What is the pH of a solution prepared by dissolving 96.1 g NaOH in enough water to make 3.2 L of solution?
A) 13.88
B) 0.12
C) 14.12
D) 10.28
E) none of these

Question

Quizplus · Accepted Answer

First, we need to calculate the number of moles of NaOH in the solution:
moles of NaOH = (mass of NaOH) / (molar mass of NaOH)
moles of NaOH = 96.1 g / 40.00 g/mol = 2.4025 mol

Next, we need to calculate the concentration of the NaOH solution in units of molarity (M):
Molarity = (moles of solute) / (liters of solution)
Molarity = 2.4025 mol / 3.2 L = 0.7508 M

Finally, we can use the fact that NaOH is a strong base to calculate the pH of the solution using the following equation:
pH = 14 - log[M]
pH = 14 - log[0.7508]
pH = 13.88

Therefore, the pH of the solution is 13.88, so the correct answer is A) 13.88.

What Is the PH of a Solution Prepared by Dissolving