Textbook Question
Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. c. Fe(NO3)2(ππ)+KOH(ππ)βΆ
Ch.4 - Reactions in Aqueous Solution
Chapter 4, Problem 29
You know that an unlabeled bottle contains an aqueous solution of one of the following: AgNO3,CaCl2, or Al2(SO4)3. You take a portion of the solution and add an aqueous solution of Ba(NO3)2 to it, and observe that a white solid precipitates Then you take another portion of the unlabeled solution and add an aqueous solution of NaCl to it; nothing appears to happen. What is the most likely identity of the solution in the unlabeled bottle: silver nitrate, calcium chloride, aluminum sulfate?
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Identify the possible reactions with Ba(NO_3)_2: AgNO_3, CaCl_2, and Al_2(SO_4)_3 can all potentially react with Ba(NO_3)_2 to form a precipitate. Consider the solubility rules to determine which combinations form insoluble products.
Write the balanced chemical equations for each possible reaction: (1) AgNO_3 + Ba(NO_3)_2, (2) CaCl_2 + Ba(NO_3)_2, (3) Al_2(SO_4)_3 + Ba(NO_3)_2. Determine which reaction forms a white precipitate.
Consider the reaction with NaCl: AgNO_3 would react with NaCl to form AgCl, a white precipitate. Since no precipitate forms, AgNO_3 is unlikely to be in the bottle.
Evaluate the remaining options: Since no reaction occurs with NaCl, eliminate AgNO_3. Consider the reactions of CaCl_2 and Al_2(SO_4)_3 with Ba(NO_3)_2 and NaCl.
Conclude the identity: Based on the reactions and observations, determine which compound is most consistent with the formation of a white precipitate with Ba(NO_3)_2 and no reaction with NaCl.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Precipitation Reactions
Precipitation reactions occur when two soluble salts react in solution to form an insoluble solid, known as a precipitate. In this scenario, the addition of Ba(NO3)2 leads to the formation of a white precipitate, indicating that a reaction has occurred. The identity of the precipitate can help identify the original solution based on the solubility rules of the involved compounds.
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Solubility Rules
Solubility rules are guidelines that predict whether a compound will dissolve in water. For example, barium sulfate (BaSO4) is insoluble, while calcium chloride (CaCl2) and sodium chloride (NaCl) are soluble. Understanding these rules is crucial for determining which compounds will precipitate when mixed, aiding in the identification of the unknown solution.
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Ionic Compounds and Their Reactions
Ionic compounds, such as AgNO3, CaCl2, and Al2(SO4)3, dissociate into their constituent ions in aqueous solution. The behavior of these ions during reactions, such as forming precipitates or remaining in solution, is essential for identifying the unknown solution. The lack of reaction with NaCl suggests that the solution does not contain ions that would form an insoluble compound with chloride ions.
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Related Practice
Textbook Question
Separate samples of a solution of an unknown ionic compound are treated with dilute AgNO3, Pb1NO322, and BaCl2. Precipitates form in all three cases. Which of the following could be the anion of the unknown salt: Br-, CO32-, NO3-?
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Textbook Question
Three solutions are mixed together to form a single solution; in the final solution, there are 0.2 mol Pb1CH3COO)2, 0.1 mol Na2S, and 0.1 mol CaCl2 present. What solid(s) will precipitate?
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Textbook Question
Which of the following solutions is the most acidic? a. 0.2 M LiOH b. 0.2 M HI c. 1.0 M methanol (CH3OH)
Textbook Question
Which of the following solutions is the most basic? a. 0.6π NH3 b. 0.150 M KOH c. 0.100πBa(OH)2