Vitamin C is ascorbic acid, HC6 H7 O6, which can be titrated with a strong base. HC6 H7 O6(aq)+N

step 1 Okay, here in this problem, ascorbic acid reacts with sodium hydroxide and that equation is give

Vitamin C is ascorbic acid, HC6 H7 O6, which can be titrated...

Vitamin $\mathrm{C}$ is ascorbic acid, $\mathrm{HC}_{6} \mathrm{H}_{7} \mathrm{O}_{6}$, which can be titrated with a strong base. $$ \mathrm{HC}_{6} \mathrm{H}_{7} \mathrm{O}_{6}(\mathrm{aq})+\mathrm{NaOH}(\mathrm{aq}) \longrightarrow \mathrm{NaC}_{6} \mathrm{H}_{7} \mathrm{O}_{6}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) $$ In a laboratory experiment, a student dissolved a 500.0-mg vitamin C tablet in $200.0 \mathrm{~mL}$ water and then titrated it with $0.1250 \mathrm{M} \mathrm{NaOH}$. It required $21.30 \mathrm{~mL}$ of the base to reach the equivalence point. What percentage of the mass of the tablet is impurity?

Vitamin $\mathrm{C}$ is ascorbic acid, $\mathrm{HC}_{6} \mathrm{H}_{7} \mathrm{O}_{6}$, which can be titrated with a strong base.
$$
\mathrm{HC}_{6} \mathrm{H}_{7} \mathrm{O}_{6}(\mathrm{aq})+\mathrm{NaOH}(\mathrm{aq}) \longrightarrow \mathrm{NaC}_{6} \mathrm{H}_{7} \mathrm{O}_{6}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)
$$
In a laboratory experiment, a student dissolved a 500.0-mg vitamin C tablet in $200.0 \mathrm{~mL}$ water and then titrated it with $0.1250 \mathrm{M} \mathrm{NaOH}$. It required $21.30 \mathrm{~mL}$ of the base to reach the equivalence point. What percentage of the mass of the tablet is impurity?

Key Concepts

Acid-Base Titration

Acid-base titration is a technique used to determine the concentration or amount of a substance by reacting it with a titrant of known concentration until the reaction reaches its equivalence point. It relies on the precise stoichiometric relationship between the reactants, allowing the calculation of an unknown quantity in the analyte solution.

Molarity

Molarity is a concentration unit defined as the number of moles of solute present per liter of solution. This fundamental concept is essential in titration because it relates the volume of the titrant used to the number of moles reacting, enabling quantitative analysis of the analyte.

Stoichiometry

Stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction. It enables the calculation of how much of each reactant is required to completely react with the other, based on the balanced chemical equation, and is crucial for determining the amount of substance participating in the reaction.

Equivalence Point

The equivalence point in a titration is the stage at which the added titrant has completely reacted with the analyte, according to the stoichiometric ratios given by the balanced chemical equation. Identifying the equivalence point is essential for accurate determination of the analyte’s concentration or mass.

Percentage Purity and Impurity Calculation

Percentage purity is calculated by comparing the amount of the desired pure substance to the total mass of a sample, expressed as a percentage. Conversely, the percentage of impurity is the complement, indicating the proportion of extraneous material relative to the whole sample. This calculation is important for assessing the quality and composition of a chemical sample.

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