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AP Chemistry Flashcards: Ph And Solubility

Study Ph And Solubility 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 Ph And Solubility, 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: Ph And Solubility

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QUESTION

State the KspK_{sp}Ksp​ expression for ZnSZnSZnS.

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ANSWER

Ksp=[Zn2+][S2−]K_{sp} = [Zn^{2+}][S^{2-}]Ksp​=[Zn2+][S2−]. 1:1 stoichiometry for ion products.

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Flashcard 1: State the KspK_{sp}Ksp​ expression for ZnSZnSZnS.

Answer: Ksp=[Zn2+][S2−]K_{sp} = [Zn^{2+}][S^{2-}]Ksp​=[Zn2+][S2−]. 1:1 stoichiometry for ion products.

Flashcard 2: What is the KspK_{sp}Ksp​ expression for Ca(OH)2Ca(OH)_2Ca(OH)2​?

Answer: Ksp=[Ca2+][OH−]2K_{sp} = [Ca^{2+}][OH^-]^2Ksp​=[Ca2+][OH−]2. Hydroxide ion squared due to formula stoichiometry.

Flashcard 3: Identify the KspK_{sp}Ksp​ expression for BaSO4BaSO_4BaSO4​.

Answer: Ksp=[Ba2+][SO42−]K_{sp} = [Ba^{2+}][SO_4^{2-}]Ksp​=[Ba2+][SO42−​]. 1:1 stoichiometry for ion products.

Flashcard 4: What is the definition of the solubility product constant (KspK_{sp}Ksp​)?

Answer: KspK_{sp}Ksp​ is the equilibrium constant for a solid dissolving in water. Represents dissolution equilibrium of ionic solids.

Flashcard 5: What is the pH of a solution with [H+]=1×10−3 M[H^+] = 1 \times 10^{-3} \text{ M}[H+]=1×10−3 M?

Answer: pH = 3. pH=−log⁡(10−3)=3pH = -\log(10^{-3}) = 3pH=−log(10−3)=3

Flashcard 6: What is the KspK_{sp}Ksp​ expression for CuSCuSCuS?

Answer: Ksp=[Cu2+][S2−]K_{sp} = [Cu^{2+}][S^{2-}]Ksp​=[Cu2+][S2−]. 1:1 stoichiometry for ion products.

Flashcard 7: What is the pH of a 0.1 M0.1 \text{ M}0.1 M NaOHNaOHNaOH solution?

Answer: pH = 13. Strong base: [OH−]=0.1[OH^-] = 0.1[OH−]=0.1, pOH=1pOH = 1pOH=1

Flashcard 8: What is the KspK_{sp}Ksp​ expression for Ag2CrO4Ag_2CrO_4Ag2​CrO4​?

Answer: Ksp=[Ag+]2[CrO42−]K_{sp} = [Ag^+]^2[CrO_4^{2-}]Ksp​=[Ag+]2[CrO42−​]. Silver ion squared due to formula stoichiometry.

Flashcard 9: Find the pH of a 0.075 M0.075 \text{ M}0.075 M Ba(OH)2Ba(OH)_2Ba(OH)2​ solution.

Answer: pH = 13.18. Diprotic base: [OH−]=0.15[OH^-] = 0.15[OH−]=0.15, pOH=0.82pOH = 0.82pOH=0.82

Flashcard 10: Determine the pOH of a solution with [OH−]=1×10−4 M[OH^-] = 1 \times 10^{-4} \text{ M}[OH−]=1×10−4 M.

Answer: pOH = 4. pOH=−log⁡(10−4)=4pOH = -\log(10^{-4}) = 4pOH=−log(10−4)=4

Flashcard 11: What is the KspK_{sp}Ksp​ expression for CaF2CaF_2CaF2​?

Answer: Ksp=[Ca2+][F−]2K_{sp} = [Ca^{2+}][F^-]^2Ksp​=[Ca2+][F−]2. Fluoride ion squared due to formula stoichiometry.

Flashcard 12: What is the pH of a 0.01 M0.01 \text{ M}0.01 M HClHClHCl solution?

Answer: pH = 2. Strong acid completely ionizes: [H+]=0.01[H^+] = 0.01[H+]=0.01

Flashcard 13: What is the KspK_{sp}Ksp​ expression for Mg(OH)2Mg(OH)_2Mg(OH)2​?

Answer: Ksp=[Mg2+][OH−]2K_{sp} = [Mg^{2+}][OH^-]^2Ksp​=[Mg2+][OH−]2. Hydroxide ion squared due to formula stoichiometry.

Flashcard 14: Determine the pH of a 0.025 M0.025 \text{ M}0.025 M HBrHBrHBr solution.

Answer: pH = 1.6. pH=−log⁡(0.025)=1.6pH = -\log(0.025) = 1.6pH=−log(0.025)=1.6

Flashcard 15: What is the pH of a solution with [H+]=1×10−7 M[H^+] = 1 \times 10^{-7} \text{ M}[H+]=1×10−7 M?

Answer: pH = 7. pH=−log⁡(10−7)=7pH = -\log(10^{-7}) = 7pH=−log(10−7)=7

Flashcard 16: What is the KspK_{sp}Ksp​ expression for PbSO4PbSO_4PbSO4​?

Answer: Ksp=[Pb2+][SO42−]K_{sp} = [Pb^{2+}][SO_4^{2-}]Ksp​=[Pb2+][SO42−​]. 1:1 stoichiometry for ion products.

Flashcard 17: Which solution has a higher pH: 0.1 M0.1 \text{ M}0.1 M HClHClHCl or 0.1 M0.1 \text{ M}0.1 M NaOHNaOHNaOH?

Answer: 0.1 M0.1 \text{ M}0.1 M NaOHNaOHNaOH. NaOHNaOHNaOH is basic with higher pH value.

Flashcard 18: What is the relationship between pH and pOH at 25°C?

Answer: pH+pOH=14pH + pOH = 14pH+pOH=14. Sum equals 14 at standard temperature.

Flashcard 19: What is the definition of pH?

Answer: pH is the negative logarithm of the hydrogen ion concentration: pH=−log[H+]pH = -\text{log}[H^+]pH=−log[H+]. It measures acidity using logarithmic scale.

Flashcard 20: Determine the KspK_{sp}Ksp​ expression for Fe(OH)3Fe(OH)_3Fe(OH)3​.

Answer: Ksp=[Fe3+][OH−]3K_{sp} = [Fe^{3+}][OH^-]^3Ksp​=[Fe3+][OH−]3. Hydroxide ion cubed due to formula stoichiometry.

Flashcard 21: Calculate the pH of a 0.1 M0.1 \text{ M}0.1 M CH3COOHCH_3COOHCH3​COOH solution, Ka=1.8×10−5K_a = 1.8 \times 10^{-5}Ka​=1.8×10−5.

Answer: pH ≈ 2.87. Weak acid requires ICE table calculation.

Flashcard 22: Calculate the pH of a 0.001 M0.001 \text{ M}0.001 M HNO3HNO_3HNO3​ solution.

Answer: pH = 3. Strong acid: pH=−log⁡(0.001)=3pH = -\log(0.001) = 3pH=−log(0.001)=3

Flashcard 23: State the formula for calculating pH from [H+][H^+][H+].

Answer: pH=−log[H+]pH = -\text{log}[H^+]pH=−log[H+]. Take negative log of hydrogen ion concentration.

Flashcard 24: State the formula for calculating pOH from [OH−][OH^-][OH−].

Answer: pOH=−log[OH−]pOH = -\text{log}[OH^-]pOH=−log[OH−]. Take negative log of hydroxide ion concentration.

Flashcard 25: What is the solubility product constant for PbI2PbI_2PbI2​?

Answer: Ksp=[Pb2+][I−]2K_{sp} = [Pb^{2+}][I^-]^2Ksp​=[Pb2+][I−]2. Iodide ion squared due to formula stoichiometry.

Flashcard 26: What is the KspK_{sp}Ksp​ expression for Hg2I2Hg_2I_2Hg2​I2​?

Answer: Ksp=[Hg22+][I−]2K_{sp} = [Hg_2^{2+}][I^-]^2Ksp​=[Hg22+​][I−]2. Iodide ion squared due to formula stoichiometry.

Flashcard 27: What is the KspK_{sp}Ksp​ expression for Ca(OH)2Ca(OH)_2Ca(OH)2​?

Answer: Ksp=[Ca2+][OH−]2K_{sp} = [Ca^{2+}][OH^-]^2Ksp​=[Ca2+][OH−]2. Hydroxide ion squared due to formula stoichiometry.

Flashcard 28: Identify the pH of a neutral solution at 25°C.

Answer: pH = 7. Equal concentrations of [H+][H^+][H+] and [OH−][OH^-][OH−].

Flashcard 29: What is the pH of a 0.02 M0.02 \text{ M}0.02 M KOHKOHKOH solution?

Answer: pH = 12.3. [OH−]=0.02[OH^-] = 0.02[OH−]=0.02, pOH=1.7pOH = 1.7pOH=1.7

Flashcard 30: What is the KspK_{sp}Ksp​ expression for Ag2SO4Ag_2SO_4Ag2​SO4​?

Answer: Ksp=[Ag+]2[SO42−]K_{sp} = [Ag^+]^2[SO_4^{2-}]Ksp​=[Ag+]2[SO42−​]. Silver ion squared due to formula stoichiometry.