Introduction to Acid-Base Reactions - AP Chemistry

State the formula for calculating pOH.

$pOH = -\text{log}[OH^-]$ . Negative logarithm converts hydroxide concentration to pOH scale.
What is the conjugate base of $H_2SO_4$ ?

The conjugate base of $H_2SO_4$ is $HSO_4^-$ . Sulfuric acid loses one proton to form bisulfate ion.
What is the $K_b$ value indicative of a strong base?

A large $K_b$ value indicates a strong base. Large $K_b$ means extensive ionization and stronger basicity.
What is the $K_b$ expression for ammonia, $NH_3$ ?

$K_b = \frac{[NH_4^+][OH^-]}{[NH_3]}$ . Equilibrium expression for weak base ionization.
Identify the $pH$ of a 0.1 M $HNO_3$ solution.

$pH = 1$ . Strong acid: $pH = -\log(0.1) = 1$ .
Find the pOH of a solution where $pH = 3$ .

$pOH = 11$ . Use relationship: $pH + pOH = 14$ .
What are the products of a neutralization reaction?

A salt and water are the products of a neutralization reaction. General form: acid + base → salt + water.
Which equation represents the ion-product constant for water ( $K_w$ )?

$K_w = [H^+][OH^-] = 1.0 \times 10^{-14}$ at 25°C. This equilibrium constant applies to pure water at 25°C.
Which ion forms when an acid donates a proton?

The conjugate base forms when an acid donates a proton. Result of proton donation in acid-base reactions.
What is the pH of a 0.01 M HCl solution?

$pH = 2$ . Strong acid: $pH = -\log(0.01) = 2$ .
What is the $K_a$ expression for acetic acid, $CH_3COOH$ ?

$K_a = \frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$ . Equilibrium expression for weak acid ionization.
What is the $K_a$ value indicative of a strong acid?

A large $K_a$ value indicates a strong acid. Large $K_a$ means extensive ionization and stronger acidity.
What is the relationship between $K_a$ and $K_b$ for a conjugate acid-base pair?

$K_a \times K_b = K_w$ . Fundamental relationship for conjugate acid-base pairs.
What is the main characteristic of a strong base?

A strong base completely dissociates in solution. Nearly 100% dissociation in aqueous solution.
What is the term for the equilibrium constant for water?

The term is $K_w$ , the ion-product constant for water. Represents autoionization equilibrium of pure water.
What is the definition of an acid according to the Arrhenius theory?

An acid is a substance that increases the concentration of $H^+$ ions in aqueous solution. Arrhenius theory focuses on $H^+$ ion production in water.
Identify the Lewis definition of a base.

A Lewis base is an electron pair donor. Lewis theory focuses on electron pair interactions.
Identify the Lewis definition of a base.

A Lewis base is an electron pair donor. Lewis theory focuses on electron pair interactions.
What is the pH of a neutral solution at 25°C?

The pH of a neutral solution at 25°C is 7. At neutral pH, $[H^+] = [OH^-]$ at standard temperature.
State the formula for calculating pH.

$pH = -\text{log}[H^+]$ . Negative logarithm converts concentration to pH scale.
Find the pOH of a solution where $pH = 3$ .

$pOH = 11$ . Use relationship: $pH + pOH = 14$ .
What is the $K_a$ expression for acetic acid, $CH_3COOH$ ?

$K_a = \frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$ . Equilibrium expression for weak acid ionization.
Calculate the pH given $[H^+] = 1 \times 10^{-8}$ M.

$pH = 8$ . Direct application: $pH = -\log(1 \times 10^{-8}) = 8$ .
Find the $K_a$ value given $pK_a = 3.5$ .

$K_a = 3.16 \times 10^{-4}$ . Use formula: $K_a = 10^{-pK_a} = 10^{-3.5}$ .
What is the $K_a$ value indicative of a strong acid?

A large $K_a$ value indicates a strong acid. Large $K_a$ means extensive ionization and stronger acidity.
What is the relationship between pH and pOH at 25°C?

$pH + pOH = 14$ . Derived from the water equilibrium constant at 25°C.
What is the $K_b$ value indicative of a strong base?

A large $K_b$ value indicates a strong base. Large $K_b$ means extensive ionization and stronger basicity.
Find the $K_a$ value given $pK_a = 3.5$ .

$K_a = 3.16 \times 10^{-4}$ . Use formula: $K_a = 10^{-pK_a} = 10^{-3.5}$ .
What are the products of a neutralization reaction?

A salt and water are the products of a neutralization reaction. General form: acid + base → salt + water.
What is the definition of a base according to the Arrhenius theory?

A base is a substance that increases the concentration of $OH^-$ ions in aqueous solution. Arrhenius theory focuses on $OH^-$ ion production in water.
Calculate the pH given $[H^+] = 1 \times 10^{-8}$ M.

$pH = 8$ . Direct application: $pH = -\log(1 \times 10^{-8}) = 8$ .
State the formula for calculating pH.

$pH = -\text{log}[H^+]$ . Negative logarithm converts concentration to pH scale.
Calculate the pOH given $[OH^-] = 1 \times 10^{-6}$ M.

$pOH = 6$ . Direct application: $pOH = -\log(1 \times 10^{-6}) = 6$ .
Which is a stronger base: NaOH or ammonia?

NaOH is a stronger base than ammonia. NaOH completely dissociates; ammonia only partially ionizes.
Name the conjugate base of hydrochloric acid (HCl).

The conjugate base of HCl is $Cl^-$ .. Formed by removing one proton from the acid.
State the formula for calculating pH.

$pH = -\text{log}[H^+]$ . Negative logarithm converts concentration to pH scale.
What is the $K_b$ value indicative of a strong base?

A large $K_b$ value indicates a strong base. Large $K_b$ means extensive ionization and stronger basicity.
What is the term for the equilibrium constant for water?

The term is $K_w$ , the ion-product constant for water. Represents autoionization equilibrium of pure water.
Which ion is responsible for the acidity of a solution?

The $H^+$ ion is responsible for the acidity of a solution. Higher $[H^+]$ means lower pH and greater acidity.
What is the pH of a 0.01 M NaOH solution?

$pH = 12$ . Strong base: $pOH = 2$ , so $pH = 14 - 2 = 12$ .
Which equation represents the ion-product constant for water ( $K_w$ )?

$K_w = [H^+][OH^-] = 1.0 \times 10^{-14}$ at 25°C. This equilibrium constant applies to pure water at 25°C.
What is the definition of an acid according to the Arrhenius theory?

An acid is a substance that increases the concentration of $H^+$ ions in aqueous solution. Arrhenius theory focuses on $H^+$ ion production in water.
Identify the Bronsted-Lowry definition of an acid.

A Bronsted-Lowry acid is a proton ( $H^+$ ) donor. Bronsted-Lowry theory emphasizes proton transfer reactions.
What is the main characteristic of a strong base?

A strong base completely dissociates in solution. Nearly 100% dissociation in aqueous solution.
Find the $K_b$ value given $pK_b = 4.5$ .

$K_b = 3.16 \times 10^{-5}$ . Use formula: $K_b = 10^{-pK_b} = 10^{-4.5}$ .
Which ion is responsible for the acidity of a solution?

The $H^+$ ion is responsible for the acidity of a solution. Higher $[H^+]$ means lower pH and greater acidity.
What is the definition of an acid according to the Arrhenius theory?

An acid is a substance that increases the concentration of $H^+$ ions in aqueous solution. Arrhenius theory focuses on $H^+$ ion production in water.
What is the term for the equilibrium constant for water?

The term is $K_w$ , the ion-product constant for water. Represents autoionization equilibrium of pure water.
What is the main characteristic of a strong acid?

A strong acid completely ionizes in solution. Nearly 100% ionization in aqueous solution.
What is the main characteristic of a strong acid?

A strong acid completely ionizes in solution. Nearly 100% ionization in aqueous solution.
What is the $K_b$ expression for ammonia, $NH_3$ ?

$K_b = \frac{[NH_4^+][OH^-]}{[NH_3]}$ . Equilibrium expression for weak base ionization.
What is the $K_a$ expression for acetic acid, $CH_3COOH$ ?

$K_a = \frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$ . Equilibrium expression for weak acid ionization.
What is the main characteristic of a strong acid?

A strong acid completely ionizes in solution. Nearly 100% ionization in aqueous solution.
Identify the Lewis definition of an acid.

A Lewis acid is an electron pair acceptor. Lewis theory focuses on electron pair interactions.
Identify the $pH$ of a 0.1 M $KOH$ solution.

$pH = 13$ . Strong base: $pOH = 1$ , so $pH = 14 - 1 = 13$ .
Name the conjugate base of hydrochloric acid (HCl).

The conjugate base of HCl is $Cl^-$ .. Formed by removing one proton from the acid.
Identify the $pH$ of a 0.1 M $HNO_3$ solution.

$pH = 1$ . Strong acid: $pH = -\log(0.1) = 1$ .
What is the pH of a neutral solution at 25°C?

The pH of a neutral solution at 25°C is 7. At neutral pH, $[H^+] = [OH^-]$ at standard temperature.
Which is a stronger base: NaOH or ammonia?

NaOH is a stronger base than ammonia. NaOH completely dissociates; ammonia only partially ionizes.
Calculate the pOH given $[OH^-] = 1 \times 10^{-6}$ M.

$pOH = 6$ . Direct application: $pOH = -\log(1 \times 10^{-6}) = 6$ .
Identify the Lewis definition of an acid.

A Lewis acid is an electron pair acceptor. Lewis theory focuses on electron pair interactions.
What is the main characteristic of a strong base?

A strong base completely dissociates in solution. Nearly 100% dissociation in aqueous solution.
What is the definition of a base according to the Arrhenius theory?

A base is a substance that increases the concentration of $OH^-$ ions in aqueous solution. Arrhenius theory focuses on $OH^-$ ion production in water.
What is the relationship between pH and pOH at 25°C?

$pH + pOH = 14$ . Derived from the water equilibrium constant at 25°C.
What is the $K_a$ value indicative of a strong acid?

A large $K_a$ value indicates a strong acid. Large $K_a$ means extensive ionization and stronger acidity.
Identify the Lewis definition of a base.

A Lewis base is an electron pair donor. Lewis theory focuses on electron pair interactions.
What is the $K_b$ expression for ammonia, $NH_3$ ?

$K_b = \frac{[NH_4^+][OH^-]}{[NH_3]}$ . Equilibrium expression for weak base ionization.
Which is a stronger acid: HCl or acetic acid?

HCl is a stronger acid than acetic acid. HCl completely ionizes; acetic acid only partially ionizes.
Identify the Lewis definition of an acid.

A Lewis acid is an electron pair acceptor. Lewis theory focuses on electron pair interactions.
Find the $K_b$ value given $pK_b = 4.5$ .

$K_b = 3.16 \times 10^{-5}$ . Use formula: $K_b = 10^{-pK_b} = 10^{-4.5}$ .
Find the $K_a$ value given $pK_a = 3.5$ .

$K_a = 3.16 \times 10^{-4}$ . Use formula: $K_a = 10^{-pK_a} = 10^{-3.5}$ .
Which ion is responsible for the acidity of a solution?

The $H^+$ ion is responsible for the acidity of a solution. Higher $[H^+]$ means lower pH and greater acidity.
What is the conjugate base of $H_2SO_4$ ?

The conjugate base of $H_2SO_4$ is $HSO_4^-$ . Sulfuric acid loses one proton to form bisulfate ion.
Identify the Bronsted-Lowry definition of a base.

A Bronsted-Lowry base is a proton ( $H^+$ ) acceptor. Bronsted-Lowry theory emphasizes proton transfer reactions.
Calculate the pH given $[H^+] = 1 \times 10^{-8}$ M.

$pH = 8$ . Direct application: $pH = -\log(1 \times 10^{-8}) = 8$ .
Which is a stronger base: NaOH or ammonia?

NaOH is a stronger base than ammonia. NaOH completely dissociates; ammonia only partially ionizes.
Which ion is responsible for the basicity of a solution?

The $OH^-$ ion is responsible for the basicity of a solution. Higher $[OH^-]$ means higher pH and greater basicity.
What is the pH of a 0.01 M NaOH solution?

$pH = 12$ . Strong base: $pOH = 2$ , so $pH = 14 - 2 = 12$ .
What is the pH of a 0.01 M HCl solution?

$pH = 2$ . Strong acid: $pH = -\log(0.01) = 2$ .
What are the products of a neutralization reaction?

A salt and water are the products of a neutralization reaction. General form: acid + base → salt + water.
Identify the $pH$ of a 0.1 M $HNO_3$ solution.

$pH = 1$ . Strong acid: $pH = -\log(0.1) = 1$ .
Name the conjugate base of hydrochloric acid (HCl).

The conjugate base of HCl is $Cl^-$ .. Formed by removing one proton from the acid.
What is the pH of a 0.01 M NaOH solution?

$pH = 12$ . Strong base: $pOH = 2$ , so $pH = 14 - 2 = 12$ .
Find the pH of a solution where $pOH = 4$ .

$pH = 10$ . Use relationship: $pH + pOH = 14$ .
Which ion is responsible for the basicity of a solution?

The $OH^-$ ion is responsible for the basicity of a solution. Higher $[OH^-]$ means higher pH and greater basicity.
Name the conjugate acid of ammonia (NH₃).

The conjugate acid of NH₃ is $NH_4^+$ . Formed by adding one proton to the base.
What is the conjugate acid of $OH^-$ ?

The conjugate acid of $OH^-$ is $H_2O$ . Hydroxide ion gains one proton to form water.
Which ion forms when an acid donates a proton?

The conjugate base forms when an acid donates a proton. Result of proton donation in acid-base reactions.
What is the pH of a neutral solution at 25°C?

The pH of a neutral solution at 25°C is 7. At neutral pH, $[H^+] = [OH^-]$ at standard temperature.
Identify the $pH$ of a 0.1 M $KOH$ solution.

$pH = 13$ . Strong base: $pOH = 1$ , so $pH = 14 - 1 = 13$ .
State the formula for calculating pOH.

$pOH = -\text{log}[OH^-]$ . Negative logarithm converts hydroxide concentration to pOH scale.
What is the relationship between $K_a$ and $K_b$ for a conjugate acid-base pair?

$K_a \times K_b = K_w$ . Fundamental relationship for conjugate acid-base pairs.
What is the relationship between $K_a$ and $K_b$ for a conjugate acid-base pair?

$K_a \times K_b = K_w$ . Fundamental relationship for conjugate acid-base pairs.
What is the conjugate acid of $OH^-$ ?

The conjugate acid of $OH^-$ is $H_2O$ . Hydroxide ion gains one proton to form water.
What is the pH of a 0.01 M HCl solution?

$pH = 2$ . Strong acid: $pH = -\log(0.01) = 2$ .
Which equation represents the ion-product constant for water ( $K_w$ )?

$K_w = [H^+][OH^-] = 1.0 \times 10^{-14}$ at 25°C. This equilibrium constant applies to pure water at 25°C.
Identify the Bronsted-Lowry definition of an acid.

A Bronsted-Lowry acid is a proton ( $H^+$ ) donor. Bronsted-Lowry theory emphasizes proton transfer reactions.
Identify the Bronsted-Lowry definition of an acid.

A Bronsted-Lowry acid is a proton ( $H^+$ ) donor. Bronsted-Lowry theory emphasizes proton transfer reactions.
Find the $K_b$ value given $pK_b = 4.5$ .

$K_b = 3.16 \times 10^{-5}$ . Use formula: $K_b = 10^{-pK_b} = 10^{-4.5}$ .
What is the relationship between pH and pOH at 25°C?

$pH + pOH = 14$ . Derived from the water equilibrium constant at 25°C.
Identify the Bronsted-Lowry definition of a base.

A Bronsted-Lowry base is a proton ( $H^+$ ) acceptor. Bronsted-Lowry theory emphasizes proton transfer reactions.
Which is a stronger acid: HCl or acetic acid?

HCl is a stronger acid than acetic acid. HCl completely ionizes; acetic acid only partially ionizes.
What is the conjugate acid of $OH^-$ ?

The conjugate acid of $OH^-$ is $H_2O$ . Hydroxide ion gains one proton to form water.
What is the conjugate base of $H_2SO_4$ ?

The conjugate base of $H_2SO_4$ is $HSO_4^-$ . Sulfuric acid loses one proton to form bisulfate ion.
What is the definition of a base according to the Arrhenius theory?

A base is a substance that increases the concentration of $OH^-$ ions in aqueous solution. Arrhenius theory focuses on $OH^-$ ion production in water.
Which ion is responsible for the basicity of a solution?

The $OH^-$ ion is responsible for the basicity of a solution. Higher $[OH^-]$ means higher pH and greater basicity.
Which is a stronger acid: HCl or acetic acid?

HCl is a stronger acid than acetic acid. HCl completely ionizes; acetic acid only partially ionizes.
Identify the $pH$ of a 0.1 M $KOH$ solution.

$pH = 13$ . Strong base: $pOH = 1$ , so $pH = 14 - 1 = 13$ .
Find the pOH of a solution where $pH = 3$ .

$pOH = 11$ . Use relationship: $pH + pOH = 14$ .
Identify the Bronsted-Lowry definition of a base.

A Bronsted-Lowry base is a proton ( $H^+$ ) acceptor. Bronsted-Lowry theory emphasizes proton transfer reactions.
Which ion forms when an acid donates a proton?

The conjugate base forms when an acid donates a proton. Result of proton donation in acid-base reactions.
State the formula for calculating pOH.

$pOH = -\text{log}[OH^-]$ . Negative logarithm converts hydroxide concentration to pOH scale.
Calculate the pOH given $[OH^-] = 1 \times 10^{-6}$ M.

$pOH = 6$ . Direct application: $pOH = -\log(1 \times 10^{-6}) = 6$ .

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