Question

Calculate for 0.01 n solution of ch3co2na hydrolysis constant

Answer 1

For CH3COONa the equivalent wt. = molecular wt. so the concentration can taken as 0.01 M (For salts equivalent mass = formula mass/total charge of cation or anion.) Reaction of CH3COONa in water can be written as : CH3COONa + H2O ↔​ CH3COOH + Na+  + OH- So we need to calculate the conc. of OH- to get pH of salt solution. For calculating pH , at first we will find out the value of Kb using Ka Kw = KaKb 1.00 x 10-14 = (1.80 x 10-5) (Kb) Kb = 5.56 x​ 10-10 Use the Kb expression to calculate the [OH¯]: Kb = [Na+][OH-]/CH3COONa........(1) Let the change in concentration after dissociation is x, so the conc. of Na+, OH- would be x. Putting the valuesin eq (1) we get : 5.56 x 10-10 = [(x) (x)] / (0.01 - x) neglect the minus x x = 2.3 x 10-6 M =[OH-] = [Na+]  Calculate pOH, then pH: pOH = - log [2.3 x 10-6 M ] = 5.6 pH = 14 - pOH = 14 - 5.6 = 8.4

Answer 2

The solution is provided in the attachment.

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