(a) What volume of 0.115 M HClO 4 solution is needed to neutralize 50.00 mL of 0.0875 M NaOH?

Identify the balanced chemical equation for the reaction: $$ \text{HClO}_4 + \text{NaOH} \rightarrow \text{NaClO}_4 + \text{H}_2\text{O} .. $$Determine the moles of NaOH using its concentration and volume: $$ \text{moles of NaOH} = \text{Molarity} \times \text{Volume} .. $$Since the reaction is a 1:1 molar ratio, the moles of HClO_{4} needed will be equal to the moles of NaOH.. Calculate the volume of HClO_{4} solution required using its concentration: $$ \text{Volume of HClO}_4 = \frac{\text{moles of HClO}_4}{\text{Molarity of HClO}_4} .. $$Convert the volume from liters to milliliters if necessary, as the final answer should be in milliliters.

(a) What volume of 0.115 M HClO4 solution is needed to neutralize 50.00 mL of 0.0875 M NaOH?

Identify the balanced chemical equation for the reaction: $$ \text{HClO}_4 + \text{NaOH} \rightarrow \text{NaClO}_4 + \text{H}_2\text{O} . $$Determine the moles of NaOH using its concentration and volume: $$ \text{moles of NaOH} = \text{Molarity} \times \text{Volume} . $$Since the reaction is a 1:1 molar ratio, the moles of HClO_{4} needed will be equal to the moles of NaOH. Calculate the volume of HClO_{4} solution required using its concentration: $$ \text{Volume of HClO}_4 = \frac{\text{moles of HClO}_4}{\text{Molarity of HClO}_4} . $$Convert the volume from liters to milliliters if necessary, as the final answer should be in milliliters.

Ch.4 - Reactions in Aqueous Solution

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.4 - Reactions in Aqueous Solution

Problem 81a

Chapter 4, Problem 81a

(a) What volume of 0.115 M HClO₄ solution is needed to neutralize 50.00 mL of 0.0875 M NaOH?

Verified step by step guidance

Identify the balanced chemical equation for the reaction: $ \text{HClO}_4 + \text{NaOH} \rightarrow \text{NaClO}_4 + \text{H}_2\text{O} $.

Determine the moles of NaOH using its concentration and volume: $ \text{moles of NaOH} = \text{Molarity} \times \text{Volume} $.

Since the reaction is a 1:1 molar ratio, the moles of HClO₄ needed will be equal to the moles of NaOH.

Calculate the volume of HClO₄ solution required using its concentration: $ \text{Volume of HClO}_4 = \frac{\text{moles of HClO}_4}{\text{Molarity of HClO}_4} $.

Convert the volume from liters to milliliters if necessary, as the final answer should be in milliliters.

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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, hydrochloric acid (HClO4) reacts with sodium hydroxide (NaOH) to form water and sodium perchlorate. Understanding this reaction is crucial for determining the stoichiometry involved in the neutralization process.

Molarity (M)

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). In this question, the molarity of both HClO4 and NaOH solutions is provided, which is essential for calculating the volume of acid needed to neutralize the base.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. For the neutralization of NaOH by HClO4, the stoichiometric coefficients indicate the ratio in which the reactants react. This concept is vital for determining the exact volume of HClO4 required to completely neutralize the given amount of NaOH.