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Chapter 4: Problem 41

Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each: (a) solid cadmium sulfide reacts with an aqueous solution of sulfuric acid; (b) solid magnesium carbonate reacts with an aqueous solution of perchloric acid.

Short Answer

Expert verified
(a) The balanced molecular and net ionic equations for the reaction between solid cadmium sulfide and aqueous sulfuric acid are: CdS (s) + H2SO4 (aq) 鈫� CdSO4 (aq) + H2S (g) CdS (s) + 2H鈦� (aq) 鈫� Cd虏鈦� (aq) + H2S (g) The gas formed in this reaction is hydrogen sulfide (H2S). (b) The balanced molecular and net ionic equations for the reaction between solid magnesium carbonate and aqueous perchloric acid are: MgCO3 (s) + 2HClO4 (aq) 鈫� Mg(ClO4)2 (aq) + CO2 (g) + H2O (l) MgCO3 (s) + 2H鈦� (aq) 鈫� Mg虏鈦� (aq) + CO2 (g) + H2O (l) The gas formed in this reaction is carbon dioxide (CO2).

Step by step solution

01

Write the unbalanced equation

The given reaction is between solid cadmium sulfide (CdS) and an aqueous solution of sulfuric acid (H2SO4). Write the unbalanced equation for the reaction: CdS (s) + H2SO4 (aq) 鈫� ...
02

Predict the products and balance the equation

The reaction between CdS and H2SO4 will form cadmium sulfate (CdSO4) and hydrogen sulfide gas (H2S). Write the balanced equation for the reaction: CdS (s) + H2SO4 (aq) 鈫� CdSO4 (aq) + H2S (g)
03

Write the net ionic equation

First, write the complete ionic equation: CdS (s) + 2H鈦� (aq) + SO鈧劼测伝 (aq) 鈫� Cd虏鈦� (aq) + SO鈧劼测伝 (aq) + H2S (g) Eliminate the spectator ions, in this case, SO鈧劼测伝 (aq), to get the net ionic equation: CdS (s) + 2H鈦� (aq) 鈫� Cd虏鈦� (aq) + H2S (g) The gas formed in this reaction is hydrogen sulfide (H2S). (b) Solid magnesium carbonate reacts with an aqueous solution of perchloric acid.
04

Write the unbalanced equation

The given reaction is between solid magnesium carbonate (MgCO3) and an aqueous solution of perchloric acid (HClO4). Write the unbalanced equation for the reaction: MgCO3 (s) + HClO4 (aq) 鈫� ...
05

Predict the products and balance the equation

The reaction between MgCO3 and HClO4 will form magnesium perchlorate (Mg(ClO4)2) and carbon dioxide gas (CO2) as well as water (H2O). Write the balanced equation for the reaction: MgCO3 (s) + 2HClO4 (aq) 鈫� Mg(ClO4)2 (aq) + CO2 (g) + H2O (l)
06

Write the net ionic equation

First, write the complete ionic equation: MgCO3 (s) + 2H鈦� (aq) + 2ClO鈧勨伝 (aq) 鈫� Mg虏鈦� (aq) + 2ClO鈧勨伝 (aq) + CO2 (g) + H2O (l) Eliminate the spectator ions, in this case, 2ClO鈧勨伝 (aq), to get the net ionic equation: MgCO3 (s) + 2H鈦� (aq) 鈫� Mg虏鈦� (aq) + CO2 (g) + H2O (l) The gas formed in this reaction is carbon dioxide (CO2).

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Most popular questions from this chapter

Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (a) \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}\) and \(\mathrm{NaOH}\), (b) \(\mathrm{NaOH}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\), (c) \(\mathrm{Na}_{2} \mathrm{~S}\) and \(\mathrm{Cu}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\).

Which of the following ions will always be a spectator ion in a precipitation reaction? (a) Cl", (b) \(\mathrm{NO}_{3}^{-}\), (c) \(\mathrm{NH}_{4}^{+},(\mathrm{d}) \mathrm{S}^{2-},(\mathrm{e}) \mathrm{SO}_{4}{ }^{2-}\). Explain briefly. [Section 4.2]

(a) What volume of \(0.115 \mathrm{M} \mathrm{HClO}_{4}\) solution is needed to neutralize \(50.00 \mathrm{~mL}\) of \(0.0875 \mathrm{M} \mathrm{NaOH}\) ? (b) What volume of \(0.128 \mathrm{M} \mathrm{HCl}\) is needed to neutralize \(2.87 \mathrm{~g}\) of \(\mathrm{Mg}(\mathrm{OH})_{2} ?\) (c) If \(25.8 \mathrm{~mL}\) of \(\mathrm{AgNO}_{3}\) is needed to precipitate all the \(\mathrm{Cl}^{-}\) ions in a \(785-\mathrm{mg}\) sample of \(\mathrm{KCl}\) (forming \(\mathrm{AgCl}\), what is the molarity of the \(\mathrm{AgNO}_{3}\) solution? (d) If \(45.3 \mathrm{~mL}\) of \(0.108 \mathrm{M} \mathrm{HCl}\) solution is needed to neutralize a solution of \(\mathrm{KOH}\), how many grams of \(\mathrm{KOH}\) must be present in the solution?

The concentration of hydrogen peroxide in a solution is determined by titrating a \(10.0\) -mL sample of the solution with permanganate ion. $$ \begin{array}{r} 2 \mathrm{MnO}_{4}^{-}(a q)+5 \mathrm{H}_{2} \mathrm{O}_{2}(a q)+6 \mathrm{H}^{+}(a q) \longrightarrow \\ 2 \mathrm{Mn}^{2+}(a q)+5 \mathrm{O}_{2}(g)+8 \mathrm{H}_{2} \mathrm{O}(l) \end{array} $$ If it takes \(14.8 \mathrm{~mL}\) of \(0.134 \mathrm{M} \mathrm{MnO}_{4}^{-}\) solution to reach the equivalence point, what is the molarity of the hydrogen peroxide solution?

Methanol, \(\mathrm{CH}_{3} \mathrm{OH}\), and hydrogen chloride, \(\mathrm{HCl}\), are both molecular substances, yet an aqueous solution of methanol does not conduct an electrical current, whereas a solution of \(\mathrm{HCl}\) does conduct. Account for this difference. [Section 4.1]
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