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Chapter 4: Problem 21

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

Expert verified
Three soluble bromide salts are \(NaBr\), \(KBr\), and \(CaBr_2\); three insoluble bromide salts are \(AgBr\), \(PbBr_2\), and \(HgBr_2\). Three soluble sulfate salts are \(Na_2SO_4\), \(K_2SO_4\), and \((NH_4)_2SO_4\); three insoluble sulfate salts are \(BaSO_4\), \(CaSO_4\), and \(PbSO_4\). Three soluble hydroxide salts are \(NaOH\), \(KOH\), and \(Ba(OH)_2\); three insoluble hydroxide salts are \(Al(OH)_3\), \(Fe(OH)_3\), and \(Ni(OH)_2\). Three soluble phosphate salts are \(Na_3PO_4\), \(K_3PO_4\), and \((NH_4)_3PO_4\); three insoluble phosphate salts are \(Ca_3(PO_4)_2\), \(AlPO_4\), and \(FePO_4\). Six insoluble \(\mathrm{Pb}^{2+}\) salts are \(PbSO_4\), \(Pb_3(PO_4)_2\), \(Pb(OH)_2\), \(PbBr_2\), \(PbI_2\), and \(PbCO_3\); one soluble \(\mathrm{Pb}^{2+}\) salt is \(Pb(NO_3)_2\).

Step by step solution

01

Solubility Rules for Bromide (Br-) Salts

Bromide salts are generally soluble, with a few exceptions. Bromide salts of silver (Ag), lead (Pb), and mercury (Hg) are insoluble.
02

Soluble Bromide Salts

Here are three examples of soluble bromide salts: 1. Sodium bromide (\(NaBr\)) 2. Potassium bromide (\(KBr\)) 3. Calcium bromide (\(CaBr_2\))
03

Insoluble Bromide Salts

Here are three examples of insoluble bromide salts: 1. Silver bromide (\(AgBr\)) 2. Lead(II) bromide (\(PbBr_2\)) 3. Mercury(II) bromide (\(HgBr_2\))
04

Solubility Rules for Sulfate (SO4^2-) Salts

Sulfate salts are generally soluble, with few exceptions, like sulfates of barium (Ba), calcium (Ca), strontium (Sr), lead (Pb), and mercury (Hg).
05

Soluble Sulfate Salts

Here are three examples of soluble sulfate salts: 1. Sodium sulfate (\(Na_2SO_4\)) 2. Potassium sulfate (\(K_2SO_4\)) 3. Ammonium sulfate (\((NH_4)_2SO_4\))
06

Insoluble Sulfate Salts

Here are three examples of insoluble sulfate salts: 1. Barium sulfate (\(BaSO_4\)) 2. Calcium sulfate (\(CaSO_4\)) 3. Lead(II) sulfate (\(PbSO_4\))
07

Solubility Rules for Hydroxide (OH-) Salts

Hydroxide salts are generally insoluble, except for alkali metal hydroxides (Group 1 metals) and some heavy Group 2 metal hydroxides (like Ba and Sr).
08

Soluble Hydroxide Salts

Here are three examples of soluble hydroxide salts: 1. Sodium hydroxide (\(NaOH\)) 2. Potassium hydroxide (\(KOH\)) 3. Barium hydroxide (\(Ba(OH)_2\))
09

Insoluble Hydroxide Salts

Here are three examples of insoluble hydroxide salts: 1. Aluminum hydroxide (\(Al(OH)_3\)) 2. Iron(III) hydroxide (\(Fe(OH)_3\)) 3. Nickel(II) hydroxide (\(Ni(OH)_2\))
10

Solubility Rules for Phosphate (PO4^3-) Salts

Phosphate salts are generally insoluble, except for salts of Group 1 metals (alkali metals) and ammonium.
11

Soluble Phosphate Salts

Here are three examples of soluble phosphate salts: 1. Sodium phosphate (\(Na_3PO_4\)) 2. Potassium phosphate (\(K_3PO_4\)) 3. Ammonium phosphate (\((NH_4)_3PO_4\))
12

Insoluble Phosphate Salts

Here are three examples of insoluble phosphate salts: 1. Calcium phosphate (\(Ca_3(PO_4)_2\)) 2. Aluminum phosphate (\(AlPO_4\)) 3. Iron(III) phosphate (\(FePO_4\))
13

Insoluble Lead(II) (Pb^2+) Salts

Here are six examples of insoluble lead(II) salts: 1. Lead(II) sulfate (\(PbSO_4\)) 2. Lead(II) phosphate (\(Pb_3(PO_4)_2\)) 3. Lead(II) hydroxide (\(Pb(OH)_2\)) 4. Lead(II) bromide (\(PbBr_2\)) 5. Lead(II) iodide (\(PbI_2\)) 6. Lead(II) carbonate (\(PbCO_3\))
14

Soluble Lead(II) Salt

Here's an example of a soluble lead(II) salt: 1. Lead(II) nitrate (\(Pb(NO_3)_2\))

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Most popular questions from this chapter

A 50.00 -mL sample of solution containing \(\mathrm{Fe}^{2+}\) ions is titrated with a 0.0216 \(\mathrm{M} \mathrm{KMnO}_{4}\) solution. It required 20.62 \(\mathrm{mL}\) of \(\mathrm{KMnO}_{4}\) solution to oxidize all the \(\mathrm{Fe}^{2+}\) ions to \(\mathrm{Fe}^{3+}\) ions by the reaction $$\mathrm{MnO}_{4}^{-}(a q)+\mathrm{Fe}^{2+}(a q) \stackrel{\text { Acidic }}{\longrightarrow} \mathrm{Mn}^{2+}(a q)+\mathrm{Fe}^{3+}(a q) \text{(Unbalanced)} $$ a. What was the concentration of \(\mathrm{Fe}^{2+}\) ions in the sample solution? b. What volume of 0.0150\(M \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) solution would it take to do the same titration? The reaction is $$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{Fe}^{2+}(a q) \stackrel{\mathrm{Acidic}}{\longrightarrow} \mathrm{Cr}^{3+}(a q) +\mathrm{Fe}^{3+}(a q) \text {(Unbalanced)} $$

An average human being has about 5.0 \(\mathrm{L}\) of blood in his or her body. If an average person were to eat 32.0 \(\mathrm{g}\) of sugar (sucrose, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}, 342.30 \mathrm{g} / \mathrm{mol}\) ), and all that sugar were dissolved into the bloodstream, how would the molarity of the blood sugar change?

A \(10.00-\mathrm{mL}\) . sample of vinegar, an aqueous solution of acetic acid \(\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right),\) is titrated with \(0.5062 \mathrm{M} \mathrm{NaOH},\) and 16.58 mL is required to reach the equivalence point. a. What is the molarity of the acetic acid? b. If the density of the vinegar is \(1.006 \mathrm{g} / \mathrm{cm}^{3},\) what is the mass percent of acetic acid in the vinegar?

A solution is prepared by dissolving 0.6706 g oxalic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\) in enough water to make 100.0 \(\mathrm{mL}\) of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the oxalic acid solution?

You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final concentration be within 1% of 0.02 M and that the concentration must be known accurately to the fourth decimal place. How would you prepare this solution? Specify the glassware you would use, the accuracy needed for the balance, and the ranges of acceptable masses of \(\mathrm{KIO}_{3}\) that can be used
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