Introduction to Acid-Base Reactions - AP Chemistry
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Calculate the pH given $[H^+] = 1 \times 10^{-8}$ M.
Calculate the pH given $[H^+] = 1 \times 10^{-8}$ M.
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$pH = 8$. Direct application: $pH = -\log(1 \times 10^{-8}) = 8$.
$pH = 8$. Direct application: $pH = -\log(1 \times 10^{-8}) = 8$.
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What is the main characteristic of a strong acid?
What is the main characteristic of a strong acid?
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A strong acid completely ionizes in solution. Nearly 100% ionization in aqueous solution.
A strong acid completely ionizes in solution. Nearly 100% ionization in aqueous solution.
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What is the $K_a$ value indicative of a strong acid?
What is the $K_a$ value indicative of a strong acid?
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A large $K_a$ value indicates a strong acid. Large $K_a$ means extensive ionization and stronger acidity.
A large $K_a$ value indicates a strong acid. Large $K_a$ means extensive ionization and stronger acidity.
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What is the $K_a$ expression for acetic acid, $CH_3COOH$?
What is the $K_a$ expression for acetic acid, $CH_3COOH$?
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$K_a = \frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$. Equilibrium expression for weak acid ionization.
$K_a = \frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$. Equilibrium expression for weak acid ionization.
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What is the relationship between $K_a$ and $K_b$ for a conjugate acid-base pair?
What is the relationship between $K_a$ and $K_b$ for a conjugate acid-base pair?
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$K_a \times K_b = K_w$. Fundamental relationship for conjugate acid-base pairs.
$K_a \times K_b = K_w$. Fundamental relationship for conjugate acid-base pairs.
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What is the pH of a 0.01 M HCl solution?
What is the pH of a 0.01 M HCl solution?
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$pH = 2$. Strong acid: $pH = -\log(0.01) = 2$.
$pH = 2$. Strong acid: $pH = -\log(0.01) = 2$.
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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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$pH + pOH = 14$. Derived from the water equilibrium constant at 25°C.
$pH + pOH = 14$. Derived from the water equilibrium constant at 25°C.
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What is the definition of an acid according to the Arrhenius theory?
What is the definition of an acid according to the Arrhenius theory?
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An acid is a substance that increases the concentration of $H^+$ ions in aqueous solution. Arrhenius theory focuses on $H^+$ ion production in water.
An acid is a substance that increases the concentration of $H^+$ ions in aqueous solution. Arrhenius theory focuses on $H^+$ ion production in water.
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Name the conjugate base of hydrochloric acid (HCl).
Name the conjugate base of hydrochloric acid (HCl).
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The conjugate base of HCl is $Cl^-$.. Formed by removing one proton from the acid.
The conjugate base of HCl is $Cl^-$.. Formed by removing one proton from the acid.
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What is the main characteristic of a strong base?
What is the main characteristic of a strong base?
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A strong base completely dissociates in solution. Nearly 100% dissociation in aqueous solution.
A strong base completely dissociates in solution. Nearly 100% dissociation in aqueous solution.
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Which ion is responsible for the acidity of a solution?
Which ion is responsible for the acidity of a solution?
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The $H^+$ ion is responsible for the acidity of a solution. Higher $[H^+]$ means lower pH and greater acidity.
The $H^+$ ion is responsible for the acidity of a solution. Higher $[H^+]$ means lower pH and greater acidity.
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Which ion is responsible for the basicity of a solution?
Which ion is responsible for the basicity of a solution?
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The $OH^-$ ion is responsible for the basicity of a solution. Higher $[OH^-]$ means higher pH and greater basicity.
The $OH^-$ ion is responsible for the basicity of a solution. Higher $[OH^-]$ means higher pH and greater basicity.
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Which is a stronger acid: HCl or acetic acid?
Which is a stronger acid: HCl or acetic acid?
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HCl is a stronger acid than acetic acid. HCl completely ionizes; acetic acid only partially ionizes.
HCl is a stronger acid than acetic acid. HCl completely ionizes; acetic acid only partially ionizes.
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What is the conjugate base of $H_2SO_4$?
What is the conjugate base of $H_2SO_4$?
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The conjugate base of $H_2SO_4$ is $HSO_4^-$. Sulfuric acid loses one proton to form bisulfate ion.
The conjugate base of $H_2SO_4$ is $HSO_4^-$. Sulfuric acid loses one proton to form bisulfate ion.
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What is the $K_b$ value indicative of a strong base?
What is the $K_b$ value indicative of a strong base?
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A large $K_b$ value indicates a strong base. Large $K_b$ means extensive ionization and stronger basicity.
A large $K_b$ value indicates a strong base. Large $K_b$ means extensive ionization and stronger basicity.
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Identify the $pH$ of a 0.1 M $KOH$ solution.
Identify the $pH$ of a 0.1 M $KOH$ solution.
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$pH = 13$. Strong base: $pOH = 1$, so $pH = 14 - 1 = 13$.
$pH = 13$. Strong base: $pOH = 1$, so $pH = 14 - 1 = 13$.
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Which ion forms when an acid donates a proton?
Which ion forms when an acid donates a proton?
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The conjugate base forms when an acid donates a proton. Result of proton donation in acid-base reactions.
The conjugate base forms when an acid donates a proton. Result of proton donation in acid-base reactions.
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Find the $K_a$ value given $pK_a = 3.5$.
Find the $K_a$ value given $pK_a = 3.5$.
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$K_a = 3.16 \times 10^{-4}$. Use formula: $K_a = 10^{-pK_a} = 10^{-3.5}$.
$K_a = 3.16 \times 10^{-4}$. Use formula: $K_a = 10^{-pK_a} = 10^{-3.5}$.
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What is the term for the equilibrium constant for water?
What is the term for the equilibrium constant for water?
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The term is $K_w$, the ion-product constant for water. Represents autoionization equilibrium of pure water.
The term is $K_w$, the ion-product constant for water. Represents autoionization equilibrium of pure water.
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Find the $K_b$ value given $pK_b = 4.5$.
Find the $K_b$ value given $pK_b = 4.5$.
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$K_b = 3.16 \times 10^{-5}$. Use formula: $K_b = 10^{-pK_b} = 10^{-4.5}$.
$K_b = 3.16 \times 10^{-5}$. Use formula: $K_b = 10^{-pK_b} = 10^{-4.5}$.
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State the formula for calculating pOH.
State the formula for calculating pOH.
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$pOH = -\text{log}[OH^-]$. Negative logarithm converts hydroxide concentration to pOH scale.
$pOH = -\text{log}[OH^-]$. Negative logarithm converts hydroxide concentration to pOH scale.
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Find the pOH of a solution where $pH = 3$.
Find the pOH of a solution where $pH = 3$.
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$pOH = 11$. Use relationship: $pH + pOH = 14$.
$pOH = 11$. Use relationship: $pH + pOH = 14$.
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Calculate the pOH given $[OH^-] = 1 \times 10^{-6}$ M.
Calculate the pOH given $[OH^-] = 1 \times 10^{-6}$ M.
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$pOH = 6$. Direct application: $pOH = -\log(1 \times 10^{-6}) = 6$.
$pOH = 6$. Direct application: $pOH = -\log(1 \times 10^{-6}) = 6$.
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Identify the $pH$ of a 0.1 M $HNO_3$ solution.
Identify the $pH$ of a 0.1 M $HNO_3$ solution.
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$pH = 1$. Strong acid: $pH = -\log(0.1) = 1$.
$pH = 1$. Strong acid: $pH = -\log(0.1) = 1$.
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What is the pH of a 0.01 M NaOH solution?
What is the pH of a 0.01 M NaOH solution?
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$pH = 12$. Strong base: $pOH = 2$, so $pH = 14 - 2 = 12$.
$pH = 12$. Strong base: $pOH = 2$, so $pH = 14 - 2 = 12$.
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Identify the Bronsted-Lowry definition of a base.
Identify the Bronsted-Lowry definition of a base.
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A Bronsted-Lowry base is a proton ($H^+$) acceptor. Bronsted-Lowry theory emphasizes proton transfer reactions.
A Bronsted-Lowry base is a proton ($H^+$) acceptor. Bronsted-Lowry theory emphasizes proton transfer reactions.
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What are the products of a neutralization reaction?
What are the products of a neutralization reaction?
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A salt and water are the products of a neutralization reaction. General form: acid + base → salt + water.
A salt and water are the products of a neutralization reaction. General form: acid + base → salt + water.
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What is the pH of a neutral solution at 25°C?
What is the pH of a neutral solution at 25°C?
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The pH of a neutral solution at 25°C is 7. At neutral pH, $[H^+] = [OH^-]$ at standard temperature.
The pH of a neutral solution at 25°C is 7. At neutral pH, $[H^+] = [OH^-]$ at standard temperature.
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What is the $K_a$ expression for acetic acid, $CH_3COOH$?
What is the $K_a$ expression for acetic acid, $CH_3COOH$?
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$K_a = \frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$. Equilibrium expression for weak acid ionization.
$K_a = \frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$. Equilibrium expression for weak acid ionization.
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What is the conjugate acid of $OH^-$?
What is the conjugate acid of $OH^-$?
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The conjugate acid of $OH^-$ is $H_2O$. Hydroxide ion gains one proton to form water.
The conjugate acid of $OH^-$ is $H_2O$. Hydroxide ion gains one proton to form water.
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