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Chapter 4: Problem 45

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. \(\mathrm{K}_{2} \mathrm{~S}(a q)+\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)\)

Short Answer

Expert verified
Precipitates formed in each case are: - a. No precipitate - b. Al(OH)₃ - c. CaSO₄ - d. NiS

Step by step solution

01

a. FeSO4(aq) + KCl(aq)

1. Analyze the chemical equation: The given solutions are: FeSO4(aq) - containing Fe²⁺ and SO₄²⁻ ions, and KCl(aq) - containing K⁺ and Cl⁻ ions. 2. Determine the possible combinations: The possible combinations of these ions are: FeCl₂ and K₂SO₄. 3. Check solubility: According to the solubility rules, both FeCl₂ and K₂SO₄ are soluble, so no precipitate will form in this case.
02

b. Al(NO₃)₃(aq) + Ba(OH)₂(aq)

1. Analyze the chemical equation: The given solutions are: Al(NO₃)₃(aq) - containing Al³⁺ and NO₃⁻ ions, and Ba(OH)₂(aq) - containing Ba²⁺ and OH⁻ ions. 2. Determine the possible combinations: The possible combinations of these ions are: Al(OH)₃ and Ba(NO₃)₂. 3. Check solubility: According to the solubility rules, Al(OH)₃ is insoluble, and Ba(NO₃)₂ is soluble. 4. Write down the balanced chemical equation: When these two solutions are combined, a precipitate will form as Al(OH)₃. \[ Al^{3+}(aq) + 3OH^{-}(aq) \rightarrow Al(OH)_3(s) \]
03

c. CaCl₂(aq) + Na₂SO₄(aq)

1. Analyze the chemical equation: The given solutions are: CaCl₂(aq) - containing Ca²⁺ and Cl⁻ ions, and Na₂SO₄(aq) - containing Na⁺ and SO₄²⁻ ions. 2. Determine the possible combinations: The possible combinations of these ions are: CaSO₄ and NaCl. 3. Check solubility: According to the solubility rules, CaSO₄ is slightly soluble (which can still form a precipitate), and NaCl is soluble. 4. Write down the balanced chemical equation: When these two solutions are combined, a precipitate will form as CaSO₄. \[ Ca^{2+}(aq) + SO_{4}^{2-}(aq) \rightarrow CaSO_4(s) \]
04

d. K₂S(aq) + Ni(NO₃)₂(aq)

1. Analyze the chemical equation: The given solutions are: K₂S(aq) - containing K⁺ and S²⁻ ions, and Ni(NO₃)₂(aq) - containing Ni²⁺ and NO₃⁻ ions. 2. Determine the possible combinations: The possible combinations of these ions are: KNO₃ and NiS. 3. Check solubility: According to the solubility rules, KNO₃ is soluble, and NiS is insoluble. 4. Write down the balanced chemical equation: When these two solutions are combined, a precipitate will form as NiS. \[ Ni^{2+}(aq) + S^{2-}(aq) \rightarrow NiS(s) \] In summary, precipitates will form in the following cases: - b. Al(NO₃)₃(aq) + Ba(OH)₂(aq) will form Al(OH)₃ - c. CaCl₂(aq) + Na₂SO₄(aq) will form CaSO₄ - d. K₂S(aq) + Ni(NO₃)₂(aq) will form NiS

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Most popular questions from this chapter

The blood alcohol \(\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{OH}\right)\) level can be determined by titrating a sample of blood plasma with an acidic potassium dichromate solution, resulting in the production of \(\mathrm{Cr}^{3+}(a q)\) and carbon dioxide. The reaction can be monitored because the dichromate ion \(\left(\mathrm{Cr}_{2} \mathrm{O}_{7}{ }^{2-}\right)\) is orange in solution, and the \(\mathrm{Cr}^{3+}\) ion is green. The balanced equation is \(16 \mathrm{H}^{+}(a q)+2 \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{OH}(a q) \longrightarrow\) \(4 \mathrm{Cr}^{3+}(a q)+2 \mathrm{CO}_{2}(g)+11 \mathrm{H}_{2} \mathrm{O}(t)\) This reaction is an oxidation-reduction reaction. What species is reduced, and what species is oxidized? How many electrons are transferred in the balanced equation above?

The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of \(204.22 \mathrm{~g} / \mathrm{mol}\). In the titration, \(34.67 \mathrm{~mL}\) of the sodium hydroxide solution was required to react with \(0.1082 \mathrm{~g}\) KHP. Calculate the molarity of the sodium hydroxide.

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Polychlorinated biphenyls (PCBs) have been used extensively as dielectric materials in electrical transformers. Because PCBs have been shown to be potentially harmful, analysis for their presence in the environment has become very important. PCBs are manufactured according to the following generic reaction: $$ \mathrm{C}_{12} \mathrm{H}_{10}+{ }_{n \mathrm{Cl}_{2}} \rightarrow \mathrm{C}_{12} \mathrm{H}_{10-n} \mathrm{Cl}_{n}+n \mathrm{HCl} $$ This reaction results in a mixture of \(\mathrm{PCB}\) products. The mixture is analyzed by decomposing the \(\mathrm{PCBs}\) and then precipitating the resulting \(\mathrm{Cl}^{-}\) as \(\mathrm{AgCl}\). a. Develop a general equation that relates the average value of \(n\) to the mass of a given mixture of \(\mathrm{PCBs}\) and the mass of \(\mathrm{AgCl}\) produced. b. A \(0.1947-g\) sample of a commercial PCB yielded \(0.4791 \mathrm{~g}\) of \(\mathrm{AgCl}\). What is the average value of \(n\) for this sample?

Describe how you would prepare \(2.00 \mathrm{~L}\) of each of the following solutions. a. \(0.250 \mathrm{M} \mathrm{NaOH}\) from solid \(\mathrm{NaOH}\) b. \(0.250 M \mathrm{NaOH}\) from \(1.00 M \mathrm{NaOH}\) stock solution c. \(0.100 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}\) from solid \(\mathrm{K}_{2} \mathrm{CrO}_{4}\) d. \(0.100 M \mathrm{~K}_{2} \mathrm{CrO}_{4}\) from \(1.75 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}\) stock solution
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