Exercises: Precipitation, Acid-Base, and Redox Reactions
Classify each reaction as precipitation, acid-base (neutralization), or oxidation-reduction, and give a short reason for each: (a)…
Classify each reaction as precipitation, acid-base (neutralization), or oxidation-reduction, and give a short reason for each:
(a) $\text{HCl}(aq) + \text{NaOH}(aq) \rightarrow \text{NaCl}(aq) + \text{H}_2\text{O}(l)$
(b) $\text{Zn}(s) + \text{CuSO}_4(aq) \rightarrow \text{ZnSO}_4(aq) + \text{Cu}(s)$
(c) $\text{AgNO}_3(aq) + \text{NaCl}(aq) \rightarrow \text{AgCl}(s) + \text{NaNO}_3(aq)$
Define oxidation and reduction in terms of the transfer of electrons. Then, in the reaction $2\,\text{Na}(s) + \text{Cl}2(g) \rightarrow 2\,\text{NaCl}(s)$, identify…
Define oxidation and reduction in terms of the transfer of electrons. Then, in the reaction $2\,\text{Na}(s) + \text{Cl}_2(g) \rightarrow 2\,\text{NaCl}(s)$, identify which species is oxidized and which is reduced.
Use the general solubility rules (compounds of $\text{Na}^+$, $\text{K}^+$, $\text{NH}4^+$ and $\text{NO}3^-$ are soluble; most carbonates are insoluble except those of…
Use the general solubility rules (compounds of $\text{Na}^+$, $\text{K}^+$, $\text{NH}_4^+$ and $\text{NO}_3^-$ are soluble; most carbonates are insoluble except those of group 1 ions) to decide whether each compound is soluble or insoluble in water: (a) $\text{KNO}_3$, (b) $\text{CaCO}_3$, (c) $\text{Na}_2\text{CO}_3$.
Sofia mixes aqueous solutions of lead(II) nitrate, $\text{Pb(NO}3)2$, and potassium iodide, KI. Write the balanced molecular equation for the double replacement…
Sofia mixes aqueous solutions of lead(II) nitrate, $\text{Pb(NO}_3)_2$, and potassium iodide, KI. Write the balanced molecular equation for the double replacement reaction. Use the rules that nitrates are soluble and that most iodides are soluble except those of $\text{Pb}^{2+}$, $\text{Ag}^+$ and $\text{Hg}_2^{2+}$ to identify the precipitate, and include state symbols.
For the reaction $\text{Mg}(s) + 2\,\text{HCl}(aq) \rightarrow \text{MgCl}2(aq) + \text{H}2(g)$, assign oxidation numbers to Mg, H, and Cl on both sides of the equation.…
For the reaction $\text{Mg}(s) + 2\,\text{HCl}(aq) \rightarrow \text{MgCl}_2(aq) + \text{H}_2(g)$, assign oxidation numbers to Mg, H, and Cl on both sides of the equation. Identify the species oxidized and reduced, the oxidizing agent, and the reducing agent.
Jayden mixes aqueous barium chloride, $\text{BaCl}2$, with aqueous sodium sulfate, $\text{Na}2\text{SO}4$. (a) Write the balanced net ionic equation, given that…
Jayden mixes aqueous barium chloride, $\text{BaCl}_2$, with aqueous sodium sulfate, $\text{Na}_2\text{SO}_4$. (a) Write the balanced net ionic equation, given that $\text{BaSO}_4$ is insoluble. (b) Identify the spectator ions. (c) Explain why this is not a redox reaction.
A lab tech has four unlabeled beakers, each containing a clear, colorless aqueous solution of one of these: $\text{NaOH}$, $\text{HNO}3$, $\text{Na}2\text{SO}4$, or…
A lab tech has four unlabeled beakers, each containing a clear, colorless aqueous solution of one of these: $\text{NaOH}$, $\text{HNO}_3$, $\text{Na}_2\text{SO}_4$, or $\text{Pb(NO}_3)_2$. She mixes pairs and records the results:
| Mixture | Observation |
|---|---|
| A + B | White solid forms |
| A + C | No visible change; the mixture feels warm |
| B + D | White solid forms |
| C + D | No visible change |
Assume $\text{Pb(OH)}_2$ and $\text{PbSO}_4$ are insoluble white solids. Identify A, B, C, and D, and write a balanced net ionic equation for each of the three mixtures that shows a reaction. Classify each reaction type.
Emma drops a strip of copper metal into a solution of silver nitrate, $\text{AgNO}3(aq)$, and after an hour she sees a gray, feathery solid on the strip while the…
Emma drops a strip of copper metal into a solution of silver nitrate, $\text{AgNO}_3(aq)$, and after an hour she sees a gray, feathery solid on the strip while the solution turns pale blue. (a) Write the balanced net ionic equation. (b) Assign oxidation numbers and identify what is oxidized and what is reduced. (c) Explain how each observation supports your equation. (d) Explain why this reaction is redox and not a precipitation reaction, even though a solid forms.