Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Problem 50

Calculate the mass of LiF in 100.0 \(\mathrm{mL}\) of 0.100 \(\mathrm{M}\) solution.

Short Answer

Expert verified
The mass of LiF in 100.0 \(\mathrm{mL}\) of 0.100 \(\mathrm{M}\) solution is 0.25938 g.

Step by step solution

01

Understand the problem

In this problem, it is important to understand what molarity (M) means. Molarity is the number of moles of solute per litre of solution.
02

Calculate the number of moles

The problem provides the volume of solution and its molarity. The volume is 100.0 ml, which is equivalent to 0.1L (as 1L = 1000 ml). The molarity is 0.100 M. Since molarity (M) = moles / volume (L), we can calculate the number of moles of LiF by multiplying the volume by the molarity. Thus, moles of LiF = volume (in L) * molarity = 0.1L * 0.100 M = 0.01 moles.
03

Calculate the mass of LiF

Once the number of moles is determined, we can calculate the mass using the molar mass of LiF. The molar mass of LiF = mass of Li + mass of F = 6.94 g/mol + 18.998 g/mol = 25.938 g/mol. Then, we multiply the number of moles by the molar mass to find the mass. So, mass = no. of moles * molar mass = 0.01 mol * 25.938 g/mol = 0.25938 g.

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

Would the compound BaSO \(_{4}\) be considered soluble in water?

What is the molarity of a solution that contains 20.0 g \(\mathrm{NaOH}\) in 2.00 \(\mathrm{L}\) of solution?

How many grams of glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6},\) are in 255 \(\mathrm{mL}\) of a 3.55 \(\mathrm{M}\) solution?

What kind of mixture is soap able to form in order to make oil and water soluble?

What are the two components of a solution, and how do they relate to each other?
See all solutions

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Making Measurements

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