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Chapter 5: Problem 22

Predict in each case whether a reaction is likely to occur. If so, write a net ionic equation. (a) $\mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{CuCl}_{2}(\mathrm{aq}) \longrightarrow$ (b) $\mathrm{Na}_{2} \mathrm{S}(\mathrm{aq})+\mathrm{FeCl}_{2}(\mathrm{aq}) \longrightarrow$ (c) $\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{aq})+\mathrm{AgNO}_{3}(\mathrm{aq}) \longrightarrow$

Short Answer

Expert verified
(a) No reaction occurs, hence no net ionic equation can be written. (b) Similarly, no reaction happens and no net ionic equation needed here. (c) The reaction here gives the net ionic equation as : \(2Ag^{+} (aq) + CO3^{2 -} (aq) \longrightarrow Ag2CO3 (s)\).

Step by step solution

01

Assess the reactivity

Looking at the reactivity series, silver (Ag) is less reactive than copper (Cu). Thus it is unlikely that copper would be displaced by silver in the first equation. Based on the reactivity series, there's no reaction.
02

Write the net ionic equation for the reaction

The first equation doesn't proceed, so there's no reaction, hence no net ionic equation.
03

Assess reactivity for second equation

The second reaction involves Na2S(aq) + FeCl2(aq). Considering the reactivity series sodium (Na) is more reactive than iron (Fe), implying sodium will not displace iron. So, no reaction occurs here.
04

Write the net ionic equation for the second reaction

As the second reaction doesn't occur, no net ionic equation will be needed.
05

Assess reactivity for third equation

The third equation is Na2CO3(aq) + AgNO3(aq). Based on the solubility rules, Ag+ ions would combine with CO3- ions to form the precipitate Ag2CO3.
06

Write the net ionic equation for the third reaction

Here, a reaction occurs. Sodium and nitrate are spectator ions and do not participate in the reaction. This leaves: \(2Ag^{+} (aq) + CO3^{2 -} (aq) \longrightarrow Ag2CO3 (s)\). This is the net ionic equation for the third reaction.

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Most popular questions from this chapter

What volume of \(0.248 \mathrm{M} \mathrm{CaCl}_{2}\) must be added to \(335 \mathrm{mL}\) of \(0.186 \mathrm{M} \mathrm{KCl}\) to produce a solution with a concentration of \(0.250 \mathrm{M} \mathrm{Cl}^{-2}\) Assume that the solution volumes are additive.

Balance these equations for redox reactions occurring in acidic solution. (a) $\mathrm{P}_{4}(\mathrm{s})+\mathrm{NO}_{3}^{-} \longrightarrow \mathrm{H}_{2} \mathrm{PO}_{4}^{-}+\mathrm{NO}(\mathrm{g})$ (b) $\mathrm{S}_{2} \mathrm{O}_{3}^{2-}+\mathrm{MnO}_{4}^{-} \longrightarrow \mathrm{SO}_{4}^{2-}+\mathrm{Mn}^{2+}$ (c) $\mathrm{HS}^{-}+\mathrm{HSO}_{3}^{-} \longrightarrow \mathrm{S}_{2} \mathrm{O}_{3}^{2-}$ (d) $\mathrm{Fe}^{3+}+\mathrm{NH}_{3} \mathrm{OH}^{+} \longrightarrow \mathrm{Fe}^{2+}+\mathrm{N}_{2} \mathrm{O}(\mathrm{g})$

Sodium hydroxide used to make standard \(\mathrm{NaOH}(\mathrm{aq})\) solutions for acid-base titrations is invariably contaminated with some sodium carbonate. (a) Explain why, except in the most precise work, the presence of this sodium carbonate generally does not seriously affect the results obtained, for example, when \(\mathrm{NaOH}(\mathrm{aq})\) is used to titrate HCl(aq). (b) Conversely, show that if \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) comprises more than \(1 \%\) to \(2 \%\) of the solute in NaOH(aq), the titration results are affected.

Household ammonia, used as a window cleaner and for other cleaning purposes, is \(\mathrm{NH}_{3}(\mathrm{aq}) .\) The \(\mathrm{NH}_{3}\) present in a 5.00 \(\mathrm{mL}\) sample is neutralized by 28.72 \(\mathrm{mL}\) of \(1.021 \mathrm{M} \mathrm{HCl}\). The net ionic equation for the neutralization is \(\mathrm{NH}_{3}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \longrightarrow \mathrm{NH}_{4}^{+}(\mathrm{aq})\) What is the molarity of \(\mathrm{NH}_{3}\) in the sample?

Explain the important distinctions between (a) a strong electrolyte and strong acid; (b) an oxidizing agent and reducing agent; (c) precipitation reactions and neutralization reactions; (d) half-reaction and overall reaction.
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