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Chapter 14: Problem 53

A very dilute solution of silver nitrate is added dropwise to a solution that contains equal concentrations of sodium chloride and potassium bromide. What salt will precipitate first?

Short Answer

Expert verified
The salt that will precipitate first is silver bromide (AgBr).

Step by step solution

01

Identify the Possible Reactions

When a solution of silver nitrate is added to a solution with sodium chloride and potassium bromide, silver nitrate provides Ag+ ions which can react with Cl- ions in sodium chloride to form silver chloride (AgCl) and with Br- ions in potassium bromide to form silver bromide (AgBr). The reactions can be written as: \[ Ag^+ + Cl^- \rightarrow AgCl \]and \[ Ag^+ + Br^- \rightarrow AgBr \]
02

Check the Solubility Product Constants

Check the \( K_{sp} \) values (Solubility product constant) for both AgCl and AgBr. The salt with the lesser \( K_{sp} \) value will precipitate first. The \( K_{sp} \) for AgCl is \( 1.8 × 10^{-10} \) whereas for AgBr it is \( 5.4 × 10^{-13} \). Since AgBr has a smaller \( K_{sp} \) value, it is less soluble in the solution and will precipitate first.
03

Understand the Reason

The reason why AgBr precipitates first is because it has a lower solubility than AgCl, as indicated by its lower \( K_{sp} \) value. Precipitation reaction takes place when the product of the concentration of the ions in the solution exceeds the \( K_{sp} \) of the substance. Since AgBr has a smaller Ksp than AgCl, the product of the concentration of Ag+ and Br- ions exceeds the \( K_{sp} \) of AgBr before it exceeds the \( K_{sp} \) of AgCl. Thus, AgBr precipitates first, leaving behind the less soluble salt.

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Most popular questions from this chapter

What changes in conditions would favor the products in the following equilibrium? $$\mathrm{PCl}_{5}(g) \rightleftarrows \mathrm{Cl}_{2}(g)+\mathrm{PCl}_{3}(g) \quad \Delta H=88 \mathrm{kJ}$$

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