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Chapter 5: Problem 5

Predict whether a precipitation reaction will occur in the following situations. If a precipitation reaction occurs, write the balanced chemical equation for the reaction. (a) \(\mathrm{NiCl}_{2}(a q)+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{~S}(a q) \longrightarrow\) (b) \(\mathrm{AgNO}_{3}(a q)+\mathrm{CaBr}_{2}(a q) \longrightarrow\)

Short Answer

Expert verified
Both reactions produce a precipitate. (a) Nickel sulfide, NiS. (b) Silver bromide, AgBr.

Step by step solution

01

Understand the concept of precipitation reactions

A precipitation reaction occurs when two aqueous solutions combine to form an insoluble solid, known as a precipitate, that falls out of solution. By examining the solubility rules, we can predict if a precipitate will form.
02

Identify the possible products

For each reaction, perform a double displacement reaction and identify the possible products. Question (a) produces NiS and NH4Cl, while question (b) forms AgBr and Ca(NO3)2.
03

Apply solubility rules

Consult the solubility rules to determine if any of the products is insoluble in water. For (a), NiS is insoluble. For (b), AgBr is insoluble. This indicates a precipitate will form in both reactions.
04

Write balanced chemical equations

For (a), the balanced equation is \(\text{NiCl}_2(aq) + (\text{NH}_4)_2\text{S}(aq) \rightarrow \text{NiS}(s) + 2\text{NH}_4\text{Cl}(aq)\). For (b), the balanced equation is \(2\text{AgNO}_3(aq) + \text{CaBr}_2(aq) \rightarrow 2\text{AgBr}(s) + \text{Ca(NO}_3\text{)}_2(aq)\). Each balanced equation confirms the precipitate formation.

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Key Concepts

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

Understanding Solubility Rules
When dealing with chemical reactions, especially in aqueous solutions, solubility rules are essential. These rules help predict whether a compound will dissolve in water or form a precipitate. A precipitate is an insoluble solid that emerges from a liquid solution. Knowing which compounds are likely to form a precipitate helps in predicting chemical reactions. Some basic solubility rules include:
  • Most nitrates (NO鈧冣伝) and acetates (CH鈧僀OO鈦�) are soluble in water.
  • Compounds containing alkali metal ions (like Na鈦�, K鈦�) and the ammonium ion (NH鈧勨伜) are generally soluble.
  • Most chlorides (Cl鈦�), bromides (Br鈦�), and iodides (I鈦�) are soluble, except those of silver (Ag鈦�), lead (Pb虏鈦�), and mercury (Hg鈧偮测伜).
  • Sulfates (SO鈧劼测伝) are generally soluble, with exceptions including barium sulfate (BaSO鈧�), lead sulfate (PbSO鈧�), and calcium sulfate (CaSO鈧�).
Applying these rules, we can determine that in the given situations, nickel sulfide (NiS) and silver bromide (AgBr) are insoluble and will form precipitates.
Exploring Double Displacement Reactions
Double displacement reactions, also known as metathesis reactions, occur when parts of two ionic compounds are exchanged, forming two new compounds. They typically follow the pattern: AB + CD 鈫� AD + CB. This type of reaction is common in aqueous solutions and often results in the formation of a precipitate. In the reactions given:
  • For (a) [NiCl鈧�(aq) + (NH鈧�)鈧係(aq) 鈫� NiS(s) + 2NH鈧凜l(aq)], the ions swap partners, resulting in nickel sulfide, which is insoluble, and ammonium chloride, which remains dissolved in water.
  • For (b) , [2AgNO鈧�(aq) + CaBr鈧�(aq) 鈫� 2AgBr(s) + Ca(NO鈧�)鈧�(aq)], we see a similar process where silver ions and bromide ions form silver bromide, an insoluble product that precipitates, while calcium nitrate is soluble.
Predicting products in double displacement reactions often involves checking solubility rules to see if any of the products will precipitate.
Importance of Balanced Chemical Equations
Balanced chemical equations are crucial for accurately representing chemical reactions. They ensure that the law of conservation of mass is followed, which states that matter cannot be created or destroyed in a chemical reaction.To balance a chemical equation, each type of atom must have the same number on both sides of the reaction. This means adjusting coefficients as needed.For the given exercises:
  • In (a), NiCl鈧� and (NH鈧�)鈧係 react to form NiS and NH鈧凜l. The balanced chemical equation is: \[ \text{NiCl}_2(aq) + (\text{NH}_4)_2\text{S}(aq) \rightarrow \text{NiS}(s) + 2\text{NH}_4\text{Cl}(aq) \]
  • In (b), 2AgNO鈧� and CaBr鈧� form 2AgBr and Ca(NO鈧�)鈧�. This balances as: \[ 2\text{AgNO}_3(aq) + \text{CaBr}_2(aq) \rightarrow 2\text{AgBr}(s) + \text{Ca(NO}_3\text{)}_2(aq) \]
Using balanced equations not only reflects the reality of the chemical process but is also essential for quantitative analysis in chemical experiments.

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Most popular questions from this chapter

The transition metals form compounds with oxygen in which the metals have different oxidation states. Calculate the oxidation number for the transition metal in the following sets of compounds: (a) \(\mathrm{Mn}\) in \(\mathrm{MnO}_{2}, \mathrm{Mn}_{2} \mathrm{O}_{3},\) and \(\mathrm{KMnO}_{4}\) (b) \(\mathrm{Cr}\) in \(\mathrm{CrO}_{2}, \mathrm{CrO}_{3},\) and \(\mathrm{Cr}_{2} \mathrm{O}_{3}\)

Which element is oxidized and which is reduced in the following reactions? (a) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)\) (b) \(2 \mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NaCl}(s)\) (c) \(\mathrm{CuCl}_{2}(a q)+\mathrm{Zn}(s) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{Cu}(s)\) (d) \(2 \mathrm{NaCl}(a q)+\mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{NaF}(a q)+\mathrm{Cl}_{2}(g)\)

Potassium, a silvery metal, reacts with bromine, a corrosive, reddish liquid, to yield potassium bromide, a white solid. Write the balanced equation, and identify the oxidizing and reducing agents.

Which of the following substances are likely to be soluble in water? (a) \(\mathrm{ZnSO}_{4}\) (b) \(\mathrm{NiCO}_{3}\) (c) \(\mathrm{PbCl}_{2}\) (d) \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)

Write balanced equations for the following reactions: (a) Hydrochloric acid reacts with calcium carbonate to form carbon dioxide and calcium chloride and water. (b) Liquid bromine reacts with solid potassium metal to form solid potassium bromide. (c) Gaseous propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) burns in oxygen to form gaseous carbon dioxide and water vapor.
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