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Chapter 7: Problem 1

Why is water an important solvent? Although you have not yet studied water in detail, can you think of some properties of water that make it so important?

Short Answer

Expert verified
Water is an important solvent because it dissolves more substances than any other liquid, making it significant in various biological processes. Its properties such as polarity, hydrogen bonding, high heat capacity, and cohesive and adhesive forces contribute to its ability to dissolve a wide range of substances and maintain stable environments for living organisms and chemical reactions.

Step by step solution

01

Introduction to Solvents

A solvent is a substance that dissolves another substance, called the solute, to form a solution. This is an essential process in many biological, chemical, and industrial processes. The solvent's properties determine how it interacts with the solute and how well it can dissolve the solute.
02

Importance of Water as a Solvent

Water is known as the "universal solvent" because it dissolves more substances than any other liquid. This property makes water extremely significant in many biological processes as the primary medium for chemical reactions, transportation of nutrients and waste products, and maintaining an ideal environment for living organisms.
03

Polarity of Water Molecules

Water (H鈧侽) molecules have a bent shape, with a slightly positive charge on the hydrogen atoms and a slightly negative charge on the oxygen atom. This uneven distribution of charges within the molecule makes it polar. The polarity of water molecules allows for strong interactions with other polar molecules and ions, helping them dissolve in water more easily.
04

Hydrogen Bonding in Water

Due to its polarity, water molecules can form hydrogen bonds with other water molecules and other polar molecules. This hydrogen bonding network contributes to water's high boiling and melting points, high heat capacity, and high surface tension. These properties make water an excellent solvent for polar solutes and contribute to its ability to dissolve many different substances.
05

Water's High Heat Capacity

Water has a high heat capacity, meaning it can absorb and release large amounts of heat before changing temperature. This property is important for maintaining stable temperatures in living organisms and the environment. In addition, dissolved molecules and ions can move more freely in a liquid with stable temperatures, leading to better solubility and transport properties.
06

Cohesion and Adhesion

Water molecules exhibit strong cohesive forces (attraction between similar molecules) and adhesive forces (attraction between different molecules). Because of these forces, water can move through narrow spaces, such as plant roots and blood vessels, and dissolve various substances as it travels. In conclusion, water's polarity, hydrogen bonding, high heat capacity, and cohesive and adhesive properties make it an essential solvent for many biological, chemical, and industrial processes.

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Most popular questions from this chapter

On the basis of the general solubility rules given in Table \(7.1,\) predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is likely, indicate which rules apply. a. iron(III) chloride, \(\mathrm{FeCl}_{3}\), and phosphoric acid, \(\mathrm{H}_{3} \mathrm{PO}_{4}\) b. barium nitrate, \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2},\) and sodium sulfate, \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) c. potassium chloride, \(\mathrm{KCl}\), and iron(II) sulfate, \(\mathrm{FeSO}_{4}\) d. lead(II) nitrate, \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2},\) and hydrochloric acid, \(\mathrm{HCl}\) e. calcium nitrate, \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2},\) and sodium chloride, \(\mathrm{NaCl}\) f. ammonium sulfide, \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S},\) and copper(II) chloride, \(\mathrm{CuCl}_{2}\)

What is a decomposition reaction? Give an example. Can such reactions also be classified in other ways?

The ionic compound produced when a strong acid and a strong base react is called a(n) ________.

For the reaction \(\mathrm{Mg}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{MgCl}_{2}(s),\) illustrate how electrons are gained and lost during the reaction.

What is a net ionic equation? What species are shown in such an equation, and which species are not shown?
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