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Chapter 4: Problem 15

We have learned in this chapter that many ionic solids dissolve in water as strong electrolytes; that is, as separated ions in solution. Which statement is most correct about this process? (a) Water is a strong acid and therefore is good at dissolving ionic solids. (b) Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges. (c) The hydrogen and oxygen bonds of water are easily broken by ionic solids.

Short Answer

Expert verified
The correct answer is (b). Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges. Water molecules are polar, with partial positive charges near the Hydrogen atoms and partial negative charges near the Oxygen atom. This allows charged ions in ionic solids to interact with the partial charges on water molecules through solvation, thus facilitating the dissolution process.

Step by step solution

01

Look at option (a)

Water is a strong acid and therefore is good at dissolving ionic solids. This statement is incorrect. Water is not a strong acid, it's actually amphoteric meaning it can act both as an acid and a base. Moreover, the ability to dissolve ionic solids is not solely determined by the acidity of a substance.
02

Look at option (b)

Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges. This statement is correct. Water molecules are polar, meaning they have a partial positive charge near the Hydrogen atoms and a partial negative charge near the Oxygen atom. When ionic solids dissolve in water, the charged ions of the solid can interact with the partial charges on water molecules. This interaction is known as solvation, and it helps to stabilize the ions in solution, facilitating the dissolution process. So the correct answer is (b).
03

Look at option (c)

The hydrogen and oxygen bonds of water are easily broken by ionic solids. This statement is incorrect. The hydrogen and oxygen atoms in a water molecule are linked through covalent bonds, which are strong and not easily broken by ionic solids. The dissolution process involves interactions between the ions and the partial charges on water molecules, but it does not involve breaking actual H-O bonds within water molecules.

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Most popular questions from this chapter

Complete and balance the following molecular equations, and then write the net ionic equation for each: (a) \(\operatorname{HBr}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow\) (b) \(\mathrm{Cu}(\mathrm{OH})_{2}(s)+\mathrm{HClO}_{4}(a q) \longrightarrow\) (c) \(\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow\)

Separate samples of a solution of an unknown salt are treated with dilute solutions of \(\mathrm{HBr}, \mathrm{H}_{2} \mathrm{SO}_{4}\), and \(\mathrm{NaOH}\). A precipitate forms in all three cases. Which of the following cations could be present in the unknown salt solution: \(\mathrm{K}^{+}, \mathrm{Pb}^{2+}, \mathrm{Ba}^{2+}\) ?

Determine the oxidation number for the indicated element in each of the following substances: (a) \(\mathrm{S}\) in \(\mathrm{SO}_{2}\), (b) \(\mathrm{C}\) in \(\mathrm{COCl}_{2}\),

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens: $$ \begin{gathered} \mathrm{Br}_{2}(a q)+2 \mathrm{NaI}(a q) \longrightarrow 2 \mathrm{NaBr}(a q)+\mathrm{I}_{2}(a q) \\ \mathrm{Cl}_{2}(a q)+2 \mathrm{NaBr}(a q) \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{Br}_{2}(a q) \end{gathered} $$ (a) Which elemental halogen would you predict is the most stable, upon mixing with other halides? (b) Predict whether a reaction will occur when elemental chlorine and potassium iodide are mixed. (c) Predict whether a reaction will occur when elemental bromine and lithium chloride are mixed.

Would you expect that anions would be physically closer to the oxygen or to the hydrogens of water molecules that surround it in solution?
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