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Chapter 1: Problem 4

Choose the correct net ionic equation representing the reaction that occurs when solutions of potassium carbonate and copper (I) chloride are mixed. (A) \(\mathrm{K}_{2} \mathrm{CO}_{3}(a q)+2 \mathrm{CuCl}(a q) \rightarrow 2 \mathrm{KCl}(a q)+\mathrm{Cu}_{2} \mathrm{CO}_{3}(s)\) (B) \(\mathrm{K}_{2} \mathrm{CO}_{3}(a q)+2 \mathrm{CuCl}(a q) \rightarrow 2 \mathrm{KCl}(\mathrm{s})+\mathrm{Cu}_{2} \mathrm{CO}_{3}(a q)\) (C) \(\mathrm{CO}_{3}^{2-}+2 \mathrm{Cu}^{+} \rightarrow \mathrm{Cu}_{2} \mathrm{CO}_{3}\) (D) \(\mathrm{CO}_{3}^{2-}+\mathrm{Cu}^{2+} \rightarrow \mathrm{CuCO}_{3}(s)\)

Short Answer

Expert verified
The correct net ionic equation is (C) \(CO_{3}^{2-}+2Cu^{+} \rightarrow Cu_{2}CO_{3}\).

Step by step solution

01

Write the Complete Ionic Equations

First, it is important to write the complete ionic equations for all the given options. This means breaking apart all the compounds (except any solid, liquid, or gas products) into their ions. The correct full ionic equation for the reaction between potassium carbonate and copper (I) chloride is: \(2K^{+}(aq) + CO_{3}^{2-}(aq) + 2Cu^{+}(aq) + 2Cl^{-}(aq) \rightarrow 2K^{+}(aq) + 2Cl^{-}(aq) + Cu_{2}CO_{3}(s)\).
02

Comparison of Ionic and Net Ionic Equations

Next, compare the complete ionic equation to the proposed net ionic equations. In a net ionic equation, we 'cancel out' the spectator ions. Those are the ions that do not participate directly in the reaction. In our case, these are \(2K^{+}(aq)\) and \(2Cl^{-}(aq)\).
03

Choose the Correct Net Ionic Equation

Finally, look for the matching equation among the options given in the problem. The correct net ionic equation here will be the one that includes only the species taking part in the reaction: the carbonate ion \(CO_{3}^{2-}\) and copper (I) ion \(Cu^{+}\), as well as the solid product, copper (I) carbonate \(Cu_{2}CO_{3}\). Hence, the correct choice is: \(CO_{3}^{2-}+2Cu^{+} \rightarrow Cu_{2}CO_{3}\). This matches with option (C).

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Most popular questions from this chapter

Use the following information to answer questions 25-28. A voltaic cell is created using the following half-cells: \(\begin{array}{ll}{\mathrm{Cr}^{3+}+3 e \rightarrow \mathrm{Cr}(s)} & {E^{\circ}=-0.41 \mathrm{V}} \\ {\mathrm{Pb}^{2+}+2 e \rightarrow \mathrm{Pb}(s)} & {E^{\circ}=-0.12 \mathrm{V}}\end{array}\) The concentrations of the solutions in each half-cell are 1.0 M. Which of the following best describes the activity in the salt bridge as the reaction progresses? (A) Electrons flow through the salt bridge from the \(\mathrm{Pb} / \mathrm{Pb}^{2+}\) half-cell to the \(\mathrm{Cr} / \mathrm{Cr}^{3+}\) half-cell. (B) \(\quad \mathrm{Pb}^{2+}\) flows to the \(\mathrm{Cr} / \mathrm{Cr}^{3+}\) flows to the \(\mathrm{Pb} / \mathrm{Pb}^{2+}\) half-cell. (C) \(\mathrm{Na}^{+}\) flows to the \(\mathrm{Cr} / \mathrm{Cr}^{3+}\) half-cell, and \(\mathrm{Cl}^{-}\) flows to the \(\mathrm{Pb} / \mathrm{Pb}^{2+}\) half- cell. (D) \(\quad \mathrm{Na}^{+}\) flows to the \(\mathrm{Pb} / \mathrm{Pb}^{2}\) half- cell, and \(\mathrm{Cl}^{-}\) flows to the \(\mathrm{Cr} / \mathrm{Cr}^{3+}\) half- cell.

A student added 1 liter of a 1.0\(M\) \(\mathrm{KCl}\) solution to 1 liter of a 1.0 \(M\) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) solution. A lead chloride precipitate formed, and nearly all of the lead ions disappeared from the solution. Which of the following lists the ions remaining in the solution in order of decreasing concentration? (A) \(\left[\mathrm{NO}_{3}^{-}\right]>\left[\mathrm{K}^{+}\right]>\left[\mathrm{Pb}^{2+}\right]\) (B) \(\left[\mathrm{NO}_{3}^{-}\right]>\left[\mathrm{Pb}^{2+}\right]>\left[\mathrm{K}^{+}\right]\) (C) \(\left[\mathrm{K}^{+}\right]>\left[\mathrm{Pb}^{2+}\right]>\left[\mathrm{NO}_{3}^{-}\right]\) (D) \(\left[\mathrm{K}^{+}\right]>\left[\mathrm{NO}_{3}^{-}\right]>\left[\mathrm{Pb}^{2+}\right]\)

Questions 45-48 refer to the following. Inside a calorimeter, 100.0 \(\mathrm{mL}\) of 1.0 \(\mathrm{M}\) hydrocyanic acid (HCN), a weak acid, and 100.0 \(\mathrm{mL}\) of 0.50 \(\mathrm{M}\) sodium hydroxide are mixed. The temperature of the mixture rises from \(21.5^{\circ} \mathrm{C}\) to \(28.5^{\circ} \mathrm{C}\) . The specific heat of the mixture is approximately \(4.2 \mathrm{J} / \mathrm{g}^{\circ} \mathrm{C},\) and the density is identical to that of water. Identify the correct net ionic equation for the reaction that takes place. (A) \(\mathrm{HCN}(a q)+\mathrm{OH}^{-}(a q) \mapsto \mathrm{CN}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) (B) \(\mathrm{HCN}(a q)+\mathrm{NaOH}(a q) \leftrightarrow \mathrm{NaCN}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) (C) \(\mathrm{H}^{+}(a q)+\mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)\) (D) \(\mathrm{H}^{+}(a q)+\mathrm{CN}^{-}(a q)+\mathrm{Na}^{+}(a q)+\mathrm{OH}^{-}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CN}^{-}(a q)+\mathrm{Na}^{+}\) (aq)

The following reaction is found to be at equilibrium at 25°C: \(2 \mathrm{SO}_{3}(g) \leftrightarrow \mathrm{O}_{2}(g)+2 \mathrm{SO}_{2}(g) \quad \Delta H=-198 \mathrm{kJ} / \mathrm{mol}\) Which of the following would cause a reduction in the value for the equilibrium constant? (A) Increasing the amount of \(\mathrm{SO}_{3}\) (B) Reducing the amount of \(\mathrm{O}_{2}\) (C) Raising the temperature (D) Lowering the temperature

A sample of a compound known to consist of only carbon, hydrogen, and oxygen is found to have a total mass of 29.05 g. If the mass of the carbon is 18.02 g and the mass of the hydrogen is 3.03 g, what is the empirical formula of the compound? (A) \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}\) (B) \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\) (C) \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{3}\) (D) \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}_{2}\)
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