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Chapter 4: Problem 37

Complete and balance each of the following molecular equations (in aqueous solution); include phase labels. Then, for each, write the net ionic equation. a. \(\mathrm{NaOH}+\mathrm{HNO}_{3} \longrightarrow\) b. \(\mathrm{HCl}+\mathrm{Ba}(\mathrm{OH})_{2} \longrightarrow\) c. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}+\mathrm{Ca}(\mathrm{OH})_{2} \longrightarrow\) d. \(\mathrm{NH}_{3}+\mathrm{HNO}_{3} \longrightarrow\)

Short Answer

Expert verified
a. Net ionic: OH鈦� (aq) + H鈦� (aq) 鈫� H鈧侽 (l) b. Net ionic: OH鈦� (aq) + H鈦� (aq) 鈫� H鈧侽 (l) c. Net ionic: HC鈧侶鈧僌鈧� (aq) + OH鈦� (aq) 鈫� H鈧侽 (l) + C鈧侶鈧僌鈧傗伝 (aq) d. Net ionic: NH鈧� (aq) + H鈦� (aq) 鈫� NH鈧勨伜 (aq)

Step by step solution

01

Equation a - Write the balanced molecular equation

For equation a, sodium hydroxide reacts with nitric acid. Both compounds dissociate in water: NaOH (aq) + HNO鈧� (aq) 鈫� NaNO鈧� (aq) + H鈧侽 (l) This is already balanced, and the phases are included.
02

Equation a - Write the net ionic equation

Remove the spectator ions from the molecular equation. Sodium nitrate remains in solution as ions, and the reaction is essentially between the hydrogen ion and hydroxide ion: OH鈦� (aq) + H鈦� (aq) 鈫� H鈧侽 (l)
03

Equation b - Write the balanced molecular equation

For equation b, hydrochloric acid reacts with barium hydroxide: 2 HCl (aq) + Ba(OH)鈧� (aq) 鈫� BaCl鈧� (aq) + 2 H鈧侽 (l) This equation is balanced and includes the phase labels.
04

Equation b - Write the net ionic equation

Remove the spectator ions (Ba虏鈦� and Cl鈦�) from the molecular equation. The net ionic equation is: 2 OH鈦� (aq) + 2 H鈦� (aq) 鈫� 2 H鈧侽 (l) Or simplifying by dividing through by 2: OH鈦� (aq) + H鈦� (aq) 鈫� H鈧侽 (l)
05

Equation c - Write the balanced molecular equation

For equation c, acetic acid reacts with calcium hydroxide: 2 HC鈧侶鈧僌鈧� (aq) + Ca(OH)鈧� (aq) 鈫� Ca(C鈧侶鈧僌鈧�)鈧� (aq) + 2 H鈧侽 (l) This equation is balanced and the phases are included.
06

Equation c - Write the net ionic equation

Since calcium acetate remains in solution, the net ionic equation focuses on hydrogen ions from acetic acid reacting with hydroxide ions: 2 HC鈧侶鈧僌鈧� (aq) + 2 OH鈦� (aq) 鈫� 2 H鈧侽 (l) + 2 C鈧侶鈧僌鈧傗伝 (aq) Or simplifying by dividing by 2: HC鈧侶鈧僌鈧� (aq) + OH鈦� (aq) 鈫� H鈧侽 (l) + C鈧侶鈧僌鈧傗伝 (aq)
07

Equation d - Write the balanced molecular equation

For equation d, ammonia reacts with nitric acid to form ammonium nitrate: NH鈧� (aq) + HNO鈧� (aq) 鈫� NH鈧凬O鈧� (aq) The equation is balanced and includes the phase labels.
08

Equation d - Write the net ionic equation

Since ammonium nitrate is soluble, it dissociates into ions. The net ionic equation shows the formation of ammonium ion: NH鈧� (aq) + H鈦� (aq) 鈫� NH鈧勨伜 (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 provides a way to represent chemical reactions, showing the complete formulas of the reactants and products. They are written by combining reactants and the products they transform into, even if these substances exist as ions in solution. For example:
  • Sodium hydroxide reacting with nitric acid is shown as: \(\mathrm{NaOH} \,(\mathrm{aq}) + \mathrm{HNO}_3 \,(\mathrm{aq}) \rightarrow \mathrm{NaNO}_3 \,(\mathrm{aq}) + \mathrm{H}_2\mathrm{O} \,(\mathrm{l}) \)
  • Phase labels like \((\mathrm{aq})\) for aqueous and \((\mathrm{l})\) for liquid describe the physical state of each compound.
Molecular equations help us visualize the whole reaction, but do not reveal the ionic nature of substances in solutions. This makes them useful for understanding the overall chemical change.
Balancing Chemical Equations
Balancing chemical equations ensures that the number of atoms for each element is the same on both sides of the equation, as dictated by the Law of Conservation of Mass. It involves adjusting the coefficients, or numbers in front of each substance's formula.
  • The steps involve counting atoms for each element in the reactants and products.
  • You then adjust coefficients so that for each element, the number of atoms in the reactants matches that in the products.
For instance, when barium hydroxide reacts with hydrochloric acid:
\(2 \mathrm{HCl}\,(\mathrm{aq}) + \mathrm{Ba(OH)}_2\,(\mathrm{aq}) \rightarrow \mathrm{BaCl}_2\,(\mathrm{aq}) + 2\mathrm{H}_2\mathrm{O}\,(\mathrm{l}) \)
This balancing ensures that the number of hydrogen, chlorine, barium, and oxygen atoms are equal on both sides.
Aqueous Solutions
In chemistry, an aqueous solution is a solution in which the solvent is water. Substances that dissolve in water, such as salt or sugar, are typically expressed with an \((\mathrm{aq})\) phase label. In these solutions, some compounds dissociate into ions, and this factor plays a crucial role in many reactions.
  • Aqueous solutions allow ions such as \(\mathrm{Na}^+, \mathrm{Cl}^-, \mathrm{OH}^-, \mathrm{H}^+\), etc., to move freely, enabling reactions like acid-base interactions.
  • This free-moving ion characteristic is essential in conducting electricity, which is why saltwater is better at conducting electricity than pure water.
Understanding the nature of aqueous solutions helps in writing net ionic equations, as it allows for the identification of ions that actively participate in the reaction.
Acid-Base Reactions
Acid-base reactions are a type of chemical reaction that occurs between an acid and a base. They typically result in the formation of water and a salt. These reactions are essential in chemical studies and everyday processes.
  • In an acid-base reaction such as \(\mathrm{NaOH} + \mathrm{HNO}_3\), the \(\mathrm{OH}^-\) from the base (sodium hydroxide) combines with \(\mathrm{H}^+\) from the acid (nitric acid) to form water.
  • Net ionic equations simplify the reaction by focusing only on the ions that form the non-ionized product (water in this example): \(\mathrm{OH}^-\,(\mathrm{aq}) + \mathrm{H}^+\,(\mathrm{aq}) \rightarrow \mathrm{H}_2\mathrm{O}\,(\mathrm{l})\).
Recognizing common acid-base reactions and their products can help you predict reaction outcomes, vital for solving chemistry problems.

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Most popular questions from this chapter

Decide whether a reaction occurs for each of the following. If it does not, write \(N R\) after the arrow. If it does, write the balanced molecular equation; then write the net ionic equation. a. \(\mathrm{LiOH}+\mathrm{HCN} \longrightarrow\) b. \(\mathrm{Li}_{2} \mathrm{CO}_{3}+\mathrm{HNO}_{3} \longrightarrow\) c. \(\mathrm{LiCl}+\mathrm{AgNO}_{3} \longrightarrow\) d. \(\mathrm{LiCl}+\mathrm{MgSO}_{4} \longrightarrow\)

Decide whether a reaction occurs for each of the following. If it does not, write \(N R\) after the arrow. If it does, write the balanced molecular equation; then write the net ionic equation. a. \(\mathrm{Al}(\mathrm{OH})_{3}+\mathrm{HNO}_{3} \longrightarrow\) b. \(\mathrm{FeS}+\mathrm{HClO}_{4} \longrightarrow\) c. \(\mathrm{CaCl}_{2}+\mathrm{NaNO}_{3} \longrightarrow\) d. \(\mathrm{MgSO}_{4}+\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2} \longrightarrow\)

A sample of \(\mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}\) was heated to \(100^{\circ} \mathrm{C}\), where it lost water and gave another hydrate of copper(II) ion that contained 29.76\% Cu. An \(85.42-\mathrm{mg}\) sample of this new hydrate gave \(93.33 \mathrm{mg}\) of barium sulfate precipitate when treated with a barium nitrate solution. What is the formula of the new hydrate?

A 25.0-mL sample of sodium sulfate solution was analyzed by adding an excess of barium chloride solution to produce barium sulfate crystals, which were filtered from the solution. $$ \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{BaCl}_{2}(a q) \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{BaSO}_{4}(s) $$ If \(5.719 \mathrm{~g}\) of barium sulfate was obtained, what was the molarity of the original \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) solution?

Insulin is a hormone that controls the use of glucose in the body. How many moles of insulin are required to make up \(28 \mathrm{~mL}\) of \(0.0048 \mathrm{M}\) insulin solution?
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