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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. (a) Write the molecular and net ionic equations for this reaction. (b) Based on the definitions of acid and base, what ion is the base in this reaction? (c) What is the acid in the reaction? (d) What is the spectator ion in the reaction?

Short Answer

Expert verified
The balanced molecular equation is: K2O(s) + H2O(l) -> 2K^(+)(aq) + 2OH^(-)(aq). The net ionic equation is: O^(2-)(aq) + H2O(l) -> 2OH^(-)(aq). The base in the reaction is the oxide ion (O^(2-)). The acid in the reaction is water (H2O), and the spectator ion in the reaction is the potassium ion (K^+).

Step by step solution

01

Write the balanced molecular equation

To write the balanced molecular equation, we need to know the reactants and the products of the reaction. In this case, the reactants are K2O (potassium oxide) and water (H2O). When K2O dissolves in water, it forms an oxide ion (O^2-) and two potassium ions (K^+). The oxide ion reacts with water to form hydroxide ions (OH^-). The balanced molecular equation is: K2O(s) + H2O(l) -> 2K^(+)(aq) + 2OH^(-)(aq)
02

Write the balanced net ionic equation

To write the net ionic equation, we need to break the molecular equation into its ionic components. Keeping in mind that K2O is a solid and H2O is a liquid, for the remaining ions, we simply write them as separate entities. Note that solid and liquid substances do not break into ions. Net ionic equation: O^(2-)(aq) + H2O(l) -> 2OH^(-)(aq)
03

Identify the base in the reaction

Based on the definitions of acids and bases, an acid is a substance that donates a proton (H^+), and a base is a substance that accepts a proton (H^+). From the net ionic equation, we can see that the oxide ion (O^(2-)) is accepting a proton and forming hydroxide ions (OH^(-)). Therefore, the base in the reaction is the oxide ion (O^(2-)).
04

Identify the acid in the reaction

The acid in the reaction is the substance that donates a proton (H^+) to the base. In the net ionic equation, the water molecule (H2O) donates a proton to the oxide ion (O^(2-)). Hence, the acid in the reaction is water (H2O).
05

Identify the spectator ion in the reaction

Spectator ions are ions that do not participate in the chemical reaction and remain unchanged. In this case, the potassium ion (K^+) does not participate in the reaction and remains unchanged throughout the process. Therefore, the spectator ion in the reaction is the potassium ion (K^+).

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Most popular questions from this chapter

When carbon dioxide dissolves in water, it is in equilibrium with carbonic acid \(\mathrm{H}_{2} \mathrm{CO}_{3},\) which is a weak electrolyte. What solutes are present in aqueous solution of this compound? Write the chemical equation for the ionization of \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

Complete and balance the following molecular equations, and then write the net ionic equation for each: (a) \(\mathrm{HBr}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow\) (b) \(\mathrm{Cu}(\mathrm{OH})_{2}(s)+\mathrm{HClO}_{4}(a q) \longrightarrow\) (c) \(\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow\)

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(a) By titration, \(15.0 \mathrm{~mL}\) of \(0.1008 \mathrm{Msodium}\) hydroxide is needed to neutralizea \(0.2053-\mathrm{g}\) sample of a weak acid. What is the molar mass of the acid if it is monoprotic? (b) An elemental analysis of the acid indicates that it is composed of $5.899 \mathrm{H}, 70.6 \% \mathrm{C},\( and \)23.5 \% \mathrm{O}$ by mass. What is its molecular formula?

Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodium bicarbonate on it and then mopping up the resulting solution. The sodium bicarbonate reacts with sulfuric acid according to: $$ \begin{aligned} 2 \mathrm{NaHCO}_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+& \\ & 2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g) \end{aligned} $$ Sodium bicarbonate is added until the fizzing due to the formation of \(\mathrm{CO}_{2}(g)\) stops. If \(27 \mathrm{~mL}\) of $6.0 \mathrm{MH}_{2} \mathrm{SO}_{4}\( was spilled, what is the minimum mass of \)\mathrm{NaHCO}_{3}$ that must be added to the spill to neutralize the acid?
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