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?

Verified step by step guidance

Calculate the moles of HCl in 50.0 mL of the solution. First, find the concentration of HCl in mol/L by converting 1.85 g/L to moles using the molar mass of HCl (36.46 g/mol).

Use the concentration of HCl to find the moles of HCl in 50.0 mL of the solution. Remember to convert mL to L by dividing by 1000.

Write the balanced chemical equation for the reaction: \( \text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O} \). Note that the reaction is a 1:1 molar ratio.

Use the moles of HCl to determine the moles of NaOH required, using the 1:1 molar ratio from the balanced equation.

Calculate the volume of 0.0850 M NaOH solution needed to provide the required moles of NaOH. Use the formula \( \text{Volume (L)} = \frac{\text{moles of NaOH}}{\text{concentration of NaOH (mol/L)}} \) and convert the volume from liters to milliliters.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

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 until the reaction reaches the equivalence point, where the amount of titrant equals the amount of substance in the sample. This process is often monitored using indicators or pH meters.

Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is a crucial concept in chemistry for calculating how much of a substance is present in a given volume of solution. In the context of titration, knowing the molarity of the titrant and the volume used allows for the calculation of the amount of solute in the analyte solution.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the relationships between the quantities of reactants and products in chemical reactions. It is essential for titration calculations, as it allows one to use balanced chemical equations to determine the proportions of reactants needed to reach the equivalence point. Understanding stoichiometry helps in calculating how much titrant is required based on the amount of analyte present.

Recommended video:

Guided course

01:16

Stoichiometry Concept

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: (b) 35.0 mL of 0.0850 M CH₃COOH?

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?

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.