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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 most correct statement about why ionic solids dissolve in water as strong electrolytes is option (b): "Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges." This is because water is a polar molecule with partial charges that can interact with ions, helping to dissolve ionic solids.

Step by step solution

01

Evaluate Option (a)

Consider the statement: "Water is a strong acid and therefore is good at dissolving ionic solids." Water is not a strong acid; in fact, it is considered neutral with a pH of 7. Therefore, this statement is incorrect.
02

Evaluate Option (b)

Consider the statement: "Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges." This statement is true. Water is a polar molecule, meaning it has a positive and a negative side (or partial charges). These partial charges can interact with ions, which helps to dissolve ionic solids. This statement appears to be a correct explanation for why ionic solids dissolve in water as strong electrolytes.
03

Evaluate Option (c)

Consider the statement: "The hydrogen and oxygen bonds of water are easily broken by ionic solids." This statement is not entirely correct. Although the hydrogen and oxygen bonds of water can be broken by ionic solids, it is the attraction between water molecules and ions that leads to the dissolution of the ionic solid, not the breaking of hydrogen and oxygen bonds within the water molecules.
04

Conclusion

Based on our evaluations of the three statements, the most correct statement about why ionic solids dissolve in water as strong electrolytes is option (b): "Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges."

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Most popular questions from this chapter

Acetone, \(\mathrm{CH}_{3} \mathrm{COCH}_{3},\) is a nonelectrolyte; hypochlorous \(\mathrm{acid}, \mathrm{HClO}\) , is a weak electrolyte; and ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl},\) is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? (b) If 0.1 mol of each compound is dissolved in solution, which one contains 0.2 mol of solute particles, which contains 0.1 mol of solute particles, and which contains somewhere between 0.1 and 0.2 mol of solute particles?

Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (a) HF, (b) acetonitrile,\(\mathrm{CH}_{3} \mathrm{CN},(\mathbf{c}) \mathrm{NaClO}_{4},(\mathbf{d}) \mathrm{Ba}(\mathrm{OH})_{2} .\)

Calicheamicin gamma-1, \(\mathrm{C}_{55} \mathrm{H}_{74} \mathrm{IN}_{3} \mathrm{O}_{21} \mathrm{S}_{4},\) is one of the most potent antibiotics known: one molecule kills one bacterial cell. Describe how you would (carefully!) prepare 25.00 \(\mathrm{mL} .\) of an aqueous calicheamicin gamma-1 solution that could kill \(1.0 \times 10^{8}\) bacteria, starting from a \(5.00 \times 10^{-9} M\) stock solution of the antibiotic.

Federal regulations set an upper limit of 50 parts per million \((\mathrm{ppm})\) of \(\mathrm{NH}_{3}\) in the air in a work environment \([\mathrm{that}\) is, 50 molecules of \(\mathrm{NH}_{3}(g)\) for every million molecules in the air]. Air from a manufacturing operation was drawn through a solution containing \(1.00 \times 10^{2} \mathrm{mL}\) of 0.0105 \(\mathrm{M}\) HCl. The \(\mathrm{NH}_{3}\) reacts with HCl according to: $$\mathrm{NH}_{3}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{NH}_{4} \mathrm{Cl}(a q)$$ After drawing air through the acid solution for 10.0 min at a rate of 10.0 \(\mathrm{L} / \mathrm{min}\) , the acid was titrated. The remaining acid needed 13.1 \(\mathrm{mL}\) of 0.0588 \(\mathrm{M} \mathrm{NaOH}\) to reach the equivalence point. (a) How many grams of \(\mathrm{NH}_{3}\) were drawn into the acid solution? (b) How many ppm of \(\mathrm{NH}_{3}\) were in the air? (Air has a density of 1.20 g/L and an average molar mass of 29.0 \(\mathrm{g} / \mathrm{mol}\) under the conditions of the experiment.) (c) Is this manufacturer in compliance with regulations?

State whether each of the following statements is true or false. Justify your answer in each case. \begin{equation} \begin{array}{l}{\text { (a) When methanol, } \mathrm{CH}_{3} \mathrm{OH}, \text { is dissolved in water, a con- }} \\ {\text { ducting solution results. }} \\ {\text { (b) When acetic acid, } \mathrm{CH}_{3} \mathrm{COOH} \text { , dissolves in water, the }} \\ {\text { solution is weakly conducting and acidic in nature. }}\end{array} \end{equation}
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