The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium hydroxide according to: CH3COOH1aq2 + NaOH1aq2¡ H2O1l2 + NaCH3COO1aq2 If 3.45 mL of vinegar needs 42.5 mL of 0.115 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.00-qt sample of this vinegar?

Key Concepts

Titration

Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant, a solution of known concentration, to a sample until the reaction reaches the equivalence point, where the amount of titrant equals the amount of substance in the sample. This method is commonly used in acid-base reactions to find the concentration of acids or bases.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (M) and is crucial for calculations in titration, as it allows for the determination of how much of a reactant is needed to react with a given amount of another substance. Understanding molarity is essential for converting volumes and concentrations during titration calculations.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the relationships between the quantities of reactants and products in a chemical reaction. It is based on the balanced chemical equation, which provides the mole ratios needed to calculate the amounts of substances involved. In the context of the titration question, stoichiometry is used to relate the volume and concentration of sodium hydroxide to the amount of acetic acid present in the vinegar.