Question

A chemist makes four successive ten-fold dilutions of 1.0x10⁻⁵ M HCl. Calculate the pH of the original solution and of each diluted solution (through 1.0x10⁻⁹ M HCl).

Answer 1

The pH of the original solution is 7.0.

What is pH?

• An aqueous solution's acidity or basicity can be determined using the pH scale, which previously stood for "potential of hydrogen."
• In comparison to basic or alkaline solutions, acidic solutions are measured to have lower pH values.

• You need to know the hydronium ion concentration in moles per liter to determine the pH of an aqueous solution (molarity).

Calculation of pH:

At 25°C, in pure water [H₃O⁺] = 1.0 × 10⁻⁷ M

HCl after four successive ten-fold dilution = (1.0 × 10⁻⁵ M) × (1/10)⁴

= 1.0 × 10⁻⁹ M

[H₃O⁺] from HCl = 1.0 × 10⁻⁹ M ≪ 1.0 × 10⁻⁷ M

Hence, the pH of solution is almost entirely depends on the dissociation of water.

pH of the original solution = -log(1.0 × 10⁻⁷) = 7.0

Hence, the pH of the original solution is 7.0.

Learn more about pH here:

brainly.com/question/2288405

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