Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 12: Problem 14

How many milliliters of a \(1.500 \mathrm{M}\) solution of \(\mathrm{NaCl}\) do you need to obtain \(100.0 \mathrm{~g}\) of \(\mathrm{NaCl} ?\)

Short Answer

Expert verified
To obtain \(100.0 ~\text{g}\) of NaCl from a \(1.500 ~\text{M}\) solution, you need \(1140 ~\text{mL}\) of the solution.

Step by step solution

01

Calculate the moles of NaCl needed

First, we need to determine the number of moles of NaCl that correspond to 100.0 g. We can calculate this using the formula moles = mass / molar mass. The molar mass of NaCl is approximately \(58.44 ~\text{g/mol}\) (22.99 g/mol for Na and 35.45 g/mol for Cl). \(moles = \dfrac{mass}{molar~mass} = \dfrac{100.0~g}{58.44 ~\text{g/mol}}\)
02

Use the Molarity Formula

Now, we will use the molarity formula: moles = molarity × volume. We will rearrange the formula to find the volume. \(volume = \dfrac{moles}{molarity}\) We know the molarity of the solution is 1.500 M, and we calculated the moles in the previous step.
03

Calculate the volume of the solution

Substitute the values obtained from Step 1 and the given molarity into the volume equation: \(volume = \dfrac{\dfrac{100.0~g}{58.44~\text{ g/mol}}}{1.500 ~\text{M}}\) Calculate the volume: \(volume = \dfrac{100.0}{(58.44)(1.500)} = \dfrac{100.0}{87.66} = 1.140 ~\text{L}\) To convert liters to milliliters, multiply by 1000. \((1.140~\text{L})\times 1000 = 1140 ~\text{mL}\)
04

State the final answer

The volume required to obtain 100.0 g of NaCl from a 1.500 M solution is \(1140 ~\text{mL}\).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

A solution of ethanol is prepared by combining \(22.5 \mathrm{~g}\) of ethanol with \(49.6 \mathrm{~g}\) of water. What is the percent composition by mass of alcohol in this solution?

The ionic lattice in which compound requires the most energy to break: \(\mathrm{KCl}, \mathrm{Mg}(\mathrm{OH})_{2}\), or \(\mathrm{NaNO}_{3}\) ? Explain your answer.

What is the volume in milliliters of \(0.0150 \mathrm{M}\) \(\mathrm{NaOH}\) solution required to neutralize \(50.0 \mathrm{~mL}\) of \(0.0100 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}(a q) ?\)

You have two solutions, one \(0.650 \mathrm{M}\) iron(III) nitrate and the other \(1.500 \mathrm{M}\) ammonium carbonate. (a) Write a net ionic equation for the precipitation reaction that occurs when these solutions are combined. (b) If you pour \(200.0 \mathrm{~mL}\) of each solution into the same flask, what is the theoretical yield of the precipitate in grams? (c) What is the molar concentration of the excess reactant ion?

Micelles are spherical, although they are usually drawn as a flat cross section (as shown on page 495). Why wouldn't micelles exist in water as flat, two-dimensional structures?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Kinetics

Read Explanation

Physical Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free