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Chapter 4: Problem 17

Differentiate between what happens when the following are added to water a. polar solute versus nonpolar solute b. KF versus \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) c. RbCl versus AgCl d. \(\mathrm{HNO}_{3}\) versus \(\mathrm{CO}\)

Short Answer

Expert verified
When added to water: a) Polar solutes dissolve due to hydrogen bonds or electrostatic interactions, while nonpolar solutes don't dissolve or dissolve poorly. b) Both KF (ionic) and C6H12O6 (polar) are soluble, but KF dissociates into ions, whereas C6H12O6 stays as individual molecules. c) RbCl (ionic) dissolves into ions, while AgCl has low solubility due to its lattice structure. d) HNO3 makes the solution acidic by ionizing, while CO has little effect as it is nonpolar and does not interact strongly with water.

Step by step solution

01

a. Polar vs Nonpolar solute

Polar solutes have a charged or polar functional group, which allows them to form hydrogen bonds or electrostatic interactions with water molecules. This results in them being soluble in water. On the other hand, nonpolar solutes do not have polar functional groups, so they do not form strong interactions with water. This often makes them insoluble or less soluble in water.
02

b. KF vs. C6H12O6

KF is potassium fluoride, an ionic compound, which will dissociate into potassium (K+) and fluoride (F-) ions when added to water. These ions will then become hydrated by the water molecules, leading to a homogeneous solution. C6H12O6 is glucose, a polar molecule with multiple hydroxyl (OH) groups that can form hydrogen bonds with water, making it soluble. Both KF and C6H12O6 are soluble in water, but KF dissociates into ions while C6H12O6 remains as individual molecules.
03

c. RbCl vs. AgCl

RbCl is rubidium chloride, an ionic compound that will dissolve in water by breaking down into its constituent ions, Rb+ and Cl-. Similar to KF, these ions will then become hydrated by water molecules, resulting in a homogeneous solution. Conversely, AgCl (silver chloride) has low solubility in water due to its strong ionic lattice structure, which is not easily broken down by the hydration energy of the water molecules. AgCl will only marginally dissolve in water, producing a saturated solution with undissolved solid AgCl present.
04

d. HNO3 vs. CO

HNO3 is nitric acid, a polar, soluble compound in water. When it dissolves, it ionizes to produce H+ and NO3- ions, making the resulting solution acidic. Carbon monoxide (CO) is a nonpolar, covalent compound, which has weak solubility in water due to the lack of strong interactions between carbon monoxide and water molecules. Since CO does not dissociate into ions or interact strongly with water, it does not affect the pH of the water. In summary, adding HNO3 makes the solution acidic, while CO has little effect on the water properties.

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Most popular questions from this chapter

A \(2.20-\) g sample of an unknown acid (empirical formula \(=\) $\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}_{3} )\( is dissolved in 1.0 \)\mathrm{L}$ of water. A titration required 25.0 mL of 0.500 M NaOH to react completely with all the acid present. Assuming the unknown acid has one acidic proton per molecule, what is the molecular formula of the unknown acid?

Separate samples of a solution of an unknown soluble ionic compound are treated with \(\mathrm{KCl}, \mathrm{Na}_{2} \mathrm{SO}_{4},\) and \(\mathrm{NaOH}\) . A precipitate forms only when $\mathrm{Na}_{2} \mathrm{SO}_{4}$ is added. Which cations could be present in the unknown soluble ionic compound?

Complete and balance each acid-base reaction. a. \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow\) Contains three acidic hydrogens b. $\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow$ Contains two acidic hydrogens c. $\mathrm{H}_{2} \operatorname{Se}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightarrow$ Contains two acidic hydrogens d. $\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow$ Contains two acidic hydrogens

Tris(pentafluorophenyl)borane, commonly known by its acronym BARF, is frequently used to initiate polymerization of ethylene or propylene in the presence of a catalytic transition metal compound. It is composed solely of C, F, and B; it is 42.23% C and 55.66% F by mass. a. What is the empirical formula of BARF? b. A 2.251-g sample of BARF dissolved in 347.0 mL of solution produces a 0.01267-M solution. What is the molecular formula of BARF?

A 30.0 -mL sample of an unknown strong base is neutralized after the addition of 12.0 \(\mathrm{mL}\) of a 0.150 \(\mathrm{M} \mathrm{HNO}_{3}\) solution. If the unknown base concentration is 0.0300 M, give some possible identities for the unknown base.
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