Textbook Question
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?
Ch.17 - Additional Aspects of Aqueous Equilibria
Chapter 17, Problem 42b
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?
Verified step by step guidance1
Identify the balanced chemical equation for the reaction: \[ \text{NH}_3 + \text{HCl} \rightarrow \text{NH}_4\text{Cl} \].
Determine the moles of \( \text{NH}_3 \) present in the solution using the formula: \[ \text{moles of NH}_3 = M_1 \times V_1 \], where \( M_1 = 0.118 \text{ M} \) and \( V_1 = 22.5 \text{ mL} \) (convert \( V_1 \) to liters).
Since the reaction is a 1:1 molar ratio, the moles of \( \text{HCl} \) needed will be equal to the moles of \( \text{NH}_3 \).
Use the moles of \( \text{HCl} \) to find the volume of \( 0.105 \text{ M} \) \( \text{HCl} \) required: \[ V_2 = \frac{\text{moles of HCl}}{M_2} \], where \( M_2 = 0.105 \text{ M} \).
Convert the volume \( V_2 \) from liters to milliliters to find the final answer.
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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, depending on the type of titration.
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Acid-Base Titration
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 (mol/L) and is crucial for calculations in titration, as it allows for the determination of how much of a reactant is needed to completely react with a given volume of another reactant. 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 the context of titration, the acid (HCl) and the base (NH3) react in a stoichiometric ratio, which is determined by their balanced chemical equation. For strong acids and weak bases, the equivalence point is reached when the number of moles of acid equals the number of moles of base, allowing for the calculation of the required volume of acid to achieve neutralization.
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Related Practice
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
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added:
(a) 15.0 mL
(b) 19.9 mL.
Textbook Question
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added:
(c) 20.0 mL.
Textbook Question
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added: (e) 35.0 mL.