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What is the pH of a solution containing 0.155 mol/l of CH3COO- and 0.025 mol/l of...

What is the pH of a solution containing 0.155 mol/l of CH3COO- and 0.025 mol/l of HCL? (pKa of CH3COO- & CH3COOH is 4.76)

Homework Answers

Answer #1

we use following formulae to calculate the pH of solution

[H3O+] = c2+{(c2)2 + 4 Ka c1} / 2 where c2 = concerntration of weak acid ,

c1= concerntration of strong acid , Ka = equillibrium constant for weak acid

now putting values we get

[H3O+] =   0.155   +{(0.155)2 + 4 *4.76 * 0.025 } / 2

= 0.155 +   (0.024 + 0.476 )/2

= 0.155 + 0.5 /2 =

= (0.155 +  0.7 )/2 = 0.4275 mol/lit

pH= - log [H3O+] = -log [0.425] = - log (4.25 * 10-1) = -log 4.25 - log 10-1

pH = 0.628 +1 = 1.628

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