A solution of NaOH with pH 13.68 requires 35.00 mL of 0.128 M HClO4 to reach the equivalence po

step 1 Okay, so we're going to react a strong acid with a strong base, and we're just going to go ahead

A solution of NaOH with pH 13.68 requires 35.00 mL of 0.128...

A solution of $\mathrm{NaOH}$ with $\mathrm{pH} 13.68$ requires $35.00 \mathrm{~mL}$ of $0.128 \mathrm{M} \mathrm{HClO}_{4}$ to reach the equivalence point. (a) What is the volume of the NaOH solution? (b) What is the $\mathrm{pH}$ at the equivalence point? (c) Calculate $\left[\mathrm{Na}^{+}\right]$ and $\left[\mathrm{ClO}_{4}^{-}\right]$ at the equivalence point. (Assume that volumes are additive.)

A solution of $\mathrm{NaOH}$ with $\mathrm{pH} 13.68$ requires $35.00 \mathrm{~mL}$ of $0.128 \mathrm{M} \mathrm{HClO}_{4}$ to reach the equivalence point.
(a) What is the volume of the NaOH solution?
(b) What is the $\mathrm{pH}$ at the equivalence point?
(c) Calculate $\left[\mathrm{Na}^{+}\right]$ and $\left[\mathrm{ClO}_{4}^{-}\right]$ at the equivalence point. (Assume that volumes are additive.)

Key Concepts

Stoichiometry in Titrations

Stoichiometry in titrations involves the quantitative relationship between the reactants – the acid and base – according to the balanced chemical equation. Knowing the volume and molarity of one reactant allows one to determine the moles of substance involved and then use the stoichiometric relationships to find volumes or concentrations of the other reactant. This principle is essential in solving for unknown quantities in titration problems.

Titration and Equivalence Point

A titration is a laboratory technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration. The equivalence point is reached when the amount of titrant added is exactly enough to completely neutralize the analyte, i.e., the acid and base react in exact stoichiometric proportions. Understanding the equivalence point is crucial for calculating concentrations and for selecting appropriate indicators or analytical techniques.

Molarity and Volume Additivity

Molarity, defined as moles of solute per liter of solution, is a measure of concentration that becomes particularly useful in titrations. When solutions are mixed during a titration, it is often assumed that their volumes are additive, meaning the total volume is the sum of the individual volumes. This assumption simplifies the calculation of resulting concentrations at various points in the titration since the diluting effect of mixing must be considered.

pH and pOH

The concepts of pH and pOH describe the acidity and basicity of a solution, respectively. pH is defined as the negative logarithm of the hydrogen ion concentration, while pOH is the negative logarithm of the hydroxide ion concentration. The two are related by the equation pH + pOH = 14 in aqueous solutions at room temperature, which allows for conversion between the two and is essential in understanding the behavior of acid–base systems.

Acid?Base Neutralization

Acid–base neutralization involves the reaction of an acid with a base to form water and a salt. In the case of strong acids and bases, the reaction goes to completion, meaning the acid and the base are fully consumed when they are present in stoichiometrically equivalent amounts. This concept is central to titrations, where an acid or base is gradually added until complete neutralization is achieved.

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