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 $6.00 \mathrm{M}$ HCl. A $75.00-\mathrm{mL}$ 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

Acid-Base Titration

Acid-base titration is an analytical technique used to determine the concentration of an acid or base by gradually adding a titrant of known concentration until the reaction reaches its equivalence point, often indicated by a pH change. This method relies on the precise stoichiometric reaction between the acid and base.

Stoichiometry of Neutralization Reaction

The stoichiometry of a neutralization reaction involves using the balanced chemical equation to relate the moles of acid to the moles of base that react completely. In acid-base reactions, such as between HCl and NaOH, the stoichiometric coefficients provide the necessary ratio to calculate unknown quantities like concentration or volume based on the moles of the reactants.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is a fundamental concept for preparing solutions, performing titrations, and understanding how the amount of a substance is distributed within a given volume, which is crucial in reaction calculations and dilutions.

Dilution Principle

The dilution principle states that when a solution is diluted, the number of moles of solute remains constant while the total volume increases, leading to a decrease in concentration. This concept is often applied using the equation M1V1 = M2V2, where the product of the initial concentration and volume equals that of the diluted solution.

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