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Chapter 10: Problem 45

Use the solubility rules to predict whether the following compounds are soluble or insoluble in water: (a) \(\mathrm{AgI}(s)\) (b) \(\mathrm{Pb}\left(\mathrm{ClO}_{4}\right)_{2}(s)\) (c) \(\mathrm{NH}_{4} \mathrm{Br}(s)\) (d) \(\mathrm{K}_{2} \mathrm{SO}_{4}(s)\) (e) \(\mathrm{SrCO}_{3}(s)\)

Short Answer

Expert verified
AgI is insoluble; Pb(ClO鈧�)鈧� is soluble; NH鈧凚r is soluble; K鈧係O鈧� is soluble; SrCO鈧� is insoluble.

Step by step solution

01

Analyze the Solubility of AgI

According to solubility rules, most halides (Cl鈦�, Br鈦�, I鈦�) are soluble, except those of silver (Ag鈦�), lead (Pb虏鈦�), and mercury (Hg鈧偮测伜). Since \(\mathrm{AgI}\) contains silver, it is insoluble in water.
02

Analyze the Solubility of Pb(ClO鈧�)鈧�

Lead (Pb虏鈦�) salts are usually insoluble; however, one important exception is lead perchlorate \(\mathrm{Pb(ClO_4)_2}\). Perchlorates (\mathrm{ClO_4}鈦�) are generally soluble regardless of the metal cation they are paired with. Therefore, \(\mathrm{Pb(ClO_4)_2}\) is soluble.
03

Analyze the Solubility of NH鈧凚r

According to solubility rules, all ammonium (\mathrm{NH_4}^+) salts are soluble in water, without exception. Therefore, \(\mathrm{NH_4Br}\) is soluble in water.
04

Analyze the Solubility of K鈧係O鈧�

The solubility rules indicate that all salts containing alkali metal ions (like K鈦�) are soluble. So, \(\mathrm{K_2SO_4}\) is soluble in water.
05

Analyze the Solubility of SrCO鈧�

Carbonates (\mathrm{CO_3}虏鈦�) are generally insoluble except when combined with alkali metals and \mathrm{NH_4}^+. Since strontium (Sr虏鈦�) is not an exception, \(\mathrm{SrCO_3}\) is insoluble in water.

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Key Concepts

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

Halides
Halides include halogen anions such as chlorine (Cl鈦�), bromine (Br鈦�), and iodine (I鈦�). The solubility of halides in water largely depends on the metal cations they form salts with.
Generally, halides are soluble in water. However, they make an exception when combined with certain cations.
  • Silver (Ag鈦�)
  • Lead (Pb虏鈦�)
  • Mercury (Hg鈧偮测伜)
These exceptions form insoluble compounds with halides. For instance, silver iodide (AgI) is insoluble in water as it contains silver, one of the exceptions.
Perchlorates
Perchlorates (\( \mathrm{ClO}_{4}^{-} \)) are anions known for their good solubility in water.
Unlike many other ions, perchlorates exhibit high solubility regardless of the kind of metal cation they are paired with.
Lead perchlorate (\( \mathrm{Pb(ClO_{4})_{2}} \)) is a perfect example of a compound with perchlorate ions that is soluble, even though lead salts are generally insoluble.
This makes perchlorates standout as reliable solubilizing agents in many chemical processes.
Ammonium Salts
All ammonium salts, containing the ammonium ion (\( \mathrm{NH}_{4}^{+} \)), are soluble in water without exception.
The ammonium ion acts as a consistent solubilizer, enabling compounds such as ammonium bromide (\( \mathrm{NH}_{4} \mathrm{Br} \)) to easily dissolve in water.
This property is utilized to aid the dissolution of compounds in various scenarios, ensuring a wide range of ammonium-based salts are compatible with aqueous solutions.
Alkali Metal Ions
Alkali metal ions are derived from alkali metals found in Group 1 of the periodic table, such as lithium (Li鈦�), sodium (Na鈦�), and potassium (K鈦�).
Compounds containing these ions are almost universally soluble in water.
For instance, potassium sulfate (\( \mathrm{K}_{2} \mathrm{SO}_{4} \)) dissolves readily in water due to the presence of potassium ions (K鈦�), a hallmark of alkali metal ions.
This predictable solubility pattern makes alkali metals particularly valuable for forming various ionic solutions and reactions.
Carbonates
Carbonates (\( \mathrm{CO}_3^{2-} \)) are anions often combined with metal cations to form salts.
Generally, carbonates are insoluble in water, a rule with few exceptions.
Substances like calcium carbonate or strontium carbonate (\( \mathrm{SrCO}_{3} \)) won't dissolve readily in water. However, carbonates paired with alkali metals or ammonium (\( \mathrm{NH}_4^+ \)) ions defy this, being soluble and demonstrating the versatility and unique behavior of alkali metal and ammonium salts.
This inconsistent solubility requires attention when predicting the behavior of carbonate compounds in aqueous environments.

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Most popular questions from this chapter

Name the following ionic compounds, which are used as fertilizers: (a) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(s)\) (b) \(\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}(s)\) (c) \(\mathrm{Ca}_{5}\left(\mathrm{PO}_{4}\right)_{2}(s)\) (d) \(\mathrm{K}_{3} \mathrm{PO}_{4}(s)\)

Complete and balance the equation for each of the following acid-base reactions, name the reaction products, and write the corresponding net ionic equation: (a) \(\mathrm{HClO}_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightarrow\) (b) \(\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{KOH}(a q) \rightarrow\) (c) \(\mathrm{HI}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(s) \rightarrow\) (d) \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{RbOH}(a q) \rightarrow\)

Write the balanced chemical equation for the following reactions: (a) When table sugar, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}(s)\), is heated on a stove, it decomposes, forming a black solid and water. (b) When chlorine gas is bubbled through a clear solution of sodium bromide, the solution turns light brown. (c) When lithium oxide is added to water, it forms a basic solution.

Indicate which element is oxidized and which is reduced in the reactions described by the following chemical equations: (a) \(\mathrm{Ca}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{CaCl}_{2}(s)\) (b) \(4 \mathrm{Al}(s)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(s)\) (c) \(2 \mathrm{Rb}(s)+\mathrm{Br}_{2}(l) \rightarrow 2 \mathrm{RbBr}(s)\) (d) \(2 \mathrm{Na}(s)+\mathrm{S}(s) \rightarrow \mathrm{Na}_{2} \mathrm{~S}(s)\)

Use the solubility rules to predict the products of the following reactions. In each case complete and balance the equation and write the net ionic equation. If no precipitate forms, then write "no reaction." (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Ca}\left(\mathrm{ClO}_{4}\right)_{2}(a q) \rightarrow\) (b) \(\mathrm{AgNO}_{3}(a q)+\mathrm{NaClO}_{4}(a q) \rightarrow\) (c) \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{NaC}_{7} \mathrm{H}_{5} \mathrm{O}_{2}(a q) \rightarrow\) (d) \(\mathrm{Pb}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}(a q)+\mathrm{KBr}(a q) \rightarrow\)
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