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Chapter 6: Problem 48

When the following solutions are mixed together, what precipitate (if any) will form? a. \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{CuSO}_{4}(a q)\) b. \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{CaCl}_{2}(a q)\) c. \(\mathrm{K}_{2} \mathrm{CO}_{3}(a q)+\mathrm{MgI}_{2}(a q)\) d. \(\mathrm{Na}_{2} \mathrm{CrO}_{4}(a q)+\mathrm{AlBr}_{3}(a q)\)

Short Answer

Expert verified
Precipitates will form in the following cases: a. \(\mathrm{Hg}_{2}\mathrm{S}\mathrm{O}_{4}\) c. \(\mathrm{MgCO}_3\) d. \(\mathrm{Al}_{2}\left(\mathrm{CrO}_{4}\right)_{3}\)

Step by step solution

01

Case A: Mixing Hg2(NO3)2 and CuSO4

In this case, we need to consider the possible products of the mixing: \(\mathrm{Hg}_{2}\mathrm{S}\mathrm{O}_{4}\) and \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\). Checking the solubility rules, we find out that \(\mathrm{Hg}_{2}\mathrm{S}\mathrm{O}_{4}\) is insoluble and will form a precipitate. Meanwhile, \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\) is soluble and will not form a precipitate.
02

Case B: Mixing Ni(NO3)2 and CaCl2

In this case, the possible products of the mixing are \(\mathrm{NiCl}_{2}\) and \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\). According to the solubility rules, both \(\mathrm{NiCl}_{2}\) and \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) are soluble in water. Therefore, no precipitate will form in this case.
03

Case C: Mixing K2CO3 and MgI2

In this case, the possible products of the mixing are \(\mathrm{K}\mathrm{I}\) and \(\mathrm{MgCO}_3\). According to the solubility rules, \(\mathrm{K}\mathrm{I}\) is soluble, but \(\mathrm{MgCO}_3\) is insoluble and will form a precipitate.
04

Case D: Mixing Na2CrO4 and AlBr3

In this case, the possible products of the mixing are \(\mathrm{NaBr}\) and \(\mathrm{Al}_{2}\left(\mathrm{CrO}_{4}\right)_{3}\). Based on the solubility rules, \(\mathrm{NaBr}\) is soluble, but \(\mathrm{Al}_{2}\left(\mathrm{CrO}_{4}\right)_{3}\) is insoluble and will form a precipitate. In summary, precipitates will form in the following cases: a. \(\mathrm{Hg}_{2}\mathrm{S}\mathrm{O}_{4}\) c. \(\mathrm{MgCO}_3\) d. \(\mathrm{Al}_{2}\left(\mathrm{CrO}_{4}\right)_{3}\)

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Most popular questions from this chapter

Zinc and magnesium metal each react with hydrochloric acid according to the following equations: $$ \begin{array}{c} \mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g) \\ \mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g) \end{array} $$ 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 HCl was added, what was the concentration of the HCl?

Complete and balance each acid-base reaction. a. \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow\) Contains three acidic hydrogens b. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow\) Contains two acidic hydrogens c. \(\mathrm{H}_{2} \mathrm{Se}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightarrow\) Contains two acidic hydrogens d. \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow\)

Consider a \(1.50-\mathrm{g}\) mixture of magnesium nitrate and magnesium chloride. After dissolving this mixture in water, 0.500 \(M\) silver nitrate is added dropwise until precipitate formation is complete. The mass of the white precipitate formed is 0.641 g. a. Calculate the mass percent of magnesium chloride in the mixture. b. Determine the minimum volume of silver nitrate that must have been added to ensure complete formation of the precipitate.

Balance each of the following oxidation-reduction reactions by using the oxidation states method. a. \(\mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) b. \(\mathrm{Mg}(s)+\mathrm{HCl}(a q) \rightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Cl}^{-}(a q)+\mathrm{H}_{2}(g)\) c. \(\mathrm{Co}^{3+}(a q)+\mathrm{Ni}(s) \rightarrow \mathrm{Co}^{2+}(a q)+\mathrm{Ni}^{2+}(a q)\) d. \(\mathrm{Zn}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{ZnSO}_{4}(a q)+\mathrm{H}_{2}(g)\)

Assign oxidation states for all atoms in each of the following compounds. a. \(U O_{2}^{2+}\) f. \(\mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7}\) b. \(\mathrm{As}_{2} \mathrm{O}_{3}\) g. \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\) c. \(\mathrm{NaBiO}_{3}\) h. \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\) d. \(\mathrm{As}_{4}\) i. \(\quad \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) e. \(\mathrm{HAsO}_{2}\)
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