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Chapter 4: Problem 1

Define solute, solvent, and solution by describing the process of dissolving a solid in a liquid.

Short Answer

Expert verified
A solute is the substance to be dissolved, a solvent is the substance in which the solute dissolves, and a solution is the mixture formed when a solute dissolves in a solvent. During the dissolving process, the solute's particles separate and distribute evenly within the solvent, forming the solution.

Step by step solution

01

Define 'Solute'

A solute is the substance that is to be dissolved. In the context of a solid dissolving in a liquid (for example, salt dissolving in water), the solid - salt - is the solute.
02

Define 'Solvent'

The solvent is the substance in which the solute dissolves. In this case, if we consider the example of salt dissolving in water, water is the solvent.
03

Define 'Solution'

A solution is the homogeneous mixture formed when a solute is dissolved in a solvent. It contains particles of two or more different substances that are uniformly distributed at a molecular level. Thus, when salt (solute) is dissolved in water (solvent), the resulting homogeneous mixture is the solution.
04

Describe the Dissolving Process

During the dissolving process, the particles of the solute (solid) separate and distribute uniformly within the solvent (liquid). This happens due to the interaction between the particles of the solute and the solvent. In the example of water and salt, the positive end of water molecules are attracted to the negative chloride ions of the salt, and the negative ends of the water molecules are attracted to the positive sodium ions. Because of these attractions, the water molecules surround and separate the salt particles, causing the salt to dissolve in water.

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Most popular questions from this chapter

Explain how you would prepare potassium iodide (KI) by means of (a) an acid- base reaction and (b) a reaction between an acid and a carbonate compound.

Determine how many grams of each of the following solutes would be needed to make \(2.50 \times 10^{2} \mathrm{~mL}\) of a \(0.100 M\) solution: (a) cesium iodide (CsI), (b) sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right),\) (c) sodium carbonate \(\left(\mathrm{Na}_{2} \mathrm{CO}_{3}\right),\) (d) potassium dichromate \(\left(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\right)\) (e) potassium permanganate \(\left(\mathrm{KMnO}_{4}\right)\).

Iron(II) can be oxidized by an acidic \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) solution according to the net ionic equation \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}+6 \mathrm{Fe}^{2+}+14 \mathrm{H}^{+} \longrightarrow\) \(2 \mathrm{Cr}^{3+}+6 \mathrm{Fe}^{3+}+7 \mathrm{H}_{2} \mathrm{O}\) If it takes \(26.0 \mathrm{~mL}\) of \(0.0250 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) to titrate \(25.0 \mathrm{~mL}\) of a solution containing \(\mathrm{Fe}^{2+},\) what is the molar concentration of \(\mathrm{Fe}^{2+} ?\)

How would you prepare \(60.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HNO}_{3}\) from a stock solution of \(4.00 \mathrm{M} \mathrm{HNO}_{3}\) ?

Explain why potassium permanganate \(\left(\mathrm{KMnO}_{4}\right)\) and potassium dichromate \(\left(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\right)\) can serve as internal indicators in redox titrations.
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