# Problem: A solution of sodium acetate (NaCH3COO) has a pH of 9.53. The acid-dissociation constant for acetic acid is 1.8 x 10-5. What is the molarity of the solution?

###### FREE Expert Solution

We’re being asked to determine the molarity of the solution of sodium acetate (NaCH3COO) if the solution has a pH of 9.53 and the acid-dissociation constant for acetic acid is 1.8 x 10-5.

NaCH3COO is a salt and it will break up in the solution:

NaCH3COO → Na+(aq) + CH3COO-(aq)

CH3COO- is the conjugate base of a weak acid (CH3COOH):

CH3COOH    +   H2O(l)    →    CH3COOH-(aq)    +     H3O+(aq)
(weak acid)                                  (conjugate base)

Since we’re dealing with a weak base, we will have to create an ICE chart to determine the equilibrium concentration of each species:

CH3COO-weak baseproton acceptor
H2O → will act as the weak acidproton donor

Equilibrium reaction:        CH3COO-(aq) + H2O(l)  CH3COOH(aq) + OH-(aq)

85% (227 ratings) ###### Problem Details

A solution of sodium acetate (NaCH3COO) has a pH of 9.53. The acid-dissociation constant for acetic acid is 1.8 x 10-5. What is the molarity of the solution?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.

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Based on our data, we think this problem is relevant for Professor Davis' class at UCF.