Water is accidentally added to 350.00 mL of a stock solution of 6.00 M HCl. A 75.00-mL sample o

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Water is accidentally added to 350.00 mL of a stock...

Water is accidentally added to $350.00 \mathrm{~mL}$ of a stock solution of $6.00 \mathrm{M} \mathrm{HCl}$. A 75.00-mL sample of the diluted solution is titrated to $\mathrm{pH} 7.00$ with $78.8 \mathrm{~mL}$ of $4.85 \mathrm{M} \mathrm{NaOH}$. How much water was accidentally added? (Assume that volumes are additive.)

Key Concepts

Titration

Titration is a laboratory technique used to determine the unknown concentration of a solution. It involves gradually adding a solution of known concentration (titrant) to a measured volume of the solution of unknown concentration until the reaction reaches its equivalence point, which is often indicated by a specific pH or color change.

Acid-Base Neutralization

Acid-base neutralization is a reaction between an acid and a base where they combine to form water and a salt. The concept is fundamental in understanding how to calculate the reactant amounts needed for complete neutralization, often relying on the stoichiometry of the reaction and the concept of equivalence points.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions, based on the balanced chemical equation. It allows for the determination of the exact amounts of substances consumed and produced in a reaction, making it essential for calculations in titrations and other quantitative analyses.

Molarity

Molarity is the measure of the concentration of a solute in a solution, expressed as moles of solute per liter of solution. It is a key concept in solution chemistry, used to quantify how concentrated a solution is and to relate the amounts of reactants and products in chemical reactions.

Dilution

Dilution refers to the process of decreasing the concentration of a solute in a solution, usually by adding more solvent. Understanding dilution is important because it allows one to calculate the new concentration of a solution after an amount of solvent has been added, while assuming that the number of moles of solute remains constant.

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