What is the pH of a solution prepared by mixing 100.00 mL of 0.20 M HCl with 50.00 mL of 0.30 M HCl? Assume that the volumes are additive.
A)0.25
B)0.30
C)0.63
D)1.70

Question

Quizplus · Accepted Answer

First, we need to calculate the total moles of HCl used:

0.20 M HCl x 0.100 L = 0.020 moles HCl
0.30 M HCl x 0.050 L = 0.015 moles HCl
Total moles of HCl = 0.020 moles + 0.015 moles = 0.035 moles

Next, we need to calculate the total volume of the solution:

100.00 mL + 50.00 mL = 150.00 mL = 0.150 L

Finally, we can use the following formula to calculate the pH:

pH = -log[H+], where [H+] is the hydrogen ion concentration

In this case, the hydrogen ion concentration can be calculated using the following equation:

0.035 moles HCl / 0.150 L = 0.233 M [H+]

pH = -log(0.233) = 0.63

Therefore, the answer is C.

What Is the PH of a Solution Prepared by Mixing