10.00 mL of 0.10 M NaOH is added to 25.00 mL of 0.10 M HCl during a titration
Which expression shows how to determine the Ht
concentration of the solution now?
A. 0.0025/0.025
B. 0.0025/0.035
C. O.0015/0.025
D. 0.0015/0.035

What is the pH of the solution after this addition?
(Write answer to two decimal places.)
pH =

Explanation:

10 mL = .01 L .

25 mL = .025 mL .

10 mL of .1 M NaOH will contain .01 x .1 = .001 moles

25 mL of .1M HCl will contain .025 x .1 = .0025 moles

acid will neutralise and after neutralisation moles of acid remaining

= .0025 - .001 = .0015 moles .

Total volume = .01 + .025 = .035 L

concentration of remaining HCl = .0015 / .035

Option D is correct.

= .042857 M

= 42.857 x 10⁻³ M .

pH = - log [42.857 x 10⁻³]

= 3 - log 42.857

= 3 - 1.632

= 1.368 .

don't understanding  .

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