Textbook Question
Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA. (a) How many moles of HA have been added at the equivalence point?
Ch.17 - Additional Aspects of Aqueous Equilibria
Chapter 17, Problem 41b
How many milliliters of 0.0850 M NaOH are required to titrate each of the following solutions to the equivalence point: (b) 35.0 mL of 0.0850 M CH3COOH?
Verified step by step guidance1
Identify the balanced chemical equation for the reaction: \( \text{CH}_3\text{COOH} + \text{NaOH} \rightarrow \text{CH}_3\text{COONa} + \text{H}_2\text{O} \). This shows a 1:1 molar ratio between acetic acid (CH3COOH) and sodium hydroxide (NaOH).
Calculate the moles of CH3COOH present in the solution using the formula: \( \text{moles} = \text{Molarity} \times \text{Volume (L)} \). Convert 35.0 mL to liters by dividing by 1000.
Since the reaction is a 1:1 molar ratio, the moles of NaOH required will be equal to the moles of CH3COOH calculated in the previous step.
Use the moles of NaOH and its molarity to find the volume required using the formula: \( \text{Volume (L)} = \frac{\text{moles}}{\text{Molarity}} \).
Convert the volume from liters to milliliters by multiplying by 1000 to find the final volume of NaOH solution needed for the titration.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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 solution until the reaction reaches its equivalence point, where the amount of titrant equals the amount of substance in the sample. This process is often indicated by a color change or a pH change.
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Acid-Base Titration
Molarity
Molarity (M) 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) and is crucial for calculations in titration, as it allows for the determination of how much of a titrant is needed to react with a given volume of analyte. Understanding molarity is essential for accurately calculating the volumes required in titration experiments.
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Neutralization Reaction
A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this context, acetic acid (CH₃COOH) reacts with sodium hydroxide (NaOH) in a 1:1 molar ratio. Recognizing the stoichiometry of the reaction is vital for determining the volume of NaOH needed to reach the equivalence point when titrating the acetic acid solution.
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Related Practice
Textbook Question
Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA. (b) What is the predominant form of B at the equivalence point?
Textbook Question
Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA. (c) Is the pH 7, less than 7, or more than 7 at the equivalence point?
Textbook Question
How many milliliters of 0.0850 M NaOH are required to titrate each of the following solutions to the equivalence point: (c) 50.0 mL of a solution that contains 1.85 g of HCl per liter?
Textbook Question
How many milliliters of 0.105 M HCl are needed to titrate each of the following solutions to the equivalence point: (a) 45.0 mL of 0.0950 M NaOH? (c) 125.0 mL of a solution that contains 1.35 g of NaOH per liter?
Textbook Question
How many milliliters of 0.105 M HCl are needed to titrate each of the following solutions to the equivalence point: (b) 22.5 mL of 0.118 M NH3?