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Chapter 3: Problem 64

Complete and balance the equations below, and classify them as precipitation, acid-base, gasforming, or oxidation-reduction reactions. Show states for reactants and products \((s, \ell, g, a q).\) (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) \(\mathrm{NiO}+\mathrm{CO} \rightarrow\)

Short Answer

Expert verified
(a) Gas-forming (NiCO鈧� + H鈧係O鈧� 鉄� NiSO鈧� + CO鈧� + H鈧侽); (b) Acid-base (Co(OH)鈧� + 2HBr 鉄� CoBr鈧� + 2H鈧侽); (c) Precipitation (AgCH鈧僀O鈧� + NaCl 鉄� AgCl + NaCH鈧僀O鈧�); (d) Redox (NiO + CO 鉄� Ni + CO鈧�).

Step by step solution

01

Balance Reaction (a)

The reaction is between nickel carbonate (NiCO鈧�) and sulfuric acid (H鈧係O鈧�). This is a reaction that forms nickel sulfate (NiSO鈧�), carbon dioxide (CO鈧�), and water (H鈧侽). The balanced equation is:\[\text{NiCO}_{3}(s) + \text{H}_{2}\text{SO}_{4}(aq) \rightarrow \text{NiSO}_{4}(aq) + \text{CO}_{2}(g) + \text{H}_{2}\text{O}(\ell)\] This is a gas-forming reaction due to the production of CO鈧� gas.
02

Balance Reaction (b)

The reaction is between cobalt(II) hydroxide (Co(OH)鈧�) and hydrobromic acid (HBr). This forms cobalt(II) bromide (CoBr鈧�) and water (H鈧侽). The balanced equation is:\[\text{Co(OH)}_{2}(s) + 2 \text{HBr}(aq) \rightarrow \text{CoBr}_{2}(aq) + 2 \text{H}_{2}\text{O}(\ell)\]This is an acid-base reaction.
03

Balance Reaction (c)

The reaction is between silver acetate (AgCH鈧僀O鈧�) and sodium chloride (NaCl). This forms silver chloride (AgCl) as a precipitate and sodium acetate (NaCH鈧僀O鈧�). The balanced equation is:\[\text{AgCH}_{3}\text{CO}_{2}(aq) + \text{NaCl}(aq) \rightarrow \text{AgCl}(s) + \text{NaCH}_{3}\text{CO}_{2}(aq)\]This is a precipitation reaction due to the formation of the solid AgCl.
04

Balance Reaction (d)

The reaction between nickel(II) oxide (NiO) and carbon monoxide (CO) is a redox reaction, forming nickel (Ni) and carbon dioxide (CO鈧�). The balanced equation is:\[\text{NiO}(s) + \text{CO}(g) \rightarrow \text{Ni}(s) + \text{CO}_{2}(g)\]This is an oxidation-reduction reaction.

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Key Concepts

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

Balancing Equations
When working with chemical reactions, balancing equations is essential. This ensures that the same number of each type of atom appears on both sides of the equation, following the law of conservation of mass. To balance a chemical equation, you need to adjust the coefficients of the reactants and products until the number of each atom is the same on both sides.
  • Start by listing the number of atoms for each element present in the reactants and products.
  • Adjust coefficients to balance each element in turn, often starting with the most complex molecule or the element that appears in the fewest substances.
  • Check and recheck until both sides of the equation have equal numbers of each type of atom.
Balancing can sometimes be challenging, especially if multiple elements are involved. Practice helps to develop a systematic approach.
Oxidation-Reduction Reactions
Oxidation-reduction reactions, also known as redox reactions, involve the transfer of electrons between substances. These reactions are characterized by changes in the oxidation states of the substances involved. One reactant will lose electrons (oxidation), while the other gains electrons (reduction).
  • To identify a redox reaction, look for the change in oxidation numbers of atoms; the atom that increases its oxidation number is oxidized, while the one that decreases its number is reduced.
  • A common method to balance redox reactions is the half-reaction method, where you separately balance the oxidation and reduction half-reactions before combining them.
Redox reactions are crucial in both biological processes and industrial applications, from energy production to waste treatment.
Acid-Base Reactions
Acid-base reactions involve the transfer of protons (H鈦� ions) between reactants. Typically, an acid donates a proton to a base. The result is often the formation of water and a salt. These reactions can be identified by the reactants: acids often contain hydrogen ions, like HCl, while bases contain hydroxide ions, like NaOH.
  • In aqueous solutions, the acid-base reaction can often be simplified to the formation of water: H鈦�(aq) + OH鈦�(aq) 鈫� H鈧侽(鈩�).
  • To balance an acid-base reaction, ensure that there is a stoichiometric balance of H鈦� and OH鈦� ions.
Understanding these reactions is essential for studying pH, buffers, and the chemical behavior of acids and bases.
Precipitation Reactions
Precipitation reactions occur when two aqueous solutions combine to form an insoluble solid known as a precipitate. These reactions are governed by solubility rules that describe whether an ionic compound will dissolve in water or form a solid.
  • To predict precipitation reactions, use a solubility chart to determine which products are insoluble.
  • The formation of the precipitate is the driving force of the reaction and is usually visible as a solid appearing in the solution.
These reactions are important in various industries and environmental processes, such as water treatment and the removal of heavy metals.

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Most popular questions from this chapter

Write an equation from the following description: reactants are gaseous \(\mathrm{NH}_{3}\) and \(\mathrm{O}_{2},\) products are gaseous \(\mathrm{NO}_{2}\) and liquid \(\mathrm{H}_{2} \mathrm{O},\) and the stoichiometric coefficients are \(4,7,4,\) and \(6,\) respectively.

Balance each of the following equations, and classify them as precipitation, acid-base, gas-forming, or oxidation-reduction reactions. Show states for reactants and products \((s, \ell, g, a q).\) (a) \(\mathrm{CuCl}_{2}+\mathrm{H}_{2} \mathrm{S} \rightarrow \mathrm{CuS}+\mathrm{HCl}\) (b) \(\mathrm{H}_{3} \mathrm{PO}_{4}+\mathrm{KOH} \rightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{K}_{3} \mathrm{PO}_{4}\) (c) \(\mathrm{Ca}+\mathrm{HBr} \rightarrow \mathrm{H}_{2}+\mathrm{CaBr}_{2}\) (d) \(\mathrm{MgCl}_{2}+\mathrm{NaOH} \rightarrow \mathrm{Mg}(\mathrm{OH})_{2}+\mathrm{NaCl}\)

Determine the oxidation number of each element in the following ions or compounds. (a) \(\mathrm{PF}_{6}\) (b) \(\mathrm{H}_{2} \mathrm{AsO}_{4}^{-}\) (c) \(\mathrm{UO}^{2+}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (e) \(\mathrm{POCl}_{3}\) (f) \(\mathrm{XeO}_{4}^{2-}\)

Balance the following equations, and then classify each as a precipitation, acid-base, or gas-forming reaction. (a) \(\mathrm{Ba}(\mathrm{OH})_{2}(\mathrm{aq})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{BaCl}_{2 (\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)\) (b) \(\mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{CoCO}_{3}(\mathrm{s}) \rightarrow \mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g})\) (c) \(\mathrm{Na}_{3} \mathrm{PO}_{4}(\mathrm{aq})+\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) \rightarrow \mathrm{Cu}_{3}\left(\mathrm{PO}_{4}\right)_{2}(\mathrm{s})+\mathrm{NaNO}_{3}(\mathrm{aq})\)

Balance each of the following equations, and then write the net ionic equation. Show states for all reactants and products (s, \(\ell, \mathrm{g},\) aq). (a) the reaction of sodium hydroxide and iron(II) chloride to give iron(II) hydroxide and sodium chloride (b) the reaction of barium chloride with sodium carbonate to give barium carbonate and sodium chloride (c) the reaction of ammonia with phosphoric acid
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