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Chapter 4: Problem 79

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 the steps of sample preparation, precipitation, isolation of the precipitate, drying, and weighing. This process helps determine the identity or purity of a compound by using the principles of stoichiometry to establish a relationship between the weight of the analyte and its formula. If the weight matches the expected weight based on the known formula, it confirms the identity or purity of the compound.

Step by step solution

01

Sample Preparation

This involves dissolving the sample in a solute to form a solution. This is done because the analyte must be in a solution before it can be analyzed.
02

Precipitation

A reagent is added to the solution which reacts with the analyte to form a precipitate. This reagent should be chosen such that it forms a precipitate with the analyte and nothing else in the solution.
03

Isolation of the Precipitate

The precipitate is then separated from the rest of the solution using a technique like filtration.
04

Drying and Weighing

The separated precipitate is then washed and dried. After the drying process, it is then weighed to find the exact amount of the analyte that was in the solution.
05

Calculation

Using the principles of stoichiometry, the weight of the analyte can be used to determine either its identity or purity. If the formula of the compound is known, the weight measured can confirm its identity (if the weight agrees with the expected weight) or determine its purity (by comparing the weight to the theoretical weight).

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Most popular questions from this chapter

A quantitative definition of solubility is the maximum number of grams of a solute that will dissolve in a given volume of water at a particular temperature. Describe an experiment that would enable you to determine the solubility of a soluble compound.

How many grams of \(\mathrm{NaCl}\) are required to precipitate most of the \(\mathrm{Ag}^{+}\) ions from \(2.50 \times 10^{2} \mathrm{~mL}\) of \(0.0113 M\) AgNO \(_{3}\) solution? Write the net ionic equation for the reaction.

Calculate the mass of \(\mathrm{KI}\) in grams required to prepare \(5.00 \times 10^{2} \mathrm{~mL}\) of a \(2.80 \mathrm{M}\) solution.

Chlorine forms a number of oxides with the following oxidation numbers: \(+1,+3,+4,+6,\) and +7 . Write a formula for each of these compounds.

A useful application of oxalic acid is the removal of rust \(\left(\mathrm{Fe}_{2} \mathrm{O}_{3}\right)\) from, say, bathtub rings according to the reaction \(\begin{aligned} \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+& 6 \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(a q) \longrightarrow \\ & 2 \mathrm{Fe}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}^{3-}(a q)+3 \mathrm{H}_{2} \mathrm{O}+6 \mathrm{H}^{+}(a q) \end{aligned}\) Calculate the number of grams of rust that can be removed by \(5.00 \times 10^{2} \mathrm{~mL}\) of a \(0.100 \mathrm{M}\) solution of oxalic acid.
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