# Using Ksp to find the concentration

• Faka
In summary, the question is asking for the concentrations of Ag+, Cl-, and Br- after equilibrium has occurred in a solution containing 0.1100 mol AgNO3, 0.1000 moles of NaCl, and 0.1000 moles of NaBr in 500 mL. The solubility product for AgCl is 1.82*10^-10 and the solubility product for AgBr is 5.0*10^-13. The formulas for solubility products and mass balances will be needed to solve this problem, and the limiting reagent will determine which salt will precipitate first and in what amount.
Faka

## Homework Statement

0.1100 mol AgNO3 translated into 500 mL of a solution containing 0.1000 moles of NaCl and NaBr 0.1000 moles. What are the concentrations of Ag+, Cl-, Br-, after equilibrium has occurred?

Solubility product for AgCl: Ksp(AgCl) = 1,82*10^-10
Solubility product for AgBr: Ksp(AgBr) = 5,0*10^-13

## The Attempt at a Solution

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Is there anybody, who can help me with this. Which equations do I have to use?
I am lost with this assignment.

You will need formulas for both solubility products and mass balances.

What will precipitate first? How much of that salt can precipitate? (hint: limiting reagent).

I have made the task. Delete the topic, thanks ! :-)

## What is Ksp and how is it used to find concentration?

Ksp stands for solubility product constant and it is a measure of the equilibrium solubility of a compound in a solution. It is used to find the concentration of a dissolved compound by relating the concentration of ions in a saturated solution to the Ksp value.

## How do you calculate the Ksp value?

The Ksp value can be calculated by multiplying the concentrations of the ions in a saturated solution raised to the power of their coefficients in the balanced chemical equation. For example, for the compound AB2, the Ksp would be [A]1[B]2.

## What is the relationship between Ksp and solubility?

Ksp and solubility are directly related. The higher the Ksp value, the more soluble the compound is in a solution. Conversely, a lower Ksp value indicates a less soluble compound.

## Can Ksp be used to predict the formation of a precipitate?

Yes, Ksp can be used to predict the formation of a precipitate. If the product of the concentrations of ions in a solution is greater than the Ksp value, a precipitate will form. If the product is less than the Ksp value, no precipitate will form.

## What factors can affect the accuracy of using Ksp to find concentration?

The accuracy of using Ksp to find concentration can be affected by factors such as temperature, pH, and the presence of other ions in the solution. These factors can alter the solubility of the compound and therefore affect the Ksp value.

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