(c) If 18.65 mLof the caesium hydroxide solution was needed to neutralize a42.3 mL aliquot of the hydroiodic acid solution, what is theconcentration (molarity) of the acid?

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Identify the balanced chemical equation for the reaction: \( \text{CsOH} + \text{HI} \rightarrow \text{CsI} + \text{H}_2\text{O} \).

Note that the reaction is a 1:1 molar ratio between CsOH and HI.

Use the formula for molarity: \( M = \frac{\text{moles of solute}}{\text{liters of solution}} \).

Calculate the moles of CsOH using its volume and molarity (if given or assumed).

Use the stoichiometry of the reaction to find the moles of HI, then calculate its molarity using the volume of the HI solution.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this case, hydroiodic acid (HI) reacts with caesium hydroxide (CsOH). The stoichiometry of the reaction is crucial for determining the relationship between the volumes and concentrations of the reactants.

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 (mol/L). To find the molarity of the hydroiodic acid, one must calculate the moles of caesium hydroxide used and relate it to the volume of the acid solution.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. It allows us to determine the amount of acid neutralized by the base. In this scenario, knowing the balanced equation helps in finding the molarity of the acid from the volume and concentration of the base used.

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