pH and Solubility - AP Chemistry
Card 1 of 30
State the $K_{sp}$ expression for $ZnS$.
State the $K_{sp}$ expression for $ZnS$.
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$K_{sp} = [Zn^{2+}][S^{2-}]$. 1:1 stoichiometry for ion products.
$K_{sp} = [Zn^{2+}][S^{2-}]$. 1:1 stoichiometry for ion products.
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What is the $K_{sp}$ expression for $Ca(OH)_2$?
What is the $K_{sp}$ expression for $Ca(OH)_2$?
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$K_{sp} = [Ca^{2+}][OH^-]^2$. Hydroxide ion squared due to formula stoichiometry.
$K_{sp} = [Ca^{2+}][OH^-]^2$. Hydroxide ion squared due to formula stoichiometry.
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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 for ion products.
$K_{sp} = [Ba^{2+}][SO_4^{2-}]$. 1:1 stoichiometry for ion products.
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What is the definition of the solubility product constant ($K_{sp}$)?
What is the definition of the solubility product constant ($K_{sp}$)?
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$K_{sp}$ is the equilibrium constant for a solid dissolving in water. Represents dissolution equilibrium of ionic solids.
$K_{sp}$ is the equilibrium constant for a solid dissolving in water. Represents dissolution equilibrium of ionic solids.
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What is the pH of a solution with $[H^+] = 1 \times 10^{-3} \text{ M}$?
What is the pH of a solution with $[H^+] = 1 \times 10^{-3} \text{ M}$?
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pH = 3. $pH = -\log(10^{-3}) = 3$
pH = 3. $pH = -\log(10^{-3}) = 3$
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What is the $K_{sp}$ expression for $CuS$?
What is the $K_{sp}$ expression for $CuS$?
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$K_{sp} = [Cu^{2+}][S^{2-}]$. 1:1 stoichiometry for ion products.
$K_{sp} = [Cu^{2+}][S^{2-}]$. 1:1 stoichiometry for ion products.
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What is the pH of a $0.1 \text{ M}$ $NaOH$ solution?
What is the pH of a $0.1 \text{ M}$ $NaOH$ solution?
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pH = 13. Strong base: $[OH^-] = 0.1$, $pOH = 1$
pH = 13. Strong base: $[OH^-] = 0.1$, $pOH = 1$
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What is the $K_{sp}$ expression for $Ag_2CrO_4$?
What is the $K_{sp}$ expression for $Ag_2CrO_4$?
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$K_{sp} = [Ag^+]^2[CrO_4^{2-}]$. Silver ion squared due to formula stoichiometry.
$K_{sp} = [Ag^+]^2[CrO_4^{2-}]$. Silver ion squared due to formula stoichiometry.
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Find the pH of a $0.075 \text{ M}$ $Ba(OH)_2$ solution.
Find the pH of a $0.075 \text{ M}$ $Ba(OH)_2$ solution.
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pH = 13.18. Diprotic base: $[OH^-] = 0.15$, $pOH = 0.82$
pH = 13.18. Diprotic base: $[OH^-] = 0.15$, $pOH = 0.82$
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Determine the pOH of a solution with $[OH^-] = 1 \times 10^{-4} \text{ M}$.
Determine the pOH of a solution with $[OH^-] = 1 \times 10^{-4} \text{ M}$.
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pOH = 4. $pOH = -\log(10^{-4}) = 4$
pOH = 4. $pOH = -\log(10^{-4}) = 4$
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What is the $K_{sp}$ expression for $CaF_2$?
What is the $K_{sp}$ expression for $CaF_2$?
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$K_{sp} = [Ca^{2+}][F^-]^2$. Fluoride ion squared due to formula stoichiometry.
$K_{sp} = [Ca^{2+}][F^-]^2$. Fluoride ion squared due to formula stoichiometry.
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What is the pH of a $0.01 \text{ M}$ $HCl$ solution?
What is the pH of a $0.01 \text{ M}$ $HCl$ solution?
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pH = 2. Strong acid completely ionizes: $[H^+] = 0.01$
pH = 2. Strong acid completely ionizes: $[H^+] = 0.01$
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What is the $K_{sp}$ expression for $Mg(OH)_2$?
What is the $K_{sp}$ expression for $Mg(OH)_2$?
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$K_{sp} = [Mg^{2+}][OH^-]^2$. Hydroxide ion squared due to formula stoichiometry.
$K_{sp} = [Mg^{2+}][OH^-]^2$. Hydroxide ion squared due to formula stoichiometry.
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Determine the pH of a $0.025 \text{ M}$ $HBr$ solution.
Determine the pH of a $0.025 \text{ M}$ $HBr$ solution.
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pH = 1.6. $pH = -\log(0.025) = 1.6$
pH = 1.6. $pH = -\log(0.025) = 1.6$
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What is the pH of a solution with $[H^+] = 1 \times 10^{-7} \text{ M}$?
What is the pH of a solution with $[H^+] = 1 \times 10^{-7} \text{ M}$?
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pH = 7. $pH = -\log(10^{-7}) = 7$
pH = 7. $pH = -\log(10^{-7}) = 7$
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What is the $K_{sp}$ expression for $PbSO_4$?
What is the $K_{sp}$ expression for $PbSO_4$?
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$K_{sp} = [Pb^{2+}][SO_4^{2-}]$. 1:1 stoichiometry for ion products.
$K_{sp} = [Pb^{2+}][SO_4^{2-}]$. 1:1 stoichiometry for ion products.
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Which solution has a higher pH: $0.1 \text{ M}$ $HCl$ or $0.1 \text{ M}$ $NaOH$?
Which solution has a higher pH: $0.1 \text{ M}$ $HCl$ or $0.1 \text{ M}$ $NaOH$?
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$0.1 \text{ M}$ $NaOH$. $NaOH$ is basic with higher pH value.
$0.1 \text{ M}$ $NaOH$. $NaOH$ is basic with higher pH value.
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What is the relationship between pH and pOH at 25°C?
What is the relationship between pH and pOH at 25°C?
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$pH + pOH = 14$. Sum equals 14 at standard temperature.
$pH + pOH = 14$. Sum equals 14 at standard temperature.
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What is the definition of pH?
What is the definition of pH?
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pH is the negative logarithm of the hydrogen ion concentration: $pH = -\text{log}[H^+]$. It measures acidity using logarithmic scale.
pH is the negative logarithm of the hydrogen ion concentration: $pH = -\text{log}[H^+]$. It measures acidity using logarithmic scale.
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Determine the $K_{sp}$ expression for $Fe(OH)_3$.
Determine the $K_{sp}$ expression for $Fe(OH)_3$.
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$K_{sp} = [Fe^{3+}][OH^-]^3$. Hydroxide ion cubed due to formula stoichiometry.
$K_{sp} = [Fe^{3+}][OH^-]^3$. Hydroxide ion cubed due to formula stoichiometry.
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Calculate the pH of a $0.1 \text{ M}$ $CH_3COOH$ solution, $K_a = 1.8 \times 10^{-5}$.
Calculate the pH of a $0.1 \text{ M}$ $CH_3COOH$ solution, $K_a = 1.8 \times 10^{-5}$.
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pH ≈ 2.87. Weak acid requires ICE table calculation.
pH ≈ 2.87. Weak acid requires ICE table calculation.
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Calculate the pH of a $0.001 \text{ M}$ $HNO_3$ solution.
Calculate the pH of a $0.001 \text{ M}$ $HNO_3$ solution.
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pH = 3. Strong acid: $pH = -\log(0.001) = 3$
pH = 3. Strong acid: $pH = -\log(0.001) = 3$
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State the formula for calculating pH from $[H^+]$.
State the formula for calculating pH from $[H^+]$.
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$pH = -\text{log}[H^+]$. Take negative log of hydrogen ion concentration.
$pH = -\text{log}[H^+]$. Take negative log of hydrogen ion concentration.
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State the formula for calculating pOH from $[OH^-]$.
State the formula for calculating pOH from $[OH^-]$.
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$pOH = -\text{log}[OH^-]$. Take negative log of hydroxide ion concentration.
$pOH = -\text{log}[OH^-]$. Take negative log of hydroxide ion concentration.
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What is the solubility product constant for $PbI_2$?
What is the solubility product constant for $PbI_2$?
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$K_{sp} = [Pb^{2+}][I^-]^2$. Iodide ion squared due to formula stoichiometry.
$K_{sp} = [Pb^{2+}][I^-]^2$. Iodide ion squared due to formula stoichiometry.
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What is the $K_{sp}$ expression for $Hg_2I_2$?
What is the $K_{sp}$ expression for $Hg_2I_2$?
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$K_{sp} = [Hg_2^{2+}][I^-]^2$. Iodide ion squared due to formula stoichiometry.
$K_{sp} = [Hg_2^{2+}][I^-]^2$. Iodide ion squared due to formula stoichiometry.
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What is the $K_{sp}$ expression for $Ca(OH)_2$?
What is the $K_{sp}$ expression for $Ca(OH)_2$?
Tap to reveal answer
$K_{sp} = [Ca^{2+}][OH^-]^2$. Hydroxide ion squared due to formula stoichiometry.
$K_{sp} = [Ca^{2+}][OH^-]^2$. Hydroxide ion squared due to formula stoichiometry.
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Identify the pH of a neutral solution at 25°C.
Identify the pH of a neutral solution at 25°C.
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pH = 7. Equal concentrations of $[H^+]$ and $[OH^-]$.
pH = 7. Equal concentrations of $[H^+]$ and $[OH^-]$.
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What is the pH of a $0.02 \text{ M}$ $KOH$ solution?
What is the pH of a $0.02 \text{ M}$ $KOH$ solution?
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pH = 12.3. $[OH^-] = 0.02$, $pOH = 1.7$
pH = 12.3. $[OH^-] = 0.02$, $pOH = 1.7$
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What is the $K_{sp}$ expression for $Ag_2SO_4$?
What is the $K_{sp}$ expression for $Ag_2SO_4$?
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$K_{sp} = [Ag^+]^2[SO_4^{2-}]$. Silver ion squared due to formula stoichiometry.
$K_{sp} = [Ag^+]^2[SO_4^{2-}]$. Silver ion squared due to formula stoichiometry.
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