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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.

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Most popular questions from this chapter

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?

Give the oxidation number of the underlined atoms in the following molecules and ions: (a) \(\underline{\mathrm{ClF}},\) (b) \(\underline{\mathrm{IF}}_{7}\), (c) \(\underline{\mathrm{CH}}_{4},\) (d) \(\underline{\mathrm{C}}_{2} \mathrm{H}_{2},\) (e) \(\underline{\mathrm{C}}_{2} \mathrm{H}_{4},\) (f) \(\mathrm{K}_{2} \mathrm{Cr} \mathrm{O}_{4},(\mathrm{~g}) \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) (h) \(\mathrm{KMnO}_{4},\) (i) \(\mathrm{NaHCO}_{3},(\mathrm{j}) \underline{\mathrm{L} i}_{2},(\mathrm{k}) \mathrm{NaIO}_{3},(\mathrm{l}) \mathrm{K} \underline{\mathrm{O}}_{2}\) \((\mathrm{m}) \underline{\mathrm{PF}}_{6}^{-},(\mathrm{n}) \mathrm{K} \underline{\mathrm{Au}} \mathrm{Cl}_{4}\)

You are given a water-soluble compound X. Describe how you would determine whether it is an electrolyte or a nonelectrolyte. If it is an electrolyte, how would you determine whether it is strong or weak? \(?\)

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