40.00 mL of 0.300 M HBr is titrated with 0.300 M NaOH. What is the pH...

Question

Question

40.00 mL of 0.300 M HBr is titrated with 0.300 M NaOH.

What is the pH of the initial HBr solution? First determine the concentration of H+ in this solution.

Then, determine the pH of the solution, based on the H+ concentration.

science chemistry

Answer 1

Answer #1

A) initial concentration calculation:

[H+] = 40.00 mL x 10^-3 L x 0.300 M = 0.012 M

[OH-] = 0.300 M (Volume is not specified, hence i assume it is 1 L solution stock)

B) Only initial pH can be calculated from given data, since volme of NaOH is not specified

[H+] =0.012 M; pH = -log [H+] = -log [0.012] = 1.92

pH of the initial HBr solution pH = 1.92

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Answer 2

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