Calculate the molar concentration of H3 O^+ions and the pH of the following solutions: (a) 25.0

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Calculate the molar concentration of H3 O^+ions and the pH...

Calculate the molar concentration of $\mathrm{H}_3 \mathrm{O}^{+}$ions and the pH of the following solutions: (a) $25.0 \mathrm{~cm}^3$ of $0.144 \mathrm{M} \mathrm{HCl}(\mathrm{aq})$ was added to $25.0 \mathrm{~cm}^3$ of $0.125 \mathrm{M} \mathrm{NaOH}(\mathrm{aq})$, (b) $25.0 \mathrm{~cm}^3$ of $0.15 \mathrm{M} \mathrm{HCl}(\mathrm{aq})$ was added to $35.0 \mathrm{~cm}^3$ of 0.15 M $\mathrm{KOH}(\mathrm{aq})$, (c) $21.2 \mathrm{~cm}^3$ of $0.22 \mathrm{~m} \mathrm{HNO}_3(\mathrm{aq})$ was added to $10.0 \mathrm{~cm}^3$ of $0.30 \mathrm{~m} \mathrm{NaOH}(\mathrm{aq})$.

Calculate the molar concentration of $\mathrm{H}_3 \mathrm{O}^{+}$ions and the pH of the following solutions:
(a) $25.0 \mathrm{~cm}^3$ of $0.144 \mathrm{M} \mathrm{HCl}(\mathrm{aq})$ was added to $25.0 \mathrm{~cm}^3$ of $0.125 \mathrm{M} \mathrm{NaOH}(\mathrm{aq})$, (b) $25.0 \mathrm{~cm}^3$ of $0.15 \mathrm{M} \mathrm{HCl}(\mathrm{aq})$ was added to $35.0 \mathrm{~cm}^3$ of 0.15 M $\mathrm{KOH}(\mathrm{aq})$, (c) $21.2 \mathrm{~cm}^3$ of $0.22 \mathrm{~m} \mathrm{HNO}_3(\mathrm{aq})$ was added to $10.0 \mathrm{~cm}^3$ of $0.30 \mathrm{~m} \mathrm{NaOH}(\mathrm{aq})$.

Key Concepts

Molar Concentration

Molar concentration, also known as molarity, is defined as the number of moles of a solute per liter of solution. It allows chemists to relate the volume of a solution to the amount of substance dissolved, which is crucial when performing quantitative analyses and reactions in solution.

Acid-Base Neutralization Reactions

Acid-base neutralization reactions involve the reaction between an acid and a base to produce water and a salt. In these reactions, protons (H? ions) from the acid combine with hydroxide ions (OH?) from the base, typically leading to the complete dissociation of both strong acids and strong bases.

Strong Acids and Strong Bases

Strong acids and strong bases are substances that completely dissociate in aqueous solution, meaning that their entire mole amount is available to react. This property simplifies calculations because the concentration of reactive ions is equal to the initial concentration of the acid or base.

Limiting Reagent

The concept of the limiting reagent is central to stoichiometry as it determines the extent of a chemical reaction. When two reactants are mixed, the reactant present in the lesser amount (in terms of stoichiometric equivalence) will be completely consumed, thus limiting the formation of products.

pH Calculation

pH is a measure of the acidity or basicity of a solution and is calculated as the negative logarithm (base 10) of the hydronium ion (H?O?) concentration. This calculation provides a convenient scale for understanding the degree of acidity in a solution, where lower pH values indicate higher acidity and higher pH values indicate higher basicity.

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