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Chapter 3: Problem 54

Balance the following equations, and then classify each as a precipitation, acid-base, or gas-forming reaction. Show states for the products (s, \(\ell, \mathrm{g},\) aq), and then balance the completed equation. Write the net ionic equation. (a) \(\mathrm{Fe}(\mathrm{OH})_{3}(\mathrm{s})+\mathrm{HNO}_{3}(\mathrm{aq}) \rightarrow \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}+\mathrm{H}_{2} \mathrm{O}\) (b) \(\mathrm{FeCO}_{3}(\mathrm{s})+\mathrm{HNO}_{3}(\mathrm{aq}) \rightarrow \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\)

Short Answer

Expert verified
(a) is an acid-base reaction; (b) is a gas-forming reaction.

Step by step solution

01

Determine States for Products

Identify the states of the products based on their chemical nature. - For (a), Fe(NO鈧)鈧 is aqueous (aq) because it is a soluble salt, and H鈧侽 is liquid (鈩). - For (b), Fe(NO鈧)鈧 is aqueous (aq), CO鈧 is a gas (g), and H鈧侽 is liquid (鈩).
02

Balance the Equations

Balance each equation considering the conservation of mass. - For (a), Fe(OH)鈧(s) + 3HNO鈧(aq) 鈫 Fe(NO鈧)鈧(aq) + 3H鈧侽(鈩) - For (b), FeCO鈧(s) + 2HNO鈧(aq) 鈫 Fe(NO鈧)鈧(aq) + CO鈧(g) + H鈧侽(鈩)
03

Classify the Reaction

Classify each reaction based on the products formed. - (a) is an acid-base reaction: Fe(OH)鈧 reacts with HNO鈧 to form Fe(NO鈧)鈧 and water. - (b) is a gas-forming reaction: FeCO鈧 reacts with HNO鈧 to form CO鈧 gas.
04

Write the Full Ionic Equation

Convert balanced molecular equations to full ionic equations by dissociating all aqueous compounds into their respective ions. - (a) Fe(OH)鈧(s) + 3H鈦(aq) + 3NO鈧冣伝(aq) 鈫 Fe鲁鈦(aq) + 3NO鈧冣伝(aq) + 3H鈧侽(鈩) - (b) FeCO鈧(s) + 2H鈦(aq) + 2NO鈧冣伝(aq) 鈫 Fe虏鈦(aq) + 2NO鈧冣伝(aq) + CO鈧(g) + H鈧侽(鈩)
05

Write the Net Ionic Equation

Simplify by canceling out spectator ions to find the net ionic equation. Spectator ions do not participate in the reaction itself. - (a) Fe(OH)鈧(s) + 3H鈦(aq) 鈫 Fe鲁鈦(aq) + 3H鈧侽(鈩) - (b) FeCO鈧(s) + 2H鈦(aq) 鈫 Fe虏鈦(aq) + CO鈧(g) + H鈧侽(鈩)

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Key Concepts

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

Acid-Base Reactions
Acid-base reactions are fundamental chemical processes in which an acid reacts with a base, typically producing water and a salt. A classic example of this type of reaction is the neutralization of acids by bases.
In the reaction provided, Fe(OH)鈧, which is a base, reacts with HNO鈧, an acid. During this reaction, a salt, Fe(NO鈧)鈧, and water, H鈧侽, are formed:
  • Reactants: Fe(OH)鈧(s) + 3HNO鈧(aq)
  • Products: Fe(NO鈧)鈧(aq) + 3H鈧侽(鈩)
Here, Fe(OH)鈧, a solid, dissolves by reacting with HNO鈧, leading to the formation of Fe鲁鈦 ions in solution, water (liquid), and NO鈧冣伝 ions. This change represents a dynamic shift from solid to liquid and aqueous states, exemplifying the transformation typical in acid-base reactions.
Gas-Forming Reactions
Gas-forming reactions are another important concept to understand in the realm of chemical reactions. These involve a chemical reaction where a gas is formed as one of the products. These reactions often occur when carbonates react with acids.
In the example reaction FeCO鈧(s) + 2HNO鈧(aq) 鈫 Fe(NO鈧)鈧(aq) + CO鈧(g) + H鈧侽(鈩), we observe:
  • FeCO鈧, a carbonate compound, reacts with nitric acid, HNO鈧.
  • One of the key products is carbon dioxide gas (CO鈧), which is easily identifiable as it escapes as bubbles during the reaction.
The presence of CO鈧 signifies that a gas is forming in the reaction, classifying it as a gas-forming reaction. This type is very common when carbonates and bicarbonates come into contact with acids.
Net Ionic Equations
Net ionic equations provide a simplified way to represent reactions by only focusing on the components that undergo a chemical change. To achieve this, one must remove the spectator ions鈥攊ons that appear unchanged on both the reactant and product sides.
For example, in the given reactions:
  • The full ionic equation for reaction (a) includes spectator ions: Fe(OH)鈧(s) + 3H鈦(aq) + 3NO鈧冣伝(aq) 鈫 Fe鲁鈦(aq) + 3NO鈧冣伝(aq) + 3H鈧侽(鈩)
  • By removing the NO鈧冣伝, which remains unchanged, the net ionic equation becomes: Fe(OH)鈧(s) + 3H鈦(aq) 鈫 Fe鲁鈦(aq) + 3H鈧侽(鈩)
The simplification helps highlight the essence of the chemical change. Similarly, grasping the net ionic equation for gas-forming reactions aids in quickly identifying the participating ions and molecules, making complex reactions easier to understand.
States of Matter in Reactions
Understanding the states of matter in a reaction is essential, as it provides crucial insight into the physical changes that accompany a chemical process. These states include solid (s), liquid (鈩), gas (g), and aqueous (aq)鈥攚here aqueous refers to a substance dissolved in water.
In the given reactions:
  • The reactants Fe(OH)鈧 and FeCO鈧 are initially in solid (s) state.
  • HNO鈧 is in aqueous (aq) solution, indicating it's dissolved in water.
  • Reaction products like H鈧侽 appear as a liquid (鈩), and CO鈧 is released as a gas (g).
Recognizing these states can help predict the behavior of substances during the reaction, such as precipitation formation, gas evolution, or solid dissolution. By understanding the implications of each state, students can better visualize and anticipate the outcome of the reaction.

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Most popular questions from this chapter

The lanthanide elements react with oxygen to give, generally, compounds of the type \(\mathrm{Ln}_{2} \mathrm{O}_{3}\) (where Ln stands for a lanthanide element). However, there are interesting exceptions, such as a common oxide of terbium, \(\mathrm{Tb}_{\mathrm{x}} \mathrm{O}_{y}\). Given that the compound is \(73.945 \%\) Tb, what is its formula? What is the oxidation number of terbium in this compound? Write a balanced equation for the reaction of terbium and oxygen to give this oxide.

Write an equation that describes the equilibrium that exists when the weak acid benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2} \mathrm{H}\right)\) dissolves in water. Identify each of the four species in solution as either Bronsted acids or Bronsted bases. Does the equilibrium favor the products or the reactants? (In acting as an acid, the \(-\mathrm{CO}_{2} \mathrm{H}\) group supplies \(\left.\mathrm{H}^{+} \text {to } \mathrm{form} \mathrm{H}_{3} \mathrm{O}^{+} .\right)\)

Write an equation that describes the equilibrium that exists when nitric acid dissolves in water. Identify each of the four species in solution as either Bronsted acids or Bronsted bases. Does the equilibrium favor the products or the reactants?

Complete and balance the equations below, and classify them as precipitation, acid-base, gas-forming, or oxidation-reduction reactions. Show states for the products \((\mathrm{s}, \ell, \mathrm{g}, \mathrm{aq}),\) and then balance the completed equation. (a) \(\mathrm{NiCO}_{3}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow\) (b) \(\mathrm{Co}(\mathrm{OH})_{2}+\mathrm{HBr} \rightarrow\) (c) \(\mathrm{AgCH}_{3} \mathrm{CO}_{2}+\mathrm{NaCl} \rightarrow\) (d) \(\mathrm{NiO}+\mathrm{CO} \rightarrow\)

Balance the following equations: (a) \(\mathrm{Cr}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{Cr}_{2} \mathrm{O}_{3}(\mathrm{s})\) (b) \(\mathrm{Cu}_{2} \mathrm{S}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{Cu}(\mathrm{s})+\mathrm{SO}_{2}(\mathrm{g})\) (c) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{3}(\ell)+\mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g})\)
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