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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
The precipitates formed for each reaction are: a. No precipitate b. \(Al(OH)_3\) c. \(CaSO_4\) d. \(NiS\)

Step by step solution

01

Identify ions present in each solution

Write the ionic forms of each compound: a. \(FeSO_4 (aq) \) = \(Fe^{2+}\) + \(SO_4^{2-}\) \\ \(KCl (aq) \) = \(K^+\) + \(Cl^-\) b. \(Al(NO_3)_3 (aq) \) = \(Al^{3+}\) + \(3NO_3^-\) \\ \(Ba (OH)_2 (aq) \) = \(Ba^{2+}\) + \(2OH^-\) c. \(CaCl_2 (aq) \) = \(Ca^{2+}\) + \(2Cl^-\) \\ \(Na_2 SO_4 (aq)\) = \(2Na^+\) + \(SO_4^{2-}\) d. \(K_2 S (aq) \) = \(2K^+\) + \(S^{2-}\) \\ \(Ni (NO_3)_2 (aq) \) = \(Ni^{2+}\) + \(2NO_3^-\)
02

Apply solubility rules

Determine which of the possible products of the combinations of solutions are insoluble. a. Possible products: \(FeCl_2\) and \(K_2SO_4\) \\ b. Possible products: \(Al(OH)_3\) and \(Ba(NO_3)_2\) \\ c. Possible products: \(CaSO_4\) and \(2NaCl\) \\ d. Possible products: \(K_2(NO_3)_2\) and \(NiS\) For each combination, check the solubility rules: a. \(FeCl_2\) is soluble and \(K_2SO_4\) is soluble. \\ b. \(Al(OH)_3\) is insoluble, and \(Ba(NO_3)_2\) is soluble. \\ c. \(CaSO_4\) is slightly insoluble, and \(2NaCl\) is soluble. \\ d. \(K_2(NO_3)_2\) is soluble, and \(NiS\) is insoluble.
03

Identify precipitates

Based on the solubility rules, identify which reactions form precipitates: a. No precipitate is formed. b. A precipitate of \(Al(OH)_3\) is formed. c. A slightly insoluble precipitate of \(CaSO_4\) is formed. d. A precipitate of \(NiS\) is formed. The precipitates formed for each reaction are: a. No precipitate \\ b. \(Al(OH)_3\) \\ c. \(CaSO_4\) \\ d. \(NiS\)

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Most popular questions from this chapter

Write the balanced formula, complete ionic, and net ionic equations for each of the following acid-base reactions. a. \(\mathrm{HClO}_{4}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(s) \rightarrow\) b. \(\mathrm{HCN}(a q)+\mathrm{NaOH}(a q) \rightarrow\) c. \(\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \rightarrow\)

Write the balanced formula equation for the acid-base reactions that occur when the following are mixed. a. potassium hydroxide (aqueous) and nitric acid b. barium hydroxide (aqueous) and hydrochloric acid c. perchloric acid \(\left[\mathrm{HClO}_{4}(a q)\right]\) and solid iron(III) hydroxide d. solid silver hydroxide and hydrobromic acid e. aqueous strontium hydroxide and hydroiodic acid

Calcium chloride is a strong electrolyte and is used to "salt" streets in the winter to melt ice and snow. Write a reaction to show how this substance breaks apart when it dissolves in water.

Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations. copper(II) sulfate \((a q)+\operatorname{iron}(s)\) $$ \operatorname{copper}(s)+\text { iron(II) sulfate }(a q) $$ \(\operatorname{copper}(\) II \()\) sulfate \((a q)+\operatorname{iron}(s)\) $$ \operatorname{copper}(s)+\text { iron(III) sulfate }(a q) $$ 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.

Many oxidation-reduction reactions can be balanced by inspection. Try to balance the following reactions by inspection. In each reaction, identify the substance reduced and the substance oxidized. a. \(\mathrm{Al}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{H}_{2}(g)\) b. \(\mathrm{CH}_{4}(g)+\mathrm{S}(s) \rightarrow \mathrm{CS}_{2}(l)+\mathrm{H}_{2} \mathrm{~S}(\mathrm{~g})\) c. \(\mathrm{C}_{3} \mathrm{H}_{8}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) d. \(\mathrm{Cu}(s)+\mathrm{Ag}^{+}(a q) \rightarrow \mathrm{Ag}(s)+\mathrm{Cu}^{2+}(a q)\)
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