Question

The pH of an aqueous solution that is 3.00% HCl by mass and has a density of 1.015 g/mL?

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2 points
0.078
4.5
7.8
0.78

Answer 1

[AI-generated answer — Bot GPT 3.5]

To calculate the pH of the solution, we need to first determine the molarity of the HCl solution.

Step 1: Calculate the molarity of the HCl solution.
Since the solution is 3.00% HCl by mass, we can assume that 100 g of the solution contains 3.00 g of HCl.
This means that if we have 100 g of the solution, we have 3.00 g of HCl. Therefore, the molarity of the HCl solution is:
3.00 g HCl / 36.46 g/mol = 0.08224 moles HCl
Volume of 100 g of the solution:
100 g / 1.015 g/mL = 98.52 mL = 0.09852 L
Molarity = moles / volume(L):
Molarity = 0.08224 mol / 0.09852 L ≈ 0.834 M

Step 2: Calculate the pH of the solution.
pH = -log[H+]
[H+] can be calculated from the molarity of the HCl solution.
[H+] = 0.834 M
pH = -log(0.834) = 0.078

Therefore, the pH of the solution is 0.078.

The correct answer is 0.078.