What is the pH of a solution that is 0.14 M in acetic acid, HC2H3O2, and 0.50 M
ID: 520114 • Letter: W
Question
What is the pH of a solution that is 0.14 M in acetic acid, HC2H3O2, and 0.50 M in sodium acetate, NaC2H3O2, at 25°C? Ka of acetic acid is 1.8 × 10^–5.
a. 4.19
b. 1.23
c. 4.74
d. 2.47
e. 5.30
What is the pH of a saturated solution of Zn(OH)2? For Zn(OH)2, Ksp = 2.1 × 10^–16.
a. 5.13
b. 8.57
c. 5.43
d. 8.87
e. 7.00
What is the pH of a solution prepared by adding 0.254 g of ammonium chloride to 115 mL of water? Kb of NH3 is 1.8 × 10^–5.
a. 5.32
b. 3.07
c. 7.00
d. 8.68
e. 10.93
The concentration of barium carbonate in a saturated aqueous solution of the salt at 25°C is 7.07× 10 ^-5M. What is the Ksp of this sparingly soluble salt?
a. 5×10^-9
b. 1.41 × 10^-12
c. 6.75 × 10^-16
d. 8.41 × 10^-3
e. 4.14 × 10^-2
Explanation / Answer
Q1. What is the pH of a solution that is 0.14 M in acetic acid, HC2H3O2, and 0.50 M in sodium acetate, NaC2H3O2, at 25°C? Ka of acetic acid is 1.8 × 10^–5.
this is a buffer so
pH = pKa + log(A-/HA)
where , A- = NaC2H3O2 and HA =HC2H3O2
pKa = -log(1.8*10^-5) = 4.75
substitute data
pH = pKa + log(A-/HA)
pH = 4.75+log(0.50/0.14)
pH = 5.30
choose E
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