Problem: What is the pH of a 0.044 M HI solution?A) 3.12B) 12.64C) 10.88D) 15.36E) 1.36

FREE Expert Solution

We’re being asked to calculate the pH of a 0.044 M HI solution.

We can calculate pH using the following equation:

pH=-log H+

Take note that:         [H+] = [H3O+]

HI is one of the strong binary acids. Since HI is a strong acid, it will completely dissociate in the solution:

HI(aq) → H+(aq) + I-(aq)

Given:            [HI] = 0.044 M

Ratio:             1 mol of HI produces 1 mol of H+

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Problem Details

What is the pH of a 0.044 M HI solution?

A) 3.12

B) 12.64

C) 10.88

D) 15.36

E) 1.36

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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 Strong Acid-Base Calculations concept. If you need more Strong Acid-Base Calculations practice, you can also practice Strong Acid-Base Calculations practice problems.

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