The pH of a solution produced when an aqueous solution of strong acid pH 5 mixed with equal volu

step 1 Dear students, in Problem 68 of chapter 7, we've asked that the pH of the solution produced when

The pH of a solution produced when an aqueous solution of...

The $\mathrm{pH}$ of a solution produced when an aqueous solution of strong acid $\mathrm{pH} 5$ mixed with equal volume of an aqueous solution of strong acid of $\mathrm{pH} 3$ is
(1) $3.3$
(2) $3.5$
(3) $4.5$
(4) $4.0$

Key Concepts

The pH scale is a measure of the acidity or basicity of a solution, defined as the negative logarithm (base 10) of the hydrogen ion concentration. This scale compresses a wide range of hydrogen ion concentrations into a manageable number range, allowing chemists to easily compare the acidity or alkalinity of different solutions.

Strong Acid

A strong acid is one that completely dissociates into its ions in water, meaning that the concentration of hydrogen ions in the solution is equal to the initial concentration of the acid. This complete dissociation simplifies calculations involving acid-base reactions and pH determination.

Mixing Solutions and Dilution Calculations

When two solutions are mixed, the total amount of solute is the sum of the moles contributed by each solution, and the resulting concentration is calculated by dividing this total by the combined volume of the solutions. In the context of mixing strong acid solutions, this principle is crucial for determining the new hydrogen ion concentration after dilution.

Logarithmic Calculation in pH Determination

Calculating pH involves applying a logarithmic transformation to the hydrogen ion concentration, using the formula pH = -log[H+]. This logarithmic relationship enables the representation of a broad range of ion concentrations in a more convenient numerical form, which is essential for understanding and comparing the strength of acids and bases.

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