Calculate the pH and pOH of the following solutions. (a) 0.94 M HBr (b) 0.042 M Sr(OH)2 (c) 0.00

step 1 In answering this question, we have to recall that the pH is equal to negative lock, the concent

Calculate the pH and pOH of the following solutions. (a)...

Calculate the $\mathrm{pH}$ and $\mathrm{pOH}$ of the following solutions.
(a) $0.94 \mathrm{M} \mathrm{HBr}$
(b) $0.042 \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}$
(c) $0.00033 \mathrm{MHCl}$
(d) $0.88 M \mathrm{RbOH}$

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Key Concepts

pH and pOH Relationship

pH is a measure of the acidity of a solution while pOH measures its basicity. They are defined as pH = -log[H+] and pOH = -log[OH–]. At 25°C, the sum of pH and pOH is 14, which allows one to be calculated from the other, reflecting the inherent balance of hydrogen and hydroxide ions in aqueous solutions.

Stoichiometry in Dissociation Reactions

This concept emphasizes the importance of accounting for the stoichiometry of a compound’s dissociation. In some bases, a single formula unit can produce more than one hydroxide ion. Properly considering the stoichiometric coefficient is crucial when calculating ion concentrations, as it impacts the logarithmic functions used in determining pH or pOH.

Strong Acid and Base Dissociation

This concept refers to the idea that strong acids and bases completely dissociate in aqueous solution. For a strong acid, such as HBr or HCl, the concentration of hydronium ions ([H3O+]) is equal to the initial acid concentration. For a strong base, the concentration of hydroxide ions ([OH–]) is determined by multiplying the base’s molarity by the number of hydroxide ions it donates upon dissociation.

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