What is the pH of the resulting solution if 25.00 ml of 0.10 M acetic acid is ad

Question

What is the pH of the resulting solution if 25.00 ml of 0.10 M acetic acid is added to 10.00 mL of 0.10 M NaOH? Assume that the volumes of the solutions are additive, K_a = 1.8 times 10^-5 for CH_3CO_2H. Calculate the pH of a solution formed by mixing 250.0 ml. of 0.15 M NH_4CI with 100.0 ml of 0.20 M NH_3. The K_b for NH_3 is 1.8 times 10^-5. A 1.00 L buffer solution is 0.150 M in HC_7H_5O_2 and 0.250 M in UC_7HSO_2 Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HC1 The K_a for HC_7H_5O_2. is 6.5 times 10^-5

Explanation / Answer

Question 1.

mmol of acid = MV = 25*0.1 = 2.5 mmol of acid

mmol of base = MV = 10*0.1 = 1 mmol of base

after neutralization

mmol of acid = 2.5-1 = 1.5

mmol of acetate formed = 0+1 = 1

apply buffer equation

pH = pKa + log(A-/HA)

pKa = -log(Ka) = -log(1.8*10^-5) = 4.75

substitute

pH = 4.75 + log(1/1.5) = 4.573

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