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Chapter 4: Problem 121

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.

Short Answer

Expert verified
An experiment to determine solubility would involve dissolving a soluble compound in water until a saturated solution is formed. The amount of compound that dissolved in the water prior to saturation would represent its solubility.

Step by step solution

01

Understanding Solubility

Solubility refers to the maximum quantity of a solute that can dissolve in a particular solvent at a specific temperature to produce a saturated solution. It's usually expressed in grams per 100 grams of water.
02

Materials Needed

For this experiment, you need the soluble compound, distilled water, a glass beaker, a stirrer, a scale to measure weight, and a thermometer to measure the temperature.
03

Preparation

Measure and pour 100 grams of distilled water into the glass beaker. Measure a starting mass of the soluble compound. Make sure the water temperature is at a constant temperature before starting the experiment.
04

Dissolution Process

Start adding small amounts of the soluble compound to the water and stirring until no more of the compound can dissolve. This state is called a saturated solution.
05

Calculating Solubility

The solubility of the soluble compound can now be calculated by measuring the amount, in grams, of the compound that has completely dissolved in the water before reaching saturation. Solubility will be represented in grams of the solute per 100 grams of water.

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Most popular questions from this chapter

Describe the basic steps involved in diluting a solution of known concentration.

Give the oxidation number of the underlined atoms in the following molecules and ions: (a) \(\mathrm{Mg}_{3} \underline{\mathrm{N}}_{2}\) (b) \(\mathrm{CsO}_{2},\) (c) \(\mathrm{CaC}_{2}\), (d) \(\underline{\mathrm{CO}}_{3}^{2-}\), (e) \(\underline{\mathrm{C}}_{2} \mathrm{O}_{4}^{2-}\) (f) \(\mathrm{Zn} \underline{\mathrm{O}}_{2}^{2-}\) \((\mathrm{g}) \mathrm{NaBH}_{4},(\mathrm{~h}) \underline{\mathrm{W}} \mathrm{O}_{4}^{2-}\)

The recommended procedure for preparing a very dilute solution is not to weigh out a very small mass or measure a very small volume of a stock solution. Instead, it is done by a series of dilutions. A sample of \(0.8214 \mathrm{~g}\) of \(\mathrm{KMnO}_{4}\) was dissolved in water and made up to the volume in a 500-mL volumetric flask. A \(2.000-\mathrm{mL}\) sample of this solution was transferred to a \(1000-\mathrm{mL}\) volumetric flask and diluted to the mark with water. Next, \(10.00 \mathrm{~mL}\) of the diluted solution were transferred to a \(250-\mathrm{mL}\) flask and diluted to the mark with water. (a) Calculate the concentration (in molarity) of the final solution. (b) Calculate the mass of \(\mathrm{KMnO}_{4}\) needed to directly prepare the final solution.

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