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Chapter 4: Problem 65

Complete the following acid-base reactions with balanced molecular, total ionic, and net ionic equations: (a) Potassium hydroxide \((a q)+\) hydrobromic acid \((a q) \longrightarrow\) (b) Ammonia(aq) + hydrochloric acid \((a q) \longrightarrow\)

Short Answer

Expert verified
(a) Net ionic: \(OH^- + H^+ \longrightarrow H_2O\). (b) Net ionic: \(NH_3 + H^+ \longrightarrow NH_4^+\)

Step by step solution

01

Write the Reactants and Products

For each reaction, write the reactants and identify the products of the reaction. For (a), potassium hydroxide reacts with hydrobromic acid, and for (b), ammonia reacts with hydrochloric acid.
02

Molecular Equation (a)

Write the balanced molecular equation for potassium hydroxide and hydrobromic acid: \[ KOH(aq) + HBr(aq) \longrightarrow KBr(aq) + H_2O(l) \]
03

Total Ionic Equation (a)

Write the total ionic equation for the reaction: \[ K^+(aq) + OH^-(aq) + H^+(aq) + Br^-(aq) \longrightarrow K^+(aq) + Br^-(aq) + H_2O(l) \]
04

Net Ionic Equation (a)

Eliminate the spectator ions to find the net ionic equation: \[ OH^-(aq) + H^+(aq) \longrightarrow H_2O(l) \]
05

Molecular Equation (b)

Write the balanced molecular equation for ammonia and hydrochloric acid: \[ NH_3(aq) + HCl(aq) \longrightarrow NH_4Cl(aq) \]
06

Total Ionic Equation (b)

Write the total ionic equation for the reaction: \[ NH_3(aq) + H^+(aq) + Cl^-(aq) \longrightarrow NH_4^+(aq) + Cl^-(aq) \]
07

Net Ionic Equation (b)

Eliminate the spectator ions to find the net ionic equation: \[ NH_3(aq) + H^+(aq) \longrightarrow NH_4^+(aq) \]

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Molecular Equation
A molecular equation represents the complete chemical formulas of reactants and products. It doesn’t split ions into their ionic forms. Essentially, it shows the reactants, which are original substances, and the products, which are new substances formed in the reaction.
In an acid-base reaction, the acid reacts with a base (often containing OH-) to produce water and a salt.
  • For example, in the reaction between potassium hydroxide (KOH) and hydrobromic acid (HBr), the molecular equation is: ewline \[ KOH(aq) + HBr(aq) \rightarrow KBr(aq) + H_2O(l) \]
  • In the reaction between ammonia (NH3) and hydrochloric acid (HCl), the molecular equation is: ewline \[ NH_3(aq) + HCl(aq) \rightarrow NH_4Cl(aq) \]
This gives a clear picture of the overall reaction, showing the compounds directly involved.
Total Ionic Equation
The total ionic equation breaks down all the aqueous compounds into their constituent ions. This helps to identify the actual ionic species present in the solution and shows the full form of the reaction happening at the ionic level.
When writing a total ionic equation, we dissociate all strong electrolytes (compounds that break into ions in solution).
  • For potassium hydroxide and hydrobromic acid, the total ionic equation is:ewline \[ K^+(aq) + OH^-(aq) + H^+(aq) + Br^-(aq) \rightarrow K^+(aq) + Br^-(aq) + H_2O(l) \]
  • For ammonia and hydrochloric acid, the total ionic equation is:ewline \[ NH_3(aq) + H^+(aq) + Cl^-(aq) \rightarrow NH_4^+(aq) + Cl^-(aq) \]
This form of the equation reveals all the ions that are present in the course of the reaction.
Net Ionic Equation
The net ionic equation removes the spectator ions (ions that do not participate in the actual chemical change) and only includes the ions that directly take part in the formation of the products.
The purpose is to focus on the substances that undergo the chemical change.
  • For potassium hydroxide and hydrobromic acid, the net ionic equation is:ewline \[ OH^-(aq) + H^+(aq) \rightarrow H_2O(l) \]
  • For ammonia and hydrochloric acid, the net ionic equation is:ewline \[ NH_3(aq) + H^+(aq) \rightarrow NH_4^+(aq) \]
This simplified form shows the essence of the reaction, specifically highlighting the hydrogen and hydroxide ions forming water, or the ammonia reacting with hydrogen ions to form ammonium ions.

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Most popular questions from this chapter

Does an aqueous solution of each of the following conduct an electric current? Explain. (a) Cesium bromide (b) Hydrogen iodide

How many total moles of ions are released when each of the following dissolves in water? (a) \(0.734 \mathrm{~mol}\) of \(\mathrm{Na}_{2} \mathrm{HPO}_{4}\) (b) \(3.86 \mathrm{~g}\) of \(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}\) (c) \(8.66 \times 10^{20}\) formula units of \(\mathrm{NiCl}_{2}\)

How many moles of \(\mathrm{H}^{+}\) ions are present in each of the following aqueous solutions? (a) \(1.40 \mathrm{~L}\) of \(0.25 \mathrm{M}\) perchloric acid (b) \(6.8 \mathrm{~mL}\) of \(0.92 \mathrm{M}\) nitric acid (c) \(2.6 \mathrm{~L}\) of \(0.085 \mathrm{M}\) hydrochloric acid

What occurs on the molecular level when an ionic compound dissolves in water?

Why do decomposition redox reactions typically have compounds as reactants, whereas combination redox and displacement redox reactions have one or more elements as reactants?
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