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Chapter 4: Problem 43

On the basis of the general solubility rules given in Table 4.1, predict which of the following substances are likely to be soluble in water. a. aluminum nitrate b. magnesium chloride c, rubidium sulfate d. nickel(II) hydroxide e. lead(II) sulfide f. magnesium hydroxide g. iron(III) phosphate

Short Answer

Expert verified
Soluble substances: aluminum nitrate (Al(NO3)3), magnesium chloride (MgCl2), and rubidium sulfate (Rb2SO4). Insoluble substances: nickel(II) hydroxide (Ni(OH)2), lead(II) sulfide (PbS), magnesium hydroxide (Mg(OH)2), and iron(III) phosphate (FePO4).

Step by step solution

01

Rule Used:

Rule 1. All nitrates (NO3-) are soluble.
02

Solubility:

Soluble b. Magnesium chloride (MgCl2):
03

Rule Used:

Rule 3. All chlorides (Cl-) are soluble, except when combined with Ag+, Pb^2+, and Hg^2+.
04

Solubility:

Soluble c. Rubidium sulfate (Rb2SO4):
05

Rule Used:

Rule 4. All sulfates (SO4^2-) are soluble, except when combined with Ca^2+, Sr^2+, Ba^2+, and Pb^2+.
06

Solubility:

Soluble d. Nickel(II) hydroxide (Ni(OH)2):
07

Rule Used:

Rule 5. All hydroxides (OH-) and oxides (O^2-) are generally insoluble, except when combined with alkali metals and ammonium.
08

Solubility:

Insoluble e. Lead(II) sulfide (PbS):
09

Rule Used:

Rule 6. All sulfides (S^2-), carbonates (CO3^2-), and phosphates (PO4^3-) are generally insoluble, except when combined with alkali metals and ammonium.
10

Solubility:

Insoluble f. Magnesium hydroxide (Mg(OH)2):
11

Rule Used:

Rule 5. All hydroxides (OH-) and oxides (O^2-) are generally insoluble, except when combined with alkali metals and ammonium.
12

Solubility:

Insoluble g. Iron(III) phosphate (FePO4):
13

Rule Used:

Rule 6. All sulfides (S^2-), carbonates (CO3^2-), and phosphates (PO4^3-) are generally insoluble, except when combined with alkali metals and ammonium.
14

Solubility:

Insoluble Thus, we can conclude that aluminum nitrate, magnesium chloride, and rubidium sulfate are soluble in water, while nickel(II) hydroxide, lead(II) sulfide, magnesium hydroxide, and iron(III) phosphate are insoluble in water.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Solubility in Water
Solubility in water is an important concept in chemistry. It determines whether a substance can dissolve in water to form a solution. When substances dissolve, their particles are evenly distributed within the water, creating a homogeneous mixture.
Understanding solubility helps predict how substances will behave in natural environments or industrial processes.
Water, being a polar solvent, often dissolves ionic compounds and polar molecules, thanks to interactions between water molecules and solute ions or molecules.
Chemical Compounds
Chemical compounds are substances formed from two or more elements that are chemically bonded together. These compounds have distinct properties and consistent compositions.
Common types include ionic compounds, like magnesium chloride, where metals and non-metals create ionic bonds, and covalent compounds, where elements share electrons.
Understanding the properties of chemical compounds, including solubility, is crucial for exploring their practical applications in labs, industries, and daily life.
Aqueous Solutions
Aqueous solutions are mixtures where water acts as the solvent. In these solutions, water dissolves the solute, which can be any substance that is capable of being broken down or separated into smaller particles in water.
For example, when magnesium chloride dissolves in water, it forms an aqueous solution with magnesium ( Mg^{2+} ) and chloride ions ( Cl^- ).
This process is vital in numerous chemical reactions, where substances must be dissolved in water to interact effectively.
General Solubility Rules
General solubility rules offer guidelines for predicting the solubility of certain chemical compounds in water. These rules are based on the interactions between ions and are helpful for anticipating how substances will dissolve.
For instance, nitrates ( NO_3^- ) are always soluble; thus, aluminum nitrate easily dissolves in water. Similarly, most chlorides are soluble, while exceptions exist for compounds with certain metals.
Learners use these rules to understand reaction mechanisms and to predict the formation of precipitates in chemical reactions.

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Most popular questions from this chapter

A mixture contains only \(\mathrm{NaCl}\) and \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} .\) A \(1.45-\mathrm{g}\) sample of the mixture is dissolved in water and an excess of \(\mathrm{NaOH}\) is added, producing a precipitate of \(\mathrm{Al}(\mathrm{OH})_{3}\). The precipitate is filtered, dried, and weighed. The mass of the precipitate is \(0.107 \mathrm{~g}\). What is the mass percent of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) in the sample?

Zinc and magnesium metal each react with hydrochloric acid according to the following equations: $$ \begin{aligned} \mathrm{Zn}(s)+2 \mathrm{HCl}(a q) & \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g) \\ \mathrm{Mg}(s)+2 \mathrm{HCl}(a q) & \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g) \end{aligned} $$ A \(10.00-\mathrm{g}\) mixture of zinc and magnesium is reacted with the stoichiometric amount of hydrochloric acid. The reaction mixture is then reacted with \(156 \mathrm{~mL}\) of \(3.00 \mathrm{M}\) silver nitrate to produce the maximum possible amount of silver chloride. a. Determine the percent magnesium by mass in the original mixture. b. If \(78.0 \mathrm{~mL}\) of \(\mathrm{HCl}\) was added, what was the concentration of the \(\mathrm{HCl} ?\)

What mass of silver chloride can be prepared by the reaction of \(100.0 \mathrm{~mL}\) of \(0.20 \mathrm{M}\) silver nitrate with \(100.0 \mathrm{~mL}\) of \(0.15 \mathrm{M}\) calcium chloride? Calculate the concentrations of each ion remaining in solution after precipitation is complete.

When the following solutions are mixed together, what precipitate (if any) will form? a. \(\mathrm{FeSO}_{4}(a q)+\mathrm{KCl}(a q)\) b. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q)\) c. \(\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)\) d. \(\mathrm{K}_{2} \mathrm{~S}(a q)+\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)\)

A solution was prepared by mixing \(50.00 \mathrm{~mL}\) of \(0.100 \mathrm{M}\) \(\mathrm{HNO}_{3}\) and \(100.00 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{HNO}_{3} .\) Calculate the molarity of the final solution of nitric acid.
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