . Fluoride ion is present in both the solid and added salt.

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AP Chemistry Flashcards: Common Ion Effect

Study Common Ion Effect 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 Common Ion Effect, 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: Common Ion Effect

/ 30

0 reviewed

0% Complete

0 reviewing

QUESTION

State the equilibrium expression for a weak acid $HA$ with $K_a$ .

Tap or drag to reveal answer

ANSWER

$K_a=\frac{[H^+][A^-]}{[HA]}$ . Products over reactants for weak acid dissociation equilibrium.

Swipe Right = I Know It! 🎉

Swipe Left = Still Learning

All flashcards

Flashcard 1: State the equilibrium expression for a weak acid $HA$ with $K_a$ .

Answer: $K_a=\frac{[H^+][A^-]}{[HA]}$ . Products over reactants for weak acid dissociation equilibrium.

Flashcard 2: What happens to $[H^+]$ when a strong acid is added to a weak acid solution?

Answer: $[H^+]$ increases; weak acid ionization decreases. Strong acid fully dissociates, suppressing weak acid's partial ionization.

Flashcard 3: What is the common-ion effect in aqueous equilibrium systems?

Answer: Added common ion shifts equilibrium left, reducing dissociation/solubility. Excess product ions drive equilibrium backward per Le Châtelier's principle.

Flashcard 4: For $AgCl(s)$ , what happens to solubility when $NaCl(aq)$ is added?

Answer: Solubility decreases (common ion $Cl^-$ ). Added chloride shifts dissolution equilibrium left.

Flashcard 5: What happens to $pH$ when $A^-$ (the conjugate base) is added to a buffer of $HA/A^-$ ?

Answer: $pH$ increases. More conjugate base consumes $H^+$ , raising pH.

Flashcard 6: For $CaF_2(s)$ , what happens to solubility when $NaF(aq)$ is added?

Answer: Solubility decreases (common ion $F^-$ ). Added fluoride shifts dissolution equilibrium left.

Flashcard 7: Identify the direction of shift when $NaOH$ is added to $NH_3(aq)$ .

Answer: Shift left; $NH_3$ forms less $NH_4^+$ . Added $OH^-$ shifts ammonia-water equilibrium left.

Flashcard 8: Identify the direction of shift when $CH_3COONa$ is added to $CH_3COOH(aq)$ .

Answer: Shift left; $CH_3COOH$ ionizes less. Added acetate ion suppresses acetic acid dissociation.

Flashcard 9: Which ion is the common ion when $NH_4Cl$ is added to a solution containing $NH_3$ ?

Answer: $NH_4^+$ . Both $NH_4Cl$ and protonated $NH_3$ contain ammonium ion.

Flashcard 10: Which ion is the common ion when $NaF$ is added to a solution containing $HF$ ?

Answer: $F^-$ . Both $NaF$ and $HF$ contain fluoride ion in solution.

Flashcard 11: What is the effect on molar solubility when a common ion is added to a sparingly soluble salt?

Answer: Molar solubility decreases. Common ion shifts dissolution equilibrium left, reducing dissolved ions.

Flashcard 12: Which relationship is correct for a conjugate pair: $K_a$ and $K_b$ at $25^\circ C$ ?

Answer: $K_aK_b=K_w=1.0\times 10^{-14}$ . Conjugate acid-base pairs multiply to water's ion product.

Flashcard 13: What is the solubility product expression for $M(OH)_2(s)\rightleftharpoons M^{2+}+2OH^-$ ?

Answer: $K_{sp}=[M^{2+}][OH^-]^2$ . Includes squared $[OH^-]$ due to stoichiometry coefficient of 2.

Flashcard 14: What is the solubility product expression for $MX(s)\rightleftharpoons M^+ + X^-$ ?

Answer: $K_{sp}=[M^+][X^-]$ . Product of ion concentrations for 1:1 salt dissolution.

Flashcard 15: What is the net ionic equation for common-ion suppression of $B$ by adding $BH^+$ ?

Answer: $B(aq)+H_2O(l)\rightleftharpoons BH^+(aq)+OH^-(aq)$ shifts left. Added $BH^+$ drives equilibrium toward unprotonated $B$ .

Flashcard 16: What is the net ionic equation for common-ion suppression of $HA$ by adding $A^-$ ?

Answer: $HA(aq)\rightleftharpoons H^+(aq)+A^-(aq)$ shifts left. Added $A^-$ drives equilibrium toward undissociated $HA$ .

Flashcard 17: State the equilibrium expression for a weak base $B$ with $K_b$ .

Answer: $K_b=\frac{[BH^+][OH^-]}{[B]}$ . Products over reactants for weak base protonation equilibrium.

Flashcard 18: What happens to $[OH^-]$ when a strong base is added to a weak base solution?

Answer: $[OH^-]$ increases; weak base ionization decreases. Strong base fully dissociates, suppressing weak base's partial ionization.

Flashcard 19: What is the equilibrium expression for a weak acid $\text{HA}$ : $\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-$ ?

Answer: $K_a=\frac{[\text{H}^+][\text{A}^-]}{[\text{HA}]}$ . Products over reactants for weak acid dissociation.

Flashcard 20: What is the common-ion effect in aqueous equilibrium systems?

Answer: Adding a shared ion shifts equilibrium left, reducing ionization/solubility. Le Châtelier's principle: system responds to minimize disturbance.

Flashcard 21: What is the molar solubility $s$ of $\text{CaF}_2$ in pure water in terms of $K_{sp}$ ?

Answer: $s=\left(\frac{K_{sp}}{4}\right)^{\frac{1}{3}}$ . For 1:2 salt, $K_{sp}=s(2s)^2=4s^3$ .

Flashcard 22: Assuming $[\text{F}^-]_{\text{initial}} \gg 2s$ , what is $s$ for $\text{CaF}_2$ in $[\text{F}^-]$ using $K_{sp}$ ?

Answer: $s\approx\frac{K_{sp}}{[\text{F}^-]^2}$ . When common ion dominates, solve $K_{sp}$ for cation concentration.

Flashcard 23: What is the molar solubility $s$ of $\text{AgCl}$ in pure water in terms of $K_{sp}$ ?

Answer: $s=\sqrt{K_{sp}}$ . For 1:1 salt, $K_{sp}=s^2$ where $s$ is molar solubility.

Flashcard 24: Which direction does $\text{B}+\text{H}_2\text{O} \rightleftharpoons \text{BH}^+ + \text{OH}^-$ shift when $[\text{BH}^+]$ is increased?

Answer: Left (toward $\text{B}$ ). Excess product drives equilibrium toward reactants.

Flashcard 25: Assuming $[\text{Cl}^-]_{\text{initial}} \gg s$ , what is $s$ for $\text{AgCl}$ in $[\text{Cl}^-]$ using $K_{sp}$ ?

Answer: $s\approx\frac{K_{sp}}{[\text{Cl}^-]}$ . When common ion dominates, solve $K_{sp}$ for remaining ion.

Flashcard 26: In $\text{AgCl}(s) \rightleftharpoons \text{Ag}^+ + \text{Cl}^-$ , what happens to $[\text{Ag}^+]$ when $[\text{Cl}^-]$ is increased?

Answer: $[\text{Ag}^+]$ decreases. To maintain constant $K_{sp}$ , $[\text{Ag}^+]$ must decrease.

Flashcard 27: Which direction does $\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-$ shift when $[\text{A}^-]$ is increased?

Answer: Left (toward $\text{HA}$ ). Excess product drives equilibrium toward reactants.

Flashcard 28: What is the buffer relationship between conjugate pairs: $\text{HA}$ and $\text{A}^-$ , in terms of the common-ion effect?

Answer: $\text{A}^-$ suppresses ionization of $\text{HA}$ . Conjugate base reduces conjugate acid ionization.

Flashcard 29: Identify the common ion when $\text{BaSO}_4(s)$ is placed in a solution of $\text{Na}_2\text{SO}_4(aq)$ .

Answer: $\text{SO}_4^{2-}$ . Sulfate ion is present in both the solid and added salt.

Flashcard 30: Identify the common ion when $\text{CaF}_2(s)$ is placed in a solution of $\text{NaF}(aq)$ .

Answer: $\text{F}^-$ . Fluoride ion is present in both the solid and added salt.

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AP Chemistry Flashcards: Common Ion Effect

What this deck covers

How to use these flashcards

AP Chemistry Flashcards: Common Ion Effect

All flashcards

Flashcard 1: State the equilibrium expression for a weak acid HAHAHA with KaK_aKa​.

Flashcard 2: What happens to [H+][H^+][H+] when a strong acid is added to a weak acid solution?

Flashcard 3: What is the common-ion effect in aqueous equilibrium systems?

Flashcard 4: For AgCl(s)AgCl(s)AgCl(s), what happens to solubility when NaCl(aq)NaCl(aq)NaCl(aq) is added?

Flashcard 5: What happens to pHpHpH when A−A^-A− (the conjugate base) is added to a buffer of HA/A−HA/A^-HA/A−?

Flashcard 6: For CaF2(s)CaF_2(s)CaF2​(s), what happens to solubility when NaF(aq)NaF(aq)NaF(aq) is added?

Flashcard 7: Identify the direction of shift when NaOHNaOHNaOH is added to NH3(aq)NH_3(aq)NH3​(aq).

Flashcard 8: Identify the direction of shift when CH3COONaCH_3COONaCH3​COONa is added to CH3COOH(aq)CH_3COOH(aq)CH3​COOH(aq).

Flashcard 9: Which ion is the common ion when NH4ClNH_4ClNH4​Cl is added to a solution containing NH3NH_3NH3​?

Flashcard 10: Which ion is the common ion when NaFNaFNaF is added to a solution containing HFHFHF?

Flashcard 11: What is the effect on molar solubility when a common ion is added to a sparingly soluble salt?

Flashcard 12: Which relationship is correct for a conjugate pair: KaK_aKa​ and KbK_bKb​ at 25∘C25^\circ C25∘C?

Flashcard 13: What is the solubility product expression for M(OH)2(s)⇌M2++2OH−M(OH)_2(s)\rightleftharpoons M^{2+}+2OH^-M(OH)2​(s)⇌M2++2OH−?

Flashcard 14: What is the solubility product expression for MX(s)⇌M++X−MX(s)\rightleftharpoons M^+ + X^-MX(s)⇌M++X−?

Flashcard 15: What is the net ionic equation for common-ion suppression of BBB by adding BH+BH^+BH+?

Flashcard 16: What is the net ionic equation for common-ion suppression of HAHAHA by adding A−A^-A−?

Flashcard 17: State the equilibrium expression for a weak base BBB with KbK_bKb​.

Flashcard 18: What happens to [OH−][OH^-][OH−] when a strong base is added to a weak base solution?

Flashcard 19: What is the equilibrium expression for a weak acid HA\text{HA}HA: HA⇌H++A−\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-HA⇌H++A−?

Flashcard 20: What is the common-ion effect in aqueous equilibrium systems?

Flashcard 21: What is the molar solubility sss of CaF2\text{CaF}_2CaF2​ in pure water in terms of KspK_{sp}Ksp​?

Flashcard 22: Assuming [F−]initial≫2s[\text{F}^-]_{\text{initial}} \gg 2s[F−]initial​≫2s, what is sss for CaF2\text{CaF}_2CaF2​ in [F−][\text{F}^-][F−] using KspK_{sp}Ksp​?

Flashcard 23: What is the molar solubility sss of AgCl\text{AgCl}AgCl in pure water in terms of KspK_{sp}Ksp​?

Flashcard 24: Which direction does B+H2O⇌BH++OH−\text{B}+\text{H}_2\text{O} \rightleftharpoons \text{BH}^+ + \text{OH}^-B+H2​O⇌BH++OH− shift when [BH+][\text{BH}^+][BH+] is increased?

Flashcard 25: Assuming [Cl−]initial≫s[\text{Cl}^-]_{\text{initial}} \gg s[Cl−]initial​≫s, what is sss for AgCl\text{AgCl}AgCl in [Cl−][\text{Cl}^-][Cl−] using KspK_{sp}Ksp​?

Flashcard 26: In AgCl(s)⇌Ag++Cl−\text{AgCl}(s) \rightleftharpoons \text{Ag}^+ + \text{Cl}^-AgCl(s)⇌Ag++Cl−, what happens to [Ag+][\text{Ag}^+][Ag+] when [Cl−][\text{Cl}^-][Cl−] is increased?

Flashcard 27: Which direction does HA⇌H++A−\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-HA⇌H++A− shift when [A−][\text{A}^-][A−] is increased?

Flashcard 28: What is the buffer relationship between conjugate pairs: HA\text{HA}HA and A−\text{A}^-A−, in terms of the common-ion effect?

Flashcard 29: Identify the common ion when BaSO4(s)\text{BaSO}_4(s)BaSO4​(s) is placed in a solution of Na2SO4(aq)\text{Na}_2\text{SO}_4(aq)Na2​SO4​(aq).

Flashcard 30: Identify the common ion when CaF2(s)\text{CaF}_2(s)CaF2​(s) is placed in a solution of NaF(aq)\text{NaF}(aq)NaF(aq).

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AP Chemistry Flashcards: Common Ion Effect

What this deck covers

How to use these flashcards

AP Chemistry Flashcards: Common Ion Effect

All flashcards

Flashcard 1: State the equilibrium expression for a weak acid HAHAHA with KaK_aKa​.

Flashcard 2: What happens to [H+][H^+][H+] when a strong acid is added to a weak acid solution?

Flashcard 3: What is the common-ion effect in aqueous equilibrium systems?

Flashcard 4: For AgCl(s)AgCl(s)AgCl(s), what happens to solubility when NaCl(aq)NaCl(aq)NaCl(aq) is added?

Flashcard 5: What happens to pHpHpH when A−A^-A− (the conjugate base) is added to a buffer of HA/A−HA/A^-HA/A−?

Flashcard 6: For CaF2(s)CaF_2(s)CaF2​(s), what happens to solubility when NaF(aq)NaF(aq)NaF(aq) is added?

Flashcard 7: Identify the direction of shift when NaOHNaOHNaOH is added to NH3(aq)NH_3(aq)NH3​(aq).

Flashcard 8: Identify the direction of shift when CH3COONaCH_3COONaCH3​COONa is added to CH3COOH(aq)CH_3COOH(aq)CH3​COOH(aq).

Flashcard 9: Which ion is the common ion when NH4ClNH_4ClNH4​Cl is added to a solution containing NH3NH_3NH3​?

Flashcard 10: Which ion is the common ion when NaFNaFNaF is added to a solution containing HFHFHF?

Flashcard 11: What is the effect on molar solubility when a common ion is added to a sparingly soluble salt?

Flashcard 12: Which relationship is correct for a conjugate pair: KaK_aKa​ and KbK_bKb​ at 25∘C25^\circ C25∘C?

Flashcard 13: What is the solubility product expression for M(OH)2(s)⇌M2++2OH−M(OH)_2(s)\rightleftharpoons M^{2+}+2OH^-M(OH)2​(s)⇌M2++2OH−?

Flashcard 14: What is the solubility product expression for MX(s)⇌M++X−MX(s)\rightleftharpoons M^+ + X^-MX(s)⇌M++X−?

Flashcard 15: What is the net ionic equation for common-ion suppression of BBB by adding BH+BH^+BH+?

Flashcard 16: What is the net ionic equation for common-ion suppression of HAHAHA by adding A−A^-A−?

Flashcard 17: State the equilibrium expression for a weak base BBB with KbK_bKb​.

Flashcard 18: What happens to [OH−][OH^-][OH−] when a strong base is added to a weak base solution?

Flashcard 19: What is the equilibrium expression for a weak acid HA\text{HA}HA: HA⇌H++A−\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-HA⇌H++A−?

Flashcard 20: What is the common-ion effect in aqueous equilibrium systems?

Flashcard 21: What is the molar solubility sss of CaF2\text{CaF}_2CaF2​ in pure water in terms of KspK_{sp}Ksp​?

Flashcard 22: Assuming [F−]initial≫2s[\text{F}^-]_{\text{initial}} \gg 2s[F−]initial​≫2s, what is sss for CaF2\text{CaF}_2CaF2​ in [F−][\text{F}^-][F−] using KspK_{sp}Ksp​?

Flashcard 23: What is the molar solubility sss of AgCl\text{AgCl}AgCl in pure water in terms of KspK_{sp}Ksp​?

Flashcard 24: Which direction does B+H2O⇌BH++OH−\text{B}+\text{H}_2\text{O} \rightleftharpoons \text{BH}^+ + \text{OH}^-B+H2​O⇌BH++OH− shift when [BH+][\text{BH}^+][BH+] is increased?

Flashcard 25: Assuming [Cl−]initial≫s[\text{Cl}^-]_{\text{initial}} \gg s[Cl−]initial​≫s, what is sss for AgCl\text{AgCl}AgCl in [Cl−][\text{Cl}^-][Cl−] using KspK_{sp}Ksp​?

Flashcard 26: In AgCl(s)⇌Ag++Cl−\text{AgCl}(s) \rightleftharpoons \text{Ag}^+ + \text{Cl}^-AgCl(s)⇌Ag++Cl−, what happens to [Ag+][\text{Ag}^+][Ag+] when [Cl−][\text{Cl}^-][Cl−] is increased?

Flashcard 27: Which direction does HA⇌H++A−\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-HA⇌H++A− shift when [A−][\text{A}^-][A−] is increased?

Flashcard 28: What is the buffer relationship between conjugate pairs: HA\text{HA}HA and A−\text{A}^-A−, in terms of the common-ion effect?

Flashcard 29: Identify the common ion when BaSO4(s)\text{BaSO}_4(s)BaSO4​(s) is placed in a solution of Na2SO4(aq)\text{Na}_2\text{SO}_4(aq)Na2​SO4​(aq).

Flashcard 30: Identify the common ion when CaF2(s)\text{CaF}_2(s)CaF2​(s) is placed in a solution of NaF(aq)\text{NaF}(aq)NaF(aq).

Flashcard 1: State the equilibrium expression for a weak acid $HA$ with $K_a$ .

Flashcard 2: What happens to $[H^+]$ when a strong acid is added to a weak acid solution?

Flashcard 4: For $AgCl(s)$ , what happens to solubility when $NaCl(aq)$ is added?

Flashcard 5: What happens to $pH$ when $A^-$ (the conjugate base) is added to a buffer of $HA/A^-$ ?

Flashcard 6: For $CaF_2(s)$ , what happens to solubility when $NaF(aq)$ is added?

Flashcard 7: Identify the direction of shift when $NaOH$ is added to $NH_3(aq)$ .

Flashcard 8: Identify the direction of shift when $CH_3COONa$ is added to $CH_3COOH(aq)$ .

Flashcard 9: Which ion is the common ion when $NH_4Cl$ is added to a solution containing $NH_3$ ?

Flashcard 10: Which ion is the common ion when $NaF$ is added to a solution containing $HF$ ?

Flashcard 12: Which relationship is correct for a conjugate pair: $K_a$ and $K_b$ at $25^\circ C$ ?

Flashcard 13: What is the solubility product expression for $M(OH)_2(s)\rightleftharpoons M^{2+}+2OH^-$ ?

Flashcard 14: What is the solubility product expression for $MX(s)\rightleftharpoons M^+ + X^-$ ?

Flashcard 15: What is the net ionic equation for common-ion suppression of $B$ by adding $BH^+$ ?

Flashcard 16: What is the net ionic equation for common-ion suppression of $HA$ by adding $A^-$ ?

Flashcard 17: State the equilibrium expression for a weak base $B$ with $K_b$ .

Flashcard 18: What happens to $[OH^-]$ when a strong base is added to a weak base solution?

Flashcard 19: What is the equilibrium expression for a weak acid $\text{HA}$ : $\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-$ ?

Flashcard 21: What is the molar solubility $s$ of $\text{CaF}_2$ in pure water in terms of $K_{sp}$ ?

Flashcard 22: Assuming $[\text{F}^-]_{\text{initial}} \gg 2s$ , what is $s$ for $\text{CaF}_2$ in $[\text{F}^-]$ using $K_{sp}$ ?

Flashcard 23: What is the molar solubility $s$ of $\text{AgCl}$ in pure water in terms of $K_{sp}$ ?

Flashcard 24: Which direction does $\text{B}+\text{H}_2\text{O} \rightleftharpoons \text{BH}^+ + \text{OH}^-$ shift when $[\text{BH}^+]$ is increased?

Flashcard 25: Assuming $[\text{Cl}^-]_{\text{initial}} \gg s$ , what is $s$ for $\text{AgCl}$ in $[\text{Cl}^-]$ using $K_{sp}$ ?

Flashcard 26: In $\text{AgCl}(s) \rightleftharpoons \text{Ag}^+ + \text{Cl}^-$ , what happens to $[\text{Ag}^+]$ when $[\text{Cl}^-]$ is increased?

Flashcard 27: Which direction does $\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-$ shift when $[\text{A}^-]$ is increased?

Flashcard 28: What is the buffer relationship between conjugate pairs: $\text{HA}$ and $\text{A}^-$ , in terms of the common-ion effect?

Flashcard 29: Identify the common ion when $\text{BaSO}_4(s)$ is placed in a solution of $\text{Na}_2\text{SO}_4(aq)$ .

Flashcard 30: Identify the common ion when $\text{CaF}_2(s)$ is placed in a solution of $\text{NaF}(aq)$ .

Flashcard 1: State the equilibrium expression for a weak acid $HA$ with $K_a$ .

Flashcard 2: What happens to $[H^+]$ when a strong acid is added to a weak acid solution?

Flashcard 4: For $AgCl(s)$ , what happens to solubility when $NaCl(aq)$ is added?

Flashcard 5: What happens to $pH$ when $A^-$ (the conjugate base) is added to a buffer of $HA/A^-$ ?

Flashcard 6: For $CaF_2(s)$ , what happens to solubility when $NaF(aq)$ is added?

Flashcard 7: Identify the direction of shift when $NaOH$ is added to $NH_3(aq)$ .

Flashcard 8: Identify the direction of shift when $CH_3COONa$ is added to $CH_3COOH(aq)$ .

Flashcard 9: Which ion is the common ion when $NH_4Cl$ is added to a solution containing $NH_3$ ?

Flashcard 10: Which ion is the common ion when $NaF$ is added to a solution containing $HF$ ?

Flashcard 12: Which relationship is correct for a conjugate pair: $K_a$ and $K_b$ at $25^\circ C$ ?

Flashcard 13: What is the solubility product expression for $M(OH)_2(s)\rightleftharpoons M^{2+}+2OH^-$ ?

Flashcard 14: What is the solubility product expression for $MX(s)\rightleftharpoons M^+ + X^-$ ?

Flashcard 15: What is the net ionic equation for common-ion suppression of $B$ by adding $BH^+$ ?

Flashcard 16: What is the net ionic equation for common-ion suppression of $HA$ by adding $A^-$ ?

Flashcard 17: State the equilibrium expression for a weak base $B$ with $K_b$ .

Flashcard 18: What happens to $[OH^-]$ when a strong base is added to a weak base solution?

Flashcard 19: What is the equilibrium expression for a weak acid $\text{HA}$ : $\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-$ ?

Flashcard 21: What is the molar solubility $s$ of $\text{CaF}_2$ in pure water in terms of $K_{sp}$ ?

Flashcard 22: Assuming $[\text{F}^-]_{\text{initial}} \gg 2s$ , what is $s$ for $\text{CaF}_2$ in $[\text{F}^-]$ using $K_{sp}$ ?

Flashcard 23: What is the molar solubility $s$ of $\text{AgCl}$ in pure water in terms of $K_{sp}$ ?

Flashcard 24: Which direction does $\text{B}+\text{H}_2\text{O} \rightleftharpoons \text{BH}^+ + \text{OH}^-$ shift when $[\text{BH}^+]$ is increased?

Flashcard 25: Assuming $[\text{Cl}^-]_{\text{initial}} \gg s$ , what is $s$ for $\text{AgCl}$ in $[\text{Cl}^-]$ using $K_{sp}$ ?

Flashcard 26: In $\text{AgCl}(s) \rightleftharpoons \text{Ag}^+ + \text{Cl}^-$ , what happens to $[\text{Ag}^+]$ when $[\text{Cl}^-]$ is increased?

Flashcard 27: Which direction does $\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-$ shift when $[\text{A}^-]$ is increased?

Flashcard 28: What is the buffer relationship between conjugate pairs: $\text{HA}$ and $\text{A}^-$ , in terms of the common-ion effect?

Flashcard 29: Identify the common ion when $\text{BaSO}_4(s)$ is placed in a solution of $\text{Na}_2\text{SO}_4(aq)$ .

Flashcard 30: Identify the common ion when $\text{CaF}_2(s)$ is placed in a solution of $\text{NaF}(aq)$ .