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).

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Tutorconsortium322 Tutorconsortium322 · Answer 1 · 2022-08-29T22:34:26+02:00

The pH of the original solution is 7.0.

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).

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.

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