Given that the volume of the pure water is 480 mL and the mole of HCl added to the water is 2×10¯² mole. Therefore, the Initial and final pH of the water are:
1. The initial pH of the pure water is 7
2. The final pH of the water is 1.38
<h3>What is pH ? </h3>
This is simply a measure of the acidity / alkalinity of a solution.
The pH measures the hydrogen ion concentration while the pOH measures the hydroxide ion concentration
<h3>pH scale </h3>
The pH scale is a scale that gives an understanding of the variation of the acidity / alkalinity of a solution.
The scale ranges from 0 to 14 indicating:
- 0 to 6 indicates acid
- 7 indicates neutral (pure water)
- 8 to 14 indicate basic
<h3>How to determine the molarity </h3>
- Volume = 480 mL = 480 / 1000 = 0.48 L
- Mole of HCl = 2×10¯² mole
Molarity = mole / Volume
Molarity = 2×10¯² / 0.48
Molarity = 4.17×10¯² M
<h3>Dissociation equation </h3>
HCl(aq) —> H⁺(aq) + Cl¯(aq)
From the balanced equation above,
1 mole of HCl contains 1 mole of H⁺
Therefore,
4.17×10¯² M HCl will also contain 4.17×10¯² M H⁺
<h3>How to determine the pH </h3>
- Hydrogen ion concentration [H⁺] = 4.17×10¯² M
- pH =?
pH = –Log H⁺
pH = –Log 4.17×10¯²
pH = 1.38
Learn more about pH:
brainly.com/question/3709867
