Chapter 7: Problem 33
The same net ionic process takes place when any strong acid reacts with any strong base. Write the equation for that process.
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Balance each of the following equations that describe synthesis reactions. a. \(\mathrm{Ni}(s)+\mathrm{CO}(g) \rightarrow \mathrm{Ni}(\mathrm{CO})_{4}(g)\). b. \(\mathrm{Al}(s)+\mathrm{S}(s) \rightarrow \mathrm{Al}_{2} \mathrm{S}_{3}(s)\) c. \(\mathrm{Na}_{2} \mathrm{SO}_{3}(a q)+\mathrm{S}(s) \rightarrow \mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}(a q)\) d. \(\operatorname{Fe}(s)+\operatorname{Br}_{2}(l) \rightarrow \operatorname{Fe} \mathrm{Br}_{3}(s)\) e. \(\mathrm{Na}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{Na}_{2} \mathrm{O}_{2}(s)\)
For each of the following metals, how many electrons will the metal atoms lose when the metal reacts with a nonmetal? a. sodium b. potassium c. magnesium d. barium e. aluminum
When two solutions of ionic substances are mixed and a precipitate forms, what is the net charge of the precipitate? Why?
For each of the following unbalanced molecular equations, write the corresponding balanced net ionic equation for the reaction. a. \(\mathrm{HCl}(a q)+\mathrm{AgNO}_{3}(a q) \rightarrow \mathrm{AgCl}(s)+\mathrm{HNO}_{3}(a q)\) b. \(\mathrm{CaCl}_{2}(a q)+\mathrm{Na}_{3} \mathrm{PO}_{4}(a q) \rightarrow \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+\) \(\mathrm{NaCl}(a q)\) c. \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{BaCl}_{2}(a q) \rightarrow\) \(\mathrm{PbCl}_{2}(s)+\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) d. \(\operatorname{FeCl}_{3}(a q)+\operatorname{NaOH}(a q) \rightarrow \operatorname{Fe}(\mathrm{OH})_{3}(s)+\mathrm{NaCl}(a q)\)
Balance each of the following equations that describe synthesis reactions. a. \(\operatorname{FeO}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}(s)\) b. \(\operatorname{CO}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)\) c. \(\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{HCl}(g)\) d. \(\mathrm{K}(s)+\mathrm{S}_{8}(s) \rightarrow \mathrm{K}_{2} \mathrm{S}(s)\) e. \(\mathrm{Na}(s)+\mathrm{N}_{2}(g) \rightarrow \mathrm{Na}_{3} \mathrm{N}(s)\)
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