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  2. AP Chemistry
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What are the steps to calculate the pH of a strong acid solution?

  1. Determine the concentration of H+ ions (which equals the concentration of the strong acid). 2. Use the formula: pH = -log([H+]).
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What are the steps to calculate the pH of a strong acid solution?

  1. Determine the concentration of H+ ions (which equals the concentration of the strong acid). 2. Use the formula: pH = -log([H+]).

What are the steps to calculate the pH of a strong base solution?

  1. Determine the concentration of OH- ions (which equals the concentration of the strong base). 2. Use the formula: pOH = -log([OH-]). 3. Calculate pH using the relationship: pH = 14 - pOH.

Describe the process of calculating pH from [H+] .

  1. Identify the hydrogen ion concentration, [H+]. 2. Apply the formula: pH = -log[H+]. 3. Calculate the pH value.

Describe the process of calculating pOH from [OH-] .

  1. Identify the hydroxide ion concentration, [OH-]. 2. Apply the formula: pOH = -log[OH-]. 3. Calculate the pOH value.

What are the steps to determine pH from pOH?

  1. Obtain the pOH value. 2. Use the equation: pH = 14 - pOH. 3. Calculate the pH value.

What is the effect of increasing [H+] in a solution?

The pH decreases, making the solution more acidic.

What is the effect of increasing [OH-] in a solution?

The pOH decreases, and the pH increases, making the solution more basic.

What happens to pH if a strong acid is added to water?

The pH decreases significantly, as the concentration of H+ ions increases dramatically.

What happens to pOH if a strong base is added to water?

The pOH decreases significantly, as the concentration of OH- ions increases dramatically.

What is the effect of temperature increase on Kw?

Kw increases, meaning the autoionization of water is more favored at higher temperatures.

What are the key differences between pH and pOH?

pH: Measures acidity, based on [H+]. Lower pH = more acidic. | pOH: Measures basicity, based on [OH-]. Lower pOH = more basic.

Compare strong acids and weak acids in terms of dissociation.

Strong acids: Completely dissociate in water. | Weak acids: Partially dissociate in water, establishing an equilibrium.

Compare calculating the pH of a strong acid versus a weak acid.

Strong acid: pH calculated directly from the concentration of the acid. | Weak acid: pH calculated using the Ka expression and an ICE table.

What are the key differences between strong bases and weak bases?

Strong bases: Completely dissociate in water. | Weak bases: Partially dissociate in water, establishing an equilibrium.

Compare calculating the pOH of a strong base versus a weak base.

Strong base: pOH calculated directly from the concentration of the base. | Weak base: pOH calculated using the Kb expression and an ICE table.