Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 52

Describe the steps involved in preparing a solution of known molar concentration using a volumetric flask.

Short Answer

Expert verified
To prepare a solution of known molar concentration, first understand the concept of molarity. Calculate and measure the amount of solute needed using molarity formula. Add the solute to the volumetric flask using a funnel. Then add the solvent to the flask until it almost reaches the final volume mark, mix then add more solvent until it reaches the mark. Mix the solution thoroughly to ensure full dissolution of solute.

Step by step solution

01

Understanding Molarity

Molarity (M) is a measure of the concentration of a solute in a solution, or of any chemical species, in terms of amount of substance in a given volume. It is defined as the amount of moles of solute dissolved per litre of solution. The equation for molarity is: \( M = \frac{n}{V} \) where \( M \) is the molarity, \( n \) is the number of moles of solute, and \( V \) is the volume of the solution in litres.
02

Measuring the Solute

First, the quantity of solute needed should be calculated based on the desired molarity and volume. This can be done using the molarity formula. For example, to prepare 1L of 1M solution of Sodium Chloride (NaCl), one would need to measure out 1 mole of NaCl because \( 1M = \frac{1\, mole}{1\, Litre} \).
03

Adding the Solute to the Flask

After weighing the right amount of solute, add it into a clean, dry volumetric flask. This is typically done using a funnel to prevent any loss of solute.
04

Adding The Solvent to The Flask

Next, add solvent to the flask containing the solute. It's important to add the solvent in increments, especially when close to the mark on the flask indicating the final volume. The solvent is most commonly water.
05

Making Up The Volume and Mixing

Finally, add enough solvent to reach the mark on the neck of the flask which corresponds to the desired final volume (for example, the 1L mark). This is performed under careful inspection at eye level. After reaching the mark, secure the stopper on the flask and invert it several times to thoroughly mix the solution, ensuring that all the solute has been fully dissolved.

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) Without referring to Figure 4.10 , give the oxidation numbers of the alkali and alkaline earth metals in their compounds. (b) Give the highest oxidation numbers that the Groups \(3 \mathrm{~A}-7 \mathrm{~A}\) elements can have.

Give the oxidation number for the following species: \(\mathrm{H}_{2}, \mathrm{Se}_{8}, \mathrm{P}_{4}, \mathrm{O}, \mathrm{U}, \mathrm{As}_{4}, \mathrm{~B}_{12}\)

Identify the following as a weak or strong acid or base: (a) \(\mathrm{NH}_{3},\) (b) \(\mathrm{H}_{3} \mathrm{PO}_{4},\) (c) \(\mathrm{LiOH},\) d) \(\mathrm{HCOOH}\) (formic acid), (e) \(\mathrm{H}_{2} \mathrm{SO}_{4},\) (f) \(\mathrm{HF},(\mathrm{g}) \mathrm{Ba}(\mathrm{OH})_{2}\)

Describe the basic steps involved in an acid-base titration. Why is this technique of great practical value?

What is the difference between an ionic equation and a molecular equation?
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Physical Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Organic Chemistry

Read Explanation

Chemical Analysis

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