In qualitative analysis, Ca2+ and Ba2+ are seperated from Na+,...

Question

In qualitative analysis, Ca2+ and Ba2+ are seperated from Na+, K+, Mg2+ by adding aqueous (NH4)2CO3 to a solution that also contains aqueous NH3 (Figure 17.18). Assume that the concentrations after mixing are 0.080 M (NH4)2CO3 and 0.16 M NH3. (a) List all the Bronsted-Lowry acids and bases present initially, and identify the principal reaction.

Accepted Answer

Step 1: Identify the Bronsted-Lowry acids and bases in the solution. Bronsted-Lowry acids are substances that can donate a proton (H+), and Bronsted-Lowry bases are substances that can accept a proton. In this case, the acids are Ca2+, Ba2+, and (NH4)2CO3, and the bases are Na+, K+, Mg2+, and NH3.. Step 2: Identify the principal reaction. The principal reaction is the reaction that will occur to the greatest extent. In this case, the principal reaction is the reaction between the (NH4)2CO3 and the NH3. This is because (NH4)2CO3 is a weak acid and NH3 is a weak base, and the reaction between a weak acid and a weak base will proceed to a greater extent than the reactions between the other ions present.. Step 3: Write out the principal reaction. The reaction between (NH4)2CO3 and NH3 can be written as follows: (NH4)2CO3 + NH3 -> 2NH4+ + CO3- + NH3. In this reaction, (NH4)2CO3 donates a proton to NH3, forming NH4+ and CO3-.. Step 4: Note that the reaction will shift to the right due to Le Chatelier's principle. This is because the concentration of NH3 is greater than the concentration of (NH4)2CO3, so the reaction will shift to the right to reach equilibrium.. Step 5: Finally, remember that the Ca2+ and Ba2+ ions will not react with the (NH4)2CO3 or the NH3 to any significant extent. This is because these ions are spectator ions in this reaction, meaning they do not participate in the reaction.

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Key Concepts

Brønsted-Lowry Theory

Complex Ion Formation

Precipitation Reactions