Ch 9- Acids, Bases, Buffers Flashcards
A system is at equilibrium when the ratio of concentrations of the products to the reactions are _______.
equal
strong acids are _____% ionized in water
100%
what is the Kw value @ 25C
1 * 10 ^-14
How does the pH of a solution relate to pOH
pH + pOH = 14
What is the Henderson-Hasselbalch equation used for?
Calculating the pH of a buffer solution
Which of the following is a strong acid?
A) Acetic acid
B) Hydrochloric acid
C) Carbonic acid
D) Formic acid
B) Hydrochloric acid
what does Le Chatelier’s principle state?
if a system is no longer at equilibrium, it will react to re-establish equilibrium state
large K value means?
equilibrium favors products
K value less than one means?
equilibrium favors reactants
what is an amphiprotic species AND which is the most common?
can react as acid or base… WATER :)
The equilibrium constant for a reaction is denoted as
𝐾 and depends on the ____________ of the reaction.
temperature
What happens to the pH of a solution when a strong base is added?
A) It decreases
B) It remains the same
C) It increases
D) It becomes neutral
C) It increases
The equilibrium constant for a base equilibrium reaction is denoted as _____________.
A) 𝐾𝑎
B) 𝐾𝑏
C) 𝐾𝑤
D) 𝐾𝑝
B) 𝐾𝑏
In a buffer solution, the weak acid reacts with added ____________ to maintain pH.
base
The concentration of hydroxide ions in water is related to the ____________ constant 𝐾𝑤.
ionization
The Henderson-Hasselbalch equation calculates the pH of a buffer using the ratio of ____________ to weak acid.
conjugate base
Which of the following does NOT affect the pH of a solution?
A) Na⁺
B) Cl⁻
C) OH⁻
D) H⁺
A) Na⁺