How Do You Calculate the Solubility of AgCl in an HCl Solution with pH 2.30?

In summary, the conversation discusses calculating the solubility of AgCl in an HCl solution with a pH of 2.30 using the Ksp of silver chloride. It is determined that the concentration of HCl can be used to find the Ag concentration, which is then converted to molar solubility and converted to grams per liter. The person expresses gratitude for any help or intentions to help.
  • #1
physicsperson
20
1
[SOLVED] equilibirum and solubility product

I need some help with this question, if there are any chemistry whizzes around id really appreciate it:

Calculate the solubility of AgCl (in grams of AgCl/ L of solution) in an HCl solution having pH of 2.30. Ksp of silver chloride = 1.7 x 10^-10.
 
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  • #2
so far all i can tell is that from the ph u get the concentration of HCL, then...im lost
 
  • #3
ok i got some help, apparently u use the cl concentration from hcl and the ksp and solve for Ag conc. which should be same as the molar solubility for in mol/l of AgCl then just convert. thanks for any help or good intentions.
 

Related to How Do You Calculate the Solubility of AgCl in an HCl Solution with pH 2.30?

1. What is the definition of equilibrium?

Equilibrium is a state in which the rate of a forward reaction is equal to the rate of its reverse reaction, resulting in a constant concentration of reactants and products.

2. How is equilibrium affected by changes in concentration, pressure, and temperature?

According to Le Chatelier's principle, when the concentration of a reactant or product is increased, the equilibrium will shift in the direction that consumes or produces that substance. Changes in pressure and temperature also affect the equilibrium position, with an increase in pressure favoring the side with fewer moles of gas and an increase in temperature favoring the endothermic reaction.

3. What is the solubility product constant (Ksp)?

The solubility product constant is a measure of the maximum concentration of a solute that can dissolve in a solvent at equilibrium. It is equal to the product of the concentrations of the dissociated ions raised to the power of their coefficients in the equilibrium expression.

4. How is the solubility product constant used to determine the solubility of a substance?

The solubility product constant can be used in conjunction with the concentrations of the ions at equilibrium to calculate the solubility of a substance. By rearranging the equilibrium expression and solving for the unknown concentration, the solubility of the substance can be determined.

5. What factors can affect the solubility product constant?

The solubility product constant is affected by changes in temperature, pressure, and the presence of other substances that may interfere with the dissociation of the solute. Additionally, changes in pH can also affect the solubility of certain compounds by altering the concentrations of the ions involved.

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