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Chapter 4: Problem 16

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

Short Answer

Expert verified
In summary, an anion would be expected to be physically closer to the hydrogens of water molecules in solution because of the electrostatic interactions. The negatively charged anion is more attracted to the partially positively charged hydrogen atoms (δ+) in water molecules, while being repelled by the partially negatively charged oxygen atom (δ-).

Step by step solution

01

Understanding water molecule structure and charges

Water has a molecular structure with one oxygen atom bonded to two hydrogen atoms (H2O). The oxygen atom is more electronegative than the hydrogen atoms, meaning it attracts electron density towards itself, resulting in a partial negative charge (δ-) on the oxygen atom, and partial positive charges (δ+) on the hydrogen atoms.
02

Interaction of anions with water molecules

When an anion is present in a solution, it is negatively charged. The main force responsible for the interaction between the anion and water molecules is the electrostatic force, which is the force between charged particles. Electrostatic forces are governed by Coulomb's law, which states that unlike charges attract each other while like charges repel.
03

Determining the closest atom in water molecules to the anion

Considering the electrostatic forces, the negatively charged anion will be more attracted to the positively charged hydrogen atoms (δ+) of water molecules because of their opposite charges. Similarly, the anion will be repelled by the negatively charged oxygen atom (δ-) due to their like charges.
04

Final conclusion

Based on the electrostatic interactions between the anion and the water molecules, the anion would be expected to be physically closer to the hydrogens of water molecules in solution, as they have partial positive charges (δ+) that attract the negatively charged anion.

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Most popular questions from this chapter

Federal regulations set an upper limit of 50 parts per million (ppm) of \(\mathrm{NH}_{3}\) in the air in a work environment [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{MHCl} .\( The \)\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 \(10.0 \mathrm{~min}\) 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 \(1.20 \mathrm{~g} / \mathrm{L}\) 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?

A solid sample of \(\mathrm{Fe}(\mathrm{OH})_{3}\) is added to $0.500 \mathrm{~L}\( of \)0.250 \mathrm{M}\( aqueous \)\mathrm{H}_{2} \mathrm{SO}_{4}$. The solution that remains is still acidic. It is then titrated with $0.500 \mathrm{M} \mathrm{NaOH}\( solution, and it takes \)12.5 \mathrm{~mL}$ of the \(\mathrm{NaOH}\) solution to reach the equivalence point. What mass of \(\mathrm{Fe}(\mathrm{OH})_{3}\) was added to the $\mathrm{H}_{2} \mathrm{SO}_{4}$ solution?

(a) How many milliliters of \(0.120 \mathrm{M} \mathrm{HCl}\) are needed to completely neutralize \(50.0 \mathrm{~mL}\) of $0.101 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}$ solution? (b) How many milliliters of \(0.125 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) are needed to neutralize \(0.200 \mathrm{~g}\) of \(\mathrm{NaOH}\) ? (c) If $55.8 \mathrm{~mL}\( of a \)\mathrm{BaCl}_{2}$ solution is needed to precipitate all the sulfate ion in a \(752-\mathrm{mg}\) sample of $\mathrm{Na}_{2} \mathrm{SO}_{4}\(, what is the molarity of the \)\mathrm{BaCl}_{2}$ solution? (d) If \(42.7 \mathrm{~mL}\) of \(0.208 \mathrm{MHCl}\) solution is needed to neutralize a solution of \(\mathrm{Ca}(\mathrm{OH})_{2}\), how many grams of \(\mathrm{Ca}(\mathrm{OH})_{2}\) must be in the solution?

State whether each of the following statements is true or false. Justify your answer in each case. (a) Sulfuric acid is a monoprotic acid. (b) \(\mathrm{HCl}\) is a weak acid. (c) Methanol is a base.

State whether each of the following statements is true or false. Justify your answer in each case. (a) Electrolyte solutions conduct electricity because electrons are moving through the solution. (b) If you add a nonelectrolyte to an aqueous solution that already contains an electrolyte, the electrical conductivity will not change.
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