Question

A solution is created by measuring 3. 60 x 10-3 moles of NaOH and 5. 95 x 10-4 moles of HCl into a container and then water is added until the final volume is 1. 00 L. What is the pH of this solution? Please answer as quickly as possible

Answer 1

Answer: 11.478

Step-by-step explanation:

M = MBVB- MAVA/VA + VB

= number of moles of base - number of moles of acid/total volume

= 3.6*10^-3 - 5.95*10^-4/1

= 0.0036-0.000595 = 0.003005

[OH^-] = M = 0.003005M

POH = -log[OH^-]

= -log0.003005

= 2.522

PH = 14 - POH

= 14 - 2.522

= 11.478

Therefore, the pH of the solution is 11.478