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-?

Verified step by step guidance

Identify the possible reactions that could occur with each reagent: AgNO_3, Pb(NO_3)_2, and BaCl_2.

Consider the solubility rules for common ionic compounds to determine which anions form precipitates with the given cations.

For AgNO_3, determine which anions form insoluble silver salts, such as AgBr.

For Pb(NO_3)_2, determine which anions form insoluble lead salts, such as PbCO_3.

For BaCl_2, determine which anions form insoluble barium salts, such as BaCO_3.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

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 ionic compounds react in solution to form an insoluble solid, known as a precipitate. In this case, the addition of AgNO3, Pb(NO3)2, and BaCl2 to the unknown ionic compound results in precipitates, indicating that the anion in the unknown compound must form insoluble salts with these cations.

Solubility Rules

Solubility rules are guidelines that help predict whether a compound will dissolve in water. For example, silver (Ag+), lead (Pb2+), and barium (Ba2+) salts have specific solubility characteristics; AgBr and PbBr2 are insoluble, while BaCO3 is also insoluble. Understanding these rules is essential for determining which anions can form precipitates with the given cations.

Ionic Compounds and Anions

Ionic compounds consist of cations and anions held together by ionic bonds. The identity of the anion is crucial in predicting the behavior of the compound in solution. In this scenario, the possible anions Br-, CO32-, and NO3- must be evaluated based on their ability to form precipitates with the cations present in the reagents used.

Recommended video:

Guided course

02:11

Ionic Compounds Naming

Related Practice

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.

(a) Ba(OH)₂(aq) + FeCl₃(aq) →

(b) ZnCl₂(aq) + Cs₂CO₃(aq) →

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) Na₂S(aq) + CoSO₄(aq) →

Textbook Question

You know that an unlabeled bottle contains an aqueous solutionof one of the following: AgNO3, CaCl2, or Al21SO423. Afriend suggests that you test a portion of the solution withBa1NO322 and then with NaCl solutions. According to yourfriend's logic, which of these chemical reactions could occur,thus helping you identify the solution in the bottle?(a) Barium sulfate could precipitate. (b) Silver chloridecould precipitate. (c) Silver sulfate could precipitate.(d) More than one, but not all, of the reactions described inanswers a–c could occur. (e) All three reactions described inanswers a–c could occur.

views

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?

views

Textbook Question

State whether each of the following statements is true or false. Justify your answer in each case. (a) Sulfuric acid is a monoprotic acid.