A 25.00 mL sample of gastric juice is titrated with a 0.0210...

A 25.00 mL sample of gastric juice is titrated with a 0.0210 M NaOH solution. The titration to the equivalence point requires 26.4 mL of NaOH solution. If the equation for the reaction is $$ \mathrm{HCl}(\mathrm{aq})+\mathrm{NaOH}(\mathrm{aq}) \rightarrow \mathrm{NaCl}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell) $$ what is the molarity of HCl in the gastric juice?

A 25.00 mL sample of gastric juice is titrated with a 0.0210 M NaOH solution. The titration to the equivalence point requires 26.4 mL of NaOH solution. If the equation for the reaction is

$$
\mathrm{HCl}(\mathrm{aq})+\mathrm{NaOH}(\mathrm{aq}) \rightarrow \mathrm{NaCl}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(\ell)
$$

what is the molarity of HCl in the gastric juice?

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Key Concepts

Molarity

Molarity is a unit of concentration defined as the number of moles of solute per liter of solution. It is used to express how much substance is contained in a given volume of solution, which is essential for calculations in titrations and other quantitative chemical analyses.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to relate the moles of reactants to the moles of products. It provides the mole-to-mole ratios that enable the calculation of unknown concentrations in reactions, particularly at the equivalence point.

Titration

Titration is an analytical method used to determine the concentration of a solution by reacting it with another solution of known concentration. In acid-base titrations, a titrant of known molarity is gradually added to an analyte until the reaction reaches the point where neither component is in excess.

Equivalence Point

The equivalence point in a titration is the stage at which the moles of titrant added completely react with the moles of substance being titrated, based on the stoichiometry of the chemical reaction. At this point, the quantity of acid equals the quantity of base, according to the balanced reaction.

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