The solubility of AgCl(s) in water at 25^∘ C is 1.33 ×10^-5 mol / L and its ΔH^∘ of solution is

The solubility of AgCl(s) in water at 25^∘ C is 1.33 ×10^-5...

Key Concepts

Solubility Equilibria

This concept refers to the equilibrium established between a solid phase and its constituent ions in a saturated solution. It typically involves the solubility product constant (Ksp), which quantifies the extent to which a compound dissolves in water. Understanding solubility equilibria is crucial to predicting how much of a compound can dissolve under various conditions.

Enthalpy of Solution

The enthalpy of solution represents the heat change when a substance dissolves in a solvent. It can be either endothermic or exothermic. In endothermic dissolution, increasing the temperature generally increases solubility because additional heat favors the dissolution process, while in exothermic processes, higher temperatures might reduce solubility.

Temperature Dependence of Equilibrium

This concept involves the way temperature changes affect chemical equilibria. According to Le Chatelier's principle, if a process is endothermic, increasing the temperature shifts the equilibrium toward the products, thus increasing solubility. Conversely, for exothermic processes, higher temperatures can shift the equilibrium toward the reactants, decreasing solubility.

van't Hoff Equation

The van't Hoff equation is a mathematical expression that relates the change in the equilibrium constant of a chemical reaction to the change in temperature and the enthalpy change of the reaction. It provides a framework for quantifying how solubility (through Ksp as an equilibrium constant) varies with temperature, making it a key tool in understanding solubility trends.

Transcript

00:01 In this question we've been given two states, initial condition with a temperature with its own temperature of 298 .15k and a final condition with the temperature of 323 .15k.

00:18 And we want to determine the solubility at this temperature.

00:24 So for us to answer this question, remember we have two states and what we know is, is when we have two states, this when we are looking in terms of solubility, we're going to have a solubility product because remember the solubility product is equal to the product of the concentrations.

00:44 In this case this is ag plus and co minus.

00:50 So what we want to determine here is the solubility.

00:55 So remember since we have two states, this is going to have its own k and this is also going to have its own k.

01:02 So once we have this information, if we look at this data that we have, we can therefore tell that the formula that we can use to link these dates is, for example, lin k2 over k1 is equal to negative enthalpy change, standard enthalpy change over r multiplied by 1 over t2 minus 1 over t1.

01:32 So for us to answer this question, we first of all left to determine k1, our k1, which is equal to concentration of hg plus and cl minus.

01:46 And this is evaluated under initial conditions that we called one.

01:52 And for us to do this, we need to determine the equilibrium.

01:56 Remember, this is an equilibrium constant.

01:57 So these concentrations are concentrations at equilibrium.

02:00 We are therefore going to have an ice chart where we have the initial, the change and the concentration equilibrium.

02:17 So if we look at this, we don't consider the solids, we only consider the ions that give rise to a concentration.

02:27 So if this is initial, this is at zero because we are just initially dissolving it.

02:32 So we won't be having any of these in solution.

02:35 So initial, this is going to be 0 and this is also going to be 0.

02:40 So if this changes by a factor of x, this is also going to change by a factor of x because we have one more of each of this.

02:48 So at equilibrium, the concentration of ag plus ions is going to be equal to x and that of the chloride ions is going to be equal to x...

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