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Chapter 8: Problem 41

Write a total ionic equation and a net ionic equation for each of the following reactions. a. \(\mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \longrightarrow\) \(\mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) b. \(\mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g)\) c. \(\mathrm{CdCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \longrightarrow\) \(2 \mathrm{NaCl}(a q)+\mathrm{CdCO}_{3}(s)\)

Short Answer

Expert verified
The net ionic equations for the given reactions are: a. \(\mathrm{H}^{+}(a q) + \mathrm{OH}^{-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)\), b. \(\mathrm{Mg}(s) + 2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Mg}^{2+}(a q) + \mathrm{H}_{2}(g)\), c. \(\mathrm{Cd}^{2+}(a q) + \mathrm{CO}_3{}^{2-}(a q) \longrightarrow \mathrm{CdCO}_{3}(s)\)

Step by step solution

01

Write total ionic equation

Convert each compound into its respective ions for a total ionic equation.\na. \(\mathrm{H}^{+}(a q)+ \mathrm{Cl}^{-}(a q) + \mathrm{Na}^{+}(a q) + \mathrm{OH}^{-}(a q) \longrightarrow \mathrm{Na}^{+}(a q) + \mathrm{Cl}^{-}(a q) + \mathrm{H}_{2} \mathrm{O}(l)\)\nb. \(\mathrm{Mg}^{2+}(s) + 2 \mathrm{H}^{+}(a q) + 2 \mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{Mg}^{2+}(a q) + 2 \mathrm{Cl}^{-}(a q) + \mathrm{H}_{2}(g)\)\nc. \(\mathrm{Cd}^{2+}(a q) + 2 \mathrm{Cl}^{-}(a q) + 2 \mathrm{Na}^{+}(a q) + \mathrm{CO}_3{}^{2-}(a q) \longrightarrow 2 \mathrm{Na}^{+}(a q) + 2 \mathrm{Cl}^{-}(a q) + \mathrm{CdCO}_{3}(s)\)
02

Write net ionic equation

In the net ionic equation, remove ions present on both sides of the equation as these are the 'spectator ions'. They do not participate in the reaction.\na. \(\mathrm{H}^{+}(a q) + \mathrm{OH}^{-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)\) (Na+ and Cl- ions were removed)\nb. \(\mathrm{Mg}(s) + 2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Mg}^{2+}(a q) + \mathrm{H}_{2}(g)\) (Cl- ions were removed)\nc. \(\mathrm{Cd}^{2+}(a q) + \mathrm{CO}_3{}^{2-}(a q) \longrightarrow \mathrm{CdCO}_{3}(s)\) (Na+ and Cl- ions were removed)

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Most popular questions from this chapter

The following equations are incorrect in some way. Identify and correct each error, and then balance each equation. $$\begin{array}{l}{\text { a. } \mathrm{Li}+\mathrm{O}_{2} \rightarrow \mathrm{LiO}_{2}} \\ {\text { b. } \mathrm{MgCO}_{3} \rightarrow \mathrm{Mg}+\mathrm{C}+3 \mathrm{O}_{2}} \\ {\text { c. } \mathrm{NaI}+\mathrm{Cl}_{2} \rightarrow \mathrm{NaCl}+\mathrm{I}} \\ {\text { d. } \mathrm{AgNO}_{3}+\mathrm{CaCl}_{2} \rightarrow \mathrm{Ca}\left(\mathrm{NO}_{3}\right)+\mathrm{AgCl}_{2}} \\ {\text { e. } 3 \mathrm{Mg}+2 \mathrm{FeBr}_{3} \rightarrow \mathrm{Fe}_{2} \mathrm{Mg}_{3}+3 \mathrm{Br}_{2}}\end{array}$$

Identify the type of reaction for each of the following. Then, predict products for the reaction, and balance the equation." reaction occurs, write "no reaction." $$ \begin{array}{l}{\text { a. water }+\text { lithium } \longrightarrow} \\\ {\text { b. silver nitrate + hydrochloric acid } \rightarrow} \\ {\text { c. hydrogen iodide } \rightarrow}\end{array} $$

Design an experiment for judging the value and efficacy of different antacids. Include NaHCO \(_{3}, \operatorname{Mg}(\mathrm{OH})_{2}, \mathrm{CaCO}_{3},\) and \(\mathrm{Al}(\mathrm{OH})_{3}\) in your tests. Discover which one neutralizes the most acid and what byproducts form. Show your experiment to your teacher. If your experiment is approved, obtain the necessary chemicals from your teacher and test your procedure.

Predict the products for each of the following reactions. Write a total ionic equation and a net ionic equation for each reaction. If no reaction occurs, write "no reaction." $$\begin{array}{l}{\text { a. } \mathrm{Li}_{2} \mathrm{CO}_{3}(a q)+\mathrm{BaBr}_{2}(a q) \longrightarrow} \\ {\text { b. } \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q) \rightarrow} \\ {\text { c. } \mathrm{Al}(s)+\mathrm{NiCl}_{2}(a q) \rightarrow} \\ {\text { d. } \mathrm{K}_{2} \mathrm{CO}_{3}(a q)+\mathrm{FeCl}_{3}(a q) \rightarrow}\end{array}$$

Balance each of the following: $$ \begin{array}{l}{\text { a. } \mathrm{H}_{2}+\mathrm{Cl}_{2} \rightarrow \mathrm{HCl}} \\ {\text { b. } \mathrm{Al}+\mathrm{Fe}_{2} \mathrm{O}_{3} \rightarrow \mathrm{Al}_{2} \mathrm{O}_{3}+\mathrm{Fe}} \\ {\text { c. } \mathrm{Ba}\left(\mathrm{ClO}_{3}\right)_{2} \rightarrow \mathrm{BaCl}_{2}+\mathrm{O}_{2}} \\ {\text { d. } \mathrm{Cu}+\mathrm{HNO}_{3} \rightarrow \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{NO}+\mathrm{H}_{2} \mathrm{O}}\end{array} $$
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