Calculate the pH of a 0.575 M of sodium acetate. Use K_a of acetic acid Buffers

Question

Calculate the pH of a 0.575 M of sodium acetate. Use K_a of acetic acid Buffers ... A buffer solution is characterized by the ability to resist changes in pH when limited amounts of acid or base are added to it. A buffer is made by combining a weak acid with its conjugate base or a weak base with its conjugate acid. What is the pH of a buffer made by mixing 1.00 L of 0.020 M benzoic acid, HC_7 H_5 O_2, with 3.00 L of 0.060 M sodium benzoate, NaC_7 H_5 O_2? K_a for benzoic acid is 6.3 times 10^-5. Using Henderson-Hasselbalch equation (HHE) pH = pK_a + log [base]/[acid] What is the [H_3O^+] for a buffer solution that is 0.250 M in acid and 0.600 M in the corresponding salt if the weak acid K_a = 5.80 times 10^-7? 13. Practice 4: Calculate the pH of a solution containing 0.22 M acetic acid and 0.13 M sodium acetate. (K_a of acetic acid- 1.8 times10^-5) Practice 5:

Explanation / Answer

concentration of sodium acetate = 0.575 M

Ka of acetic acid = 1.8 x 10^-5

CH3COO-   +   H2O -----------------> CH3COOH +   OH-

0.575                                                      0                 0

0.575 - x                                                  x                  x

Kb = x^2 / 0.575 - x

5.56 x 10^-10 = x^2 / 0.575 - x

x = 1.786 x 10^-5

[OH-] = 1.786 x 10^-5 M

pOH = -log [OH-] = -log (1.786 x 10^-5)

pOH = 4.75

pH = 9.25

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