Problem: What is the pH of a 0.34 M solution of a weak acid which has a pKa of 5.40?A. 2.9B. 3.9C. 2.0D. 1.7E. 1.6

FREE Expert Solution

We’re being asked to calculate the pH of a 0.34 M weak acid with pKa of 5.40.


Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case). The dissociation of HA is as follows:


HA(aq) + H2O(l)  H3O+(aq) + A(aq)



From this, we can construct an ICE table. Remember that liquids are ignored in the ICE table.




The Ka expression for HA is:


Ka=productsreactants=[H3O+][A-][HA]


Note that each concentration is raised by the stoichiometric coefficient: [HA], [H3O+] and [A] are raised to 1.


97% (311 ratings)
View Complete Written Solution
Problem Details

What is the pH of a 0.34 M solution of a weak acid which has a pKa of 5.40?

A. 2.9

B. 3.9

C. 2.0

D. 1.7

E. 1.6

Frequently Asked Questions

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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Guloy's class at UH.