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Chapter 4: Problem 44

As \(\mathrm{K}_{2} \mathrm{O}\) dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions. Write the molecular and net ionic equations for this reaction. Based on the definitions of acid and base, what ion is the base in this reaction? What is the acid? What is the spectator ion in the reaction?

Short Answer

Expert verified
The balanced chemical equation for the reaction between \(\mathrm{K}_{2} \mathrm{O}\) and water is: \[\mathrm{K}_{2}\mathrm{O} + \mathrm{H}_{2}\mathrm{O} \rightarrow 2\mathrm{KOH}\] The molecular and net ionic equation is: \[\mathrm{K}_{2}\mathrm{O} + \mathrm{H}_{2}\mathrm{O} \rightarrow 2\mathrm{K}^{+} + 2\mathrm{OH}^{-}\] In this reaction, the base is the oxide ion (O^2-), the acid is water (\(\mathrm{H}_{2}\mathrm{O}\)), and there is no spectator ion.

Step by step solution

01

Write the balanced chemical equation

First, we write the balanced chemical equation for the reaction between \(\mathrm{K}_{2} \mathrm{O}\) and water: \[\mathrm{K}_{2}\mathrm{O} + \mathrm{H}_{2}\mathrm{O} \rightarrow 2\mathrm{KOH}\] Now, let's break down the soluble ionic compounds into their ions in order to write the molecular equation.
02

Write the molecular equation

The molecular equation involves breaking down all soluble ionic compounds into their individual ions: \[\mathrm{K}_{2}\mathrm{O} + \mathrm{H}_{2}\mathrm{O} \rightarrow 2\mathrm{K}^{+} + 2\mathrm{OH}^{-}\]
03

Write the net ionic equation

The net ionic equation can be written by removing the spectator ions, which are the ions that aren't involved in the actual reaction. In this case, there are no spectator ions, so the net ionic equation remains as: \[\mathrm{K}_{2}\mathrm{O} + \mathrm{H}_{2}\mathrm{O} \rightarrow 2\mathrm{K}^{+} + 2\mathrm{OH}^{-}\]
04

Identify the acid, base, and spectator ion

Now, let's identify the acid and base in the reaction. The base is the species that accepts a hydrogen ion (H+), which is the oxide ion (O^2-) reacting with water to form hydroxide ions (OH-). Therefore, O^2- is the base. The acid is the species that donates a hydrogen ion (H+). In this reaction, water donates a hydrogen ion to the oxide ion, so H2O is the acid. Since there are no spectator ions in this reaction, we can say there is no spectator ion in this case.

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Most popular questions from this chapter

Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (a) Aqueous acetic acid is neutralized by aqueous potassium hydroxide. (b) Solid chromium(III) hydroxide reacts with nitric acid. (c) Aqueous hypochlorous acid and aqueous calcium hydroxide react.

Name the spectator ions in any reactions that may be involved when each of the following pairs of solutions are mixed. (a) \(\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{aq})\) and \(\mathrm{MgSO}_{4}(a q)\) (b) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) and \(\mathrm{Na}_{2} \mathrm{~S}(a q)\) (c) \(\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}(a q)\) and \(\mathrm{CaCl}_{2}(a q)\)

(a) How many milliliters of \(0.120 \mathrm{M} \mathrm{HCl}\) are needed to completely neutralize \(50.0 \mathrm{~mL}\) of \(0.101 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) solution? (b) How many milliliters of \(0.125 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) are needed to neutralize \(0.200 \mathrm{~g}\) of \(\mathrm{NaOH}\) ? (c) If \(55.8 \mathrm{~mL}\) of \(\mathrm{BaCl}_{2}\) solution is needed to precipitate all the sulfate ion in a 752 -mg sample of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\), what is the molarity of the solution? (d) If \(42.7 \mathrm{~mL}\) of \(0.208 \mathrm{M} \mathrm{HCl}\) solution is needed to neutralize a solution of \(\mathrm{Ca}(\mathrm{OH})_{2}\), how many grams of \(\mathrm{Ca}(\mathrm{OH})_{2}\) must be in the solution?

The metal cadmium tends to form \(\mathrm{Cd}^{2+}\) ions. The following observations are made: (i) When a strip of zinc metal is placed in \(\mathrm{CdCl}_{2}(a q)\), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)\), nickel metal is deposited on the strip. (a) Write net ionic equations to explain each of the observations made above. (b) What can you conclude about the position of cadmium in the activity series? (c) What experiments would you need to perform to locate more precisely the position of cadmium in the activity series?

Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: (a) \(\mathrm{NiCl}_{2}\) (b) \(\mathrm{Ag}_{2} \mathrm{~S},(\mathrm{c}) \mathrm{Cs}_{3} \mathrm{PO}_{4}\) (d) \(\mathrm{SrCO}_{3}\) (e) \(\mathrm{PbSO}_{4}\).
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