A 10.0-mL sample of HNO3 was diluted to a volume of 100.00...

A $10.0-\mathrm{mL}$ sample of $\mathrm{HNO}_3$ was diluted to a volume of 100.00 mL . Then, 25 mL of that diluted solution were needed to neutralize 50.0 mL of 0.60 M KOH . What was the concentration of the original nitric acid?

Key Concepts

Dilution

Dilution involves adding solvent to a solution, which decreases its concentration while keeping the number of moles of solute constant. This concept is crucial when preparing a solution from a more concentrated stock and requires understanding the relationship between the initial and final volumes.

Titration

Titration is an analytical technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration. It involves measuring the volume of titrant needed to reach the equivalence point, whereby the moles of the reactive species in both solutions are stoichiometrically equal.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. In acid-base titrations, it allows one to calculate the concentrations and volumes of solutions by using the balanced chemical equation that describes the reaction.

Molarity

Molarity is a measure of concentration expressed as the number of moles of solute per liter of solution. It is fundamental in preparing solutions and in performing quantitative chemical analyses, such as titrations, where precise knowledge of the concentration is necessary.

Neutralization Reaction

A neutralization reaction is a type of chemical reaction in which an acid reacts with a base to produce a salt and water. In titration experiments, understanding the stoichiometry of the neutralization reaction is essential for determining the unknown concentration of the acid or base.

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