All Flashcards
What are the steps to calculate the pH of a strong acid solution?
- 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?
- 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+] .
- 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-] .
- 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?
- Obtain the pOH value. 2. Use the equation: pH = 14 - pOH. 3. Calculate the pH value.
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.
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.