What is the pH of a solution prepared by diluting 25.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL?
A)1.00
B)1.60
C)2.00
D)3.20

Question

Quizplus · Accepted Answer

M1V1 = M2V2

where,
M1 = 0.10 M (initial concentration of HCl)
V1 = 25.00 mL (volume of initial HCl solution)
M2 = unknown
V2 = 100.00 mL (final volume of diluted HCl solution)

Rearranging the formula, we get:

M2 = M1V1/V2

M2 = (0.10 M)(25.00 mL)/(100.00 mL)

M2 = 0.025 M

Now, we can use the formula for pH of an acidic solution:

pH = -log[H+]

[H+] = 0.025 M (from the dissociation of HCl)

pH = -log(0.025)

pH = 1.60

Therefore, the pH of the diluted HCl solution is 1.60, which corresponds to choice B.

What Is the PH of a Solution Prepared by Diluting