Problem: Determine the pH of each of the following solutions., 3.6×10−2 M HI, 9.23×10−2 M HClO4, a solution that is 4.0×10−2 M in HClO4 and 4.8×10−2 M in HCl, a solution that is 1.01% HCl by mass (Assume a density of 1.01 g/mL for the solution.)

FREE Expert Solution

We’re being asked to calculate the pH in each of the given solutions. We can calculate the pH using the following equation:

pH=-log H+

Take note that:         [H+] = [H3O+]


3.6×10−2 M HI

• HI is one of the strong binary acids
• strong acid →  completely dissociate in the solution:

HI(aq) → H+(aq) + I-(aq)

Given:            [HI] = 3.6×10−2 M

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

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Problem Details

Determine the pH of each of the following solutions., 3.6×10−2 M HI, 9.23×10−2 M HClO4, a solution that is 4.0×10−2 M in HClO4 and 4.8×10−2 M in HCl, a solution that is 1.01% HCl by mass (Assume a density of 1.01 g/mL for 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 Strong Acid-Base Calculations concept. If you need more Strong Acid-Base Calculations practice, you can also practice Strong Acid-Base Calculations practice problems.