Question

Calculate the pH at

25°C

of a

0.77M

solution of potassium acetate

KCH3CO2

. Note that acetic acid

HCH3CO2

is a weak acid with a

pKa

of

4.76

.

Round your answer to

1

decimal place.

Calculate the pH at 25 °C of a 0.77 M solution of potassium acetate (KCH,CO2). Note that acetic acid (HCH,CO2 is a weak acid with a pK, of 4.76. Round your answer to 1 decimal place. pH = 0 5 ?

Answer 1

Please note that I have written p[OH] instead of pOH at places . It is just a mistake please ignore it.

SOLUTION Potassium acetate (KCH10) is a basic soll. When dissolved in water, the equilibrium that establishes kar (O + ho CH₂COOH + Of Kb[chyco01] [OH-] [K CH₂ CO2 Ch₂coon K CHCo, & Ho + OH ca Initial 0.77 Equilibrium 0.17 0.27 - n²-0.77 kb Sence n is very small s no Jourtky 2. [on] - 2017ko poH] = ₃ [pko - log 0.77] The question give pka but we need pkp. We know, pka + pkp= 144 pkp = 14-4676 = 9.24 o. Plow & [ 9.36] = 4.68 Hof solution - 1h-poH = 14- 4.68 = 9.3

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