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Chapter 4: Problem 17

List the formulas of three soluble bromide salts and three insoluble bromide salts. Do the same exercise for sulfate salts, hydroxide salts, and phosphate salts (list three soluble salts and three insoluble salts). List the formulas for six insoluble \(\mathrm{Pb}^{2+}\) salts and one soluble \(\mathrm{Pb}^{2+}\) salt.

Short Answer

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Soluble salts: \(NaBr\), \(KBr\), \(CaBr_2\), \(Na_2SO_4\), \((NH_4)_2SO_4\), \(MgSO_4\), \(NaOH\), \(KOH\), \(NH_4OH\), \(Na_3PO_4\), \(K_3PO_4\), \((NH_4)_3PO_4\). Insoluble salts: \(AgBr\), \(PbBr_2\), \(Hg_2Br_2\), \(CaSO_4\), \(PbSO_4\), \(BaSO_4\), \(Ca(OH)_2\), \(Fe(OH)_3\), \(Cu(OH)_2\), \(Ca_3(PO_4)_2\), \(FePO_4\), \(AlPO_4\). Six insoluble \(\mathrm{Pb}^{2+}\) salts: \(PbCl_2\), \(PbI_2\), \(PbBr_2\), \(PbS\), \(PbCO_3\), \(PbCrO_4\). One soluble \(\mathrm{Pb}^{2+}\) salt: \(Pb(NO_3)_2\).

Step by step solution

01

Soluble Bromide Salts

Using the solubility rules, we know that most bromide salts are soluble, except for those combined with silver, lead, or mercury(I). Some examples of soluble bromide salts are: 1. Sodium bromide: \(NaBr\) 2. Potassium bromide: \(KBr\) 3. Calcium bromide: \(CaBr_2\)
02

Insoluble Bromide Salts

As mentioned above, insoluble bromide salts are typically those combined with silver, lead, or mercury(I). Examples of insoluble bromide salts include: 1. Silver bromide: \(AgBr\) 2. Lead(II) bromide: \(PbBr_2\) 3. Mercury(I) bromide: \(Hg_2Br_2\)
03

Soluble Sulfate Salts

Most sulfate salts are soluble, except for those combined with calcium, strontium, barium, lead, or mercury(I). Some examples of soluble sulfate salts are: 1. Sodium sulfate: \(Na_2SO_4\) 2. Ammonium sulfate: \((NH_4)_2SO_4\) 3. Magnesium sulfate: \(MgSO_4\)
04

Insoluble Sulfate Salts

As mentioned previously, insoluble sulfate salts are typically those combined with calcium, strontium, barium, lead, or mercury(I). Examples of insoluble sulfate salts include: 1. Calcium sulfate: \(CaSO_4\) 2. Lead(II) sulfate: \(PbSO_4\) 3. Barium sulfate: \(BaSO_4\)
05

Soluble Hydroxide Salts

Soluble hydroxide salts are typically those combined with alkali metals (Group 1 elements) or ammonium. Some examples of soluble hydroxide salts are: 1. Sodium hydroxide: \(NaOH\) 2. Potassium hydroxide: \(KOH\) 3. Ammonium hydroxide: \(NH_4OH\)
06

Insoluble Hydroxide Salts

Insoluble hydroxide salts are mostly those combined with alkaline earth metals (Group 2 elements), along with most transition metals. Examples of insoluble hydroxide salts include: 1. Calcium hydroxide: \(Ca(OH)_2\) 2. Iron(III) hydroxide: \(Fe(OH)_3\) 3. Copper(II) hydroxide: \(Cu(OH)_2\)
07

Soluble Phosphate Salts

Soluble phosphate salts are typically those combined with alkali metals or ammonium. Some examples of soluble phosphate salts are: 1. Sodium phosphate: \(Na_3PO_4\) 2. Potassium phosphate: \(K_3PO_4\) 3. Ammonium phosphate: \((NH_4)_3PO_4\)
08

Insoluble Phosphate Salts

Insoluble phosphate salts are mostly those combined with alkaline earth metals or most transition metals. Examples of insoluble phosphate salts include: 1. Calcium phosphate: \(Ca_3(PO_4)_2\) 2. Iron(III) phosphate: \(FePO_4\) 3. Aluminum phosphate: \(AlPO_4\)
09

Insoluble \(\mathrm{Pb}^{2+}\) Salts

Examples of insoluble \(\mathrm{Pb}^{2+}\) salts include: 1. Lead(II) chloride: \(PbCl_2\) 2. Lead(II) iodide: \(PbI_2\) 3. Lead(II) bromide: \(PbBr_2\) 4. Lead(II) sulfide: \(PbS\) 5. Lead(II) carbonate: \(PbCO_3\) 6. Lead(II) chromate: \(PbCrO_4\)
10

Soluble \(\mathrm{Pb}^{2+}\) Salt

An example of a soluble \(\mathrm{Pb}^{2+}\) salt is: 1. Lead(II) nitrate: \(Pb(NO_3)_2\)

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Most popular questions from this chapter

A \(450.0-\mathrm{mL}\) sample of a \(0.257-M\) solution of silver nitrate is mixed with \(400.0 \mathrm{~mL}\) of \(0.200 M\) calcium chloride. What is the concentration of \(\mathrm{Cl}^{-}\) in solution after the reaction is complete?

You are given a solid that is a mixture of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\). A \(0.205-g\) sample of the mixture is dissolved in water. An excess of an aqueous solution of \(\mathrm{BaCl}_{2}\) is added. The \(\mathrm{BaSO}_{4}\) that is formed is filtered, dried, and weighed. Its mass is \(0.298 \mathrm{~g}\). What mass of \(\mathrm{SO}_{4}^{2-}\) ion is in the sample? What is the mass percent of \(\mathrm{SO}_{4}{ }^{2-}\) ion in the sample? What are the percent compositions by mass of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) in the sample?

What acid and what base would react in aqueous solution so that the following salts appear as products in the formula equation? Write the balanced formula equation for each reaction. a. potassium perchlorate b. cesium nitrate c. calcium iodide

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 \(\mathrm{HCl} ?\)

Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations. \(\operatorname{copper}(\) II \()\) sulfate \((a q)+\) iron \((s) \longrightarrow\) \(\operatorname{copper}(s)+\) iron(II) sulfate \((a q)\) copper(II) sulfate \((a q)+\operatorname{iron}(s) \longrightarrow\) \(\operatorname{copper}(s)+\) iron(III) sulfate \((a q)\) You place \(87.7 \mathrm{~mL}\) of a \(0.500-M\) solution of copper(II) sulfate in a beaker. You then add \(2.00 \mathrm{~g}\) of iron filings to the copper(II) sulfate solution. After one of the above reactions occurs, you isolate \(2.27 \mathrm{~g}\) of copper. Which equation above describes the reaction that occurred? Support your answer.
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