Calculate the pH and pOH of the following solutions. (a) 0.0045 M Ba(OH)2 (b) 0.080 MHI (c) 0.03

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

Calculate the $\mathrm{pH}$ and $\mathrm{pOH}$ of the following solutions.
(a) $0.0045 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}$
(b) $0.080 \mathrm{MHI}$
(c) $0.030 \mathrm{M} \mathrm{Sr}(\mathrm{OH})_{2}$
(d) $12.3 \mathrm{M} \mathrm{HNO}_{3}$

Key Concepts

pH is a measure of the acidity of a solution, defined as the negative logarithm (base 10) of the hydrogen ion concentration in mol/L. It provides a quick and convenient way to specify how acidic or basic a solution is on a scale that typically ranges from 0 (very acidic) to 14 (very basic) in aqueous solutions at 25°C.

pOH

pOH is similar to pH but measures the basicity of a solution by taking the negative logarithm (base 10) of the hydroxide ion concentration. pOH complements pH, and together they can fully describe the acid-base nature of a solution.

Relationship Between pH and pOH

At standard conditions (25°C), the sum of pH and pOH is constant and equal to 14. This relationship derives from the ion-product constant for water (Kw = 1.0 × 10?¹?), allowing one to be calculated from the other.

Strong Acids and Bases

Strong acids and bases are substances that dissociate completely in water, meaning that the concentration of hydronium ions (from strong acids) or hydroxide ions (from strong bases) in the solution is directly proportional to the initial concentration of the acid or base introduced. Their complete dissociation simplifies the calculation of pH or pOH.

Dissociation Stoichiometry

In cases where the compound produces more than one ion per formula unit upon complete dissociation, it is important to account for the stoichiometry of the reaction. For example, a strong base that yields two hydroxide ions per formula unit will double the effective concentration of hydroxide ions, which must be considered when calculating pOH and subsequently pH.

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