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Chapter 4: Problem 22

Write ionic and net ionic equations for the following reactions: (a) \(\mathrm{Na}_{2} \mathrm{~S}(a q)+\mathrm{ZnCl}_{2}(a q) \longrightarrow\) (b) \(\mathrm{K}_{3} \mathrm{PO}_{4}(a q)+3 \mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow\) (c) \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow\)

Short Answer

Expert verified
a) Net Ionic Equation : \(\mathrm{S^{2-}(aq) + Zn^{2+}(aq)} \longrightarrow\)b) Net Ionic Equation : \(\mathrm{PO_{4}^{3-}(aq) + 3Sr^{2+}(aq)} \longrightarrow\)c) Net Ionic Equation : \(\mathrm{Mg^{2+}(aq) + 2OH^{-}(aq)} \longrightarrow\)

Step by step solution

01

Ionic and Net Ionic Equations

Ionic Equations are equations that show all the compounds in ionic form. Net Ionic Equations are equations that only show the key substances involved in the reaction. A rule to remember, all soluble ionic compounds and strong acids dissociate into their ions in solution.
02

Problem a: \(\mathrm{Na}_{2} \mathrm{~S}(a q)+\mathrm{ZnCl}_{2}(a q) \longrightarrow\)

First, break down the reactants in ionic form and this is the full ionic equation:\(\mathrm{2Na^{+}(aq) + S^{2-}(aq) + Zn^{2+}(aq) + 2Cl^{-}(aq)} \longrightarrow\)Next, the net ionic equation is generated by removing spectator ions, ions which occur in the same form on both sides of the equation. These are \(Na^{+}\) and \(Cl^{-}\).Hence, the net ionic equation is \(\mathrm{S^{2-}(aq) + Zn^{2+}(aq)} \longrightarrow\)
03

Problem b: \(\mathrm{K}_{3} \mathrm{PO}_{4}(a q)+3 \mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow\)

Start with the full ionic equation:\(\mathrm{3K^{+}(aq) + PO_{4}^{3-}(aq) + 3Sr^{2+}(aq) + 6NO_{3}^{-}(aq)} \longrightarrow\)Remove the spectator ions, which are \(K^{+}\) and \(NO_{3}^{-}\), to get the net ionic equation:\(\mathrm{PO_{4}^{3-}(aq) + 3Sr^{2+}(aq)} \longrightarrow\)
04

Problem c: \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow\)

Break down the reactants into ions for the full ionic equation:\(\mathrm{Mg^{2+}(aq) + 2NO_{3}^{-}(aq) + 2Na^{+}(aq) + 2OH^{-}(aq)} \longrightarrow\)Remove the spectator ions, here again, \(Na^{+}\) and \(NO_{3}^{-}\), to find the net ionic equation:\(\mathrm{Mg^{2+}(aq) + 2OH^{-}(aq)} \longrightarrow\)

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Most popular questions from this chapter

Identify each of the following species as a Bronsted acid, base, or both: (a) HI, (b) \(\mathrm{CH}_{3} \mathrm{COO}^{-}\), (c) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (d) \(\mathrm{HSO}_{4}^{-}\)

What is an oxidation number? How is it used to identify redox reactions? Explain why, except for ionic compounds, oxidation number does not have any physical significance.

Give the oxidation number for the following species: \(\mathrm{H}_{2}, \mathrm{Se}_{8}, \mathrm{P}_{4}, \mathrm{O}, \mathrm{U}, \mathrm{As}_{4}, \mathrm{~B}_{12}\)

How many grams of \(\mathrm{NaCl}\) are required to precipitate most of the \(\mathrm{Ag}^{+}\) ions from \(2.50 \times 10^{2} \mathrm{~mL}\) of \(0.0113 \mathrm{MAgNO}_{3}\) solution? Write the net ionic equation for the reaction.

Phosphorus forms many oxoacids. Indicate the oxidation number of phosphorus in each of the following acids: (a) \(\mathrm{HPO}_{3},\) (b) \(\mathrm{H}_{3} \mathrm{PO}_{2},\) (c) \(\mathrm{H}_{3} \mathrm{PO}_{3},\) d) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (e) \(\mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7},\) (f) \(\mathrm{H}_{5} \mathrm{P}_{3} \mathrm{O}_{10}\).
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