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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 a substance that is dissolved in a solvent to create a solution. A solvent is the component that does the dissolving. A solution is the resulting homogeneous mixture of the solute and the solvent.

Step by step solution

01

Define Solute

The solute is the component of a solution that is dissolved in a solvent. In the context of a solid dissolving in a liquid, the solute would be the solid substance. For example, if you dissolve salt in water, the salt would be the solute.
02

Define Solvent

The solvent is the component of a solution that does the dissolving. In other words, it is the substance in which the solute is dissolved. In the example of salt dissolving in water, water would be the solvent.
03

Define Solution

A solution is a homogeneous mixture composed of two or more substances. In such a mixture, a solute is a substance dissolved in another substance, known as a solvent. Therefore, when the solute (salt) dissolves in the solvent (water), the resulting homogeneous mixture is referred to as a solution.

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Most popular questions from this chapter

Ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\) is one of the most important nitrogen-containing fertilizers. Its purity can be analyzed by titrating a solution of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) with a standard \(\mathrm{NaOH}\) solution. In one experiment a \(0.2041-\mathrm{g}\) sample of industrially prepared \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) required \(24.42 \mathrm{~mL}\) of \(0.1023 \mathrm{M} \mathrm{NaOH}\) for neutralization. (a) Write a net ionic equation for the reaction. (b) What is the percent purity of the sample?

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

What is the difference between an ionic equation and a molecular equation?

Identify each of the following species as a Bronsted acid, base, or both: (a) HI, (b) \(\mathrm{CH}_{3} \mathrm{COO}^{-}\), (c) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (d) \(\mathrm{HSO}_{4}^{-}\)

On the basis of oxidation number considerations, one of the following oxides would not react with molecular oxygen: \(\mathrm{NO}, \mathrm{N}_{2} \mathrm{O}, \mathrm{SO}_{2}, \mathrm{SO}_{3}, \mathrm{P}_{4} \mathrm{O}_{6}\). Which one is it? Why?
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