Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 69

Describe the basic steps involved in gravimetric analysis. How does this procedure help us determine the identity of a compound or the purity of a compound if its formula is known?

Short Answer

Expert verified
Gravimetric analysis involves precipitation, filtration, washing and drying, followed by weighing the precipitate to quantify the element or compound in the sample. This procedure aids in identifying compounds and assessing their purity by comparing observed measurements with expectations based on the compound's known formula.

Step by step solution

01

Define Gravimetric Analysis

Gravimetric analysis is a technique in analytical chemistry that focuses on the measurement of mass to calculate the amount of a particular element or compound in a sample.
02

Explain the Basic Steps Involved in Gravimetric Analysis

There are typically four main steps involved in a gravimetric analysis. Step 1: Precipitation - In this step, the analyte, or element to be identified or quantified, is converted into a solid by a chemical reaction. Step 2: Filtration - The sample is then filtered to remove any liquid and isolate the solid precipitate. Step 3: Washing and Drying - The precipitate is washed to remove impurities and then dried to get rid of any moisture. Step 4: Weighing - Finally, the precipitate is weighed, and its mass is used to calculate the amount of the original compound or element in the sample.
03

Outline the Role of Gravimetric Analysis in Compound Identification and Purity Assessment

Gravimetric analysis allows for identifying a compound by defining the sample's composition. Since the mass of the precipitate is directly related to the amount of the original element or compound in the sample, measuring this mass provides the quantity of a specific element or compound. As to determining the purity of a compound, if the formula of the compound is known, gravimetric analysis can help verify the amount of a particular element or compound in the sample. If the observed measurements match the theoretical predictions based on the known formula, the sample is pure. Differences between the expected and actual measurements can indicate impurities in the sample.

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

Phosphorus forms many oxoacids. Indicate the oxidation number of phosphorus in each of the following acids: (a) \(\mathrm{HPO}_{3},\) (b) \(\mathrm{H}_{3} \mathrm{PO}_{2},\) (c) \(\mathrm{H}_{3} \mathrm{PO}_{3},\) d) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (e) \(\mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7},\) (f) \(\mathrm{H}_{5} \mathrm{P}_{3} \mathrm{O}_{10}\).

Write ionic and net ionic equations for the following reactions: (a) \(\mathrm{AgNO}_{3}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\) (b) \(\mathrm{BaCl}_{2}(a q)+\mathrm{ZnSO}_{4}(a q) \longrightarrow\) (c) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(a q)+\mathrm{CaCl}_{2}(a q) \longrightarrow\)

Water is an extremely weak electrolyte and therefore cannot conduct electricity. Why are we often cautioned not to operate electrical appliances when our hands are wet?

Calculate the mass of precipitate formed when \(2.27 \mathrm{~L}\) of \(0.0820 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) are mixed with \(3.06 \mathrm{~L}\) of \(0.0664 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}\)

The concentration of \(\mathrm{Cu}^{2+}\) ions in the water (which also contains sulfate ions) discharged from a certain industrial plant is determined by adding excess sodium sulfide \(\left(\mathrm{Na}_{2} \mathrm{~S}\right)\) solution to \(0.800 \mathrm{~L}\) of the water. The molecular equation is $$ \mathrm{Na}_{2} \mathrm{~S}(a q)+\mathrm{CuSO}_{4}(a q) \longrightarrow_{\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\operatorname{CuS}(s)} $$ Write the net ionic equation and calculate the molar concentration of \(\mathrm{Cu}^{2+}\) in the water sample if \(0.0177 \mathrm{~g}\) of solid \(\mathrm{CuS}\) is formed.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemical Reactions

Read Explanation

Nuclear Chemistry

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic 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