Problem: A 0.060 M solution of an acid has a pH of 5.12. Calculate the Ka of the acid. a. 1.04x109b. 1.26x10-4c. 9.59x10-10d. 7.58x10-6e. 9.6x10-11

FREE Expert Solution

We are being asked to calculate the Ka of a weak acid if 0.060 M solution of the weak acid has a pH of 5.12

We're going to represent the weak acid as HASince we’re dealing with a weak acid and Ka is an equilibrium expression, we will have to create an ICE chart to determine the equilibrium concentration of each species:

HAweak acidproton donor
H2O → will act as the weak baseproton acceptor


Equilibrium reaction:        HA(aq) + H2O(l)  A-(aq) + H3O+(aq)

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Problem Details

A 0.060 M solution of an acid has a pH of 5.12. Calculate the Ka of the acid. 

a. 1.04x109
b. 1.26x10-4
c. 9.59x10-10
d. 7.58x10-6
e. 9.6x10-11

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