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Among the solubility rules previously discussed is the statement: All chluble except $\mathrm{Hg}_{2} \mathrm{Cl}_{2}, \mathrm{AgCl}$$\mathrm{PbCl}_{2},$ and CuCl.(a) Write the expression for the equilibrium constant for the reaction represented by the equation$\mathrm{AgCl}(s) \rightleftharpoons \mathrm{Ag}^{+}(a q)+\mathrm{Cl}^{-}(a q) .$ Is $K_{c}>1,<1,$ or $\approx 1 ?$ Explain your answer.(b) Write the expression for the equilibrium constant for the reaction represented by the equation$\mathrm{Pb}^{2+}(a q)+2 \mathrm{Cl}^{-}(a q) \rightleftharpoons \mathrm{PbCl}_{2}(s) .$ Is $K_{c}>1,<1,$ or $\approx 1 ?$ Explain your answer.

A) Therefore, the value of $K_{c}$ for this reaction is less than 1B) Therefore, the value of $K_{c}$ for this reaction is greater than 1

Chemistry 102

Chapter 13

Fundamental Equilibrium Concepts

Chemical Equilibrium

Aqueous Equilibria

Rice University

University of Maryland - University College

University of Kentucky

Lectures

00:41

In chemistry, an ion is an…

10:03

In thermodynamics, a state…

04:31

Write solubility equilibri…

02:20

Among the solubility rules…

03:35

For each of the following …

03:24

Write the equilibrium cons…

01:26

03:29

Consider the following equ…

01:48

The following reaction is …

06:08

Calculate equilibrium cons…

05:18

Using the value of $K_{s p…

01:06

What is the equilibrium co…

02:51

Write $K_{\text {sp }}$ ex…

18:14

02:09

For which of the following…

01:47

Use the appropriate values…

01:38

09:41

Write balanced equations a…

03:36

The chemistry of silver(I)…

a. Using the $K_{\mathrm{s…

05:37

The equilibrium constant f…

20:29

So for this question, we've got to insoluble souls and we want to think about the equilibrium of these salts with the ions that are capable of dissolving in the solution. So we make solutions of these individual salts, these insoluble salt. Um, there will be a small amount of their ions that do make it under solution. We can describe the relationship between the number of ions that will actually dissolve when they reach an equilibrium between being dissolved in the solid state in the bottom of the container, using our equilibrium, uh, constant and equilibrium expressions. So each of these we can write an equilibrium constant, and we know that the equilibrium constant is only going to include a curious species and gases. So in both of these cases, because this insoluble saw itself as a solid, we're going to ignore it within the context of the delivery of expression. And for these, So for the for part A. We have written that silver chloride is going to be breaking up into silver ions and chloride ions because the silver chloride solid is one of our reactions is it is the only reactive. We don't have any Equus or gas phase reactive, So our equilibrium expression is not going to have any re reactions. So for that reason, the equilibrium equation, it's simply going to be silver kind. And I owns the concentration of silver katana hands multiplied by the concentration of silver or chloride ion in irons. So because this is an insoluble salt, it implies that the products are not heavily favored. What we can infer from that is the equilibrium constant. For this, uh, expression is going to be less than one. Conversely, if we consider the equation presented in part be, what we're looking at is an insoluble soul. But the reverse reaction said the process of taking the ions of this insoluble solved and producing a solid so the equilibrium constant for this reaction is going to be very similar. The only difference being now are insoluble. Soul is one of our products because solids again don't get included in the reaction equation. We're just going to have a place holder here representing one, and the reactions are going to go on the bottom. And the only other difference with this equation is because the coefficient in front of chloride in this equation is, too. There's going to be a two exponents tied to the chloride term within the Saudi ability equation written here. And because this sold is insoluble, it means that we have these ions and solution the formation a high enough concentration. We have these irons and solution. The formation of the salt is going to be heavily favorable. And what that means is that the equilibrium equation written in this direction for this equation is going to be greater than one.

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