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Find the pH of each of the following solutions of mixtures of acids. Part A 0.120 M in HBr and 0.125 M in HCHO, Express yourPart B 0.170 M in HNO2 and 8.5x10-2 Min HNO3 Express your answer to two decimal places. IVO AQ R O 2 ? pH = 0.593 Submit PrevPart C 0.190 M in HCHO2 and 0.22 M in HC2H2O2 Express your answer to two decimal places. VO AQ R o 2 ? pH = 0.387 Submit PrevPart D 5.5x10-2 M in acetic acid and 5.5x10-2 M in hydrocyanic acid Express your answer to two decimal places. ? IVO AEQ * R

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Answer #1

Part A : pH = 0.920

Part B : pH = 1.07

Part C : pH = 2.62

Part D : pH = 3.01

Explanation

Part A : HBr is a very strong acid and dissociates completely whereas formic acid HCHO2 is a weak acid and does not dissociate completely.

Acid dissociation constant of HCHO2 = 1.8 x 10-4

We can safely assume that all H+ in solution comes from HBr

[H+] = [HBr] = 0.120 M

pH = -log[H+]

pH = -log(0.120 M)

pH = 0.920

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