# CHEM 152

posted by .

At 50oC, the solubility of silver chloride, AgCl, is 5.2 x 10-4 g/100 mL. Calculate the Ksp at this temperature.

• CHEM 152 -

Convert 5.2 x 10^-4 g/100 mL to moles/L.

Then Ksp = (Ag^+)(Cl^-)

## Similar Questions

1. ### Chemistry

What is the solubility of silver chloride in water at 25C?
2. ### Chemistry

So the Ksp for silver chloride is 1.8*10^-10, how could I find the concentration of silver ions in this saturated solution. Then how I find the total ion concentration?
3. ### chemistry

Calculate the solubility of silver chloride in a 0.1 mol/L solution of sodium chloride at 25°C.?
4. ### chemistry

Calculatet the solubility of silver chloride in a 0.10 mol/L solution of sodium chloride at 25 degrees celsius.At SATP, Ksp AgCl(s) = 1.8 x 10^-10
5. ### chemistry

Calculate the solubility of silver chloride in a 0.010 mol/L solution of sodium chloride at 25 degrees Celsius. At SATP, Ksp AgCl(s) = 1.8 x 10^-10

Calculate the molar solubility of silver chloride (AgCl) in: a-deionized water and b-.20M NaCl solution Given Ksp=1.6*10^-10
7. ### chem

a) Co(H2O)6^2 + 4 Cl^‐1 (aq) ⇄ CoCl4^‐2 (aq) + 6 H2O (l) Rewrite the net ionic equation above including the energy term where appropriate. The Delta H for this reaction is +50 kJ/mol. b) Silver chloride (AgCl) is …
8. ### Chemistry

Calculate solubility of AgCl (in g/L) in a 6.5*10^-3 M silver Nitrate solution ksp= 1.8 * 10^-10 (AgCl molecular mass is 143.3g) any idea on how to do this this is what i tried> AgCl--> Ag + Cl I 6.5*10^-3 0 C same x E same x …
9. ### Chemistry

Calculate solubility of AgCl (in g/L) in a 6.5*10^-3 M silver Nitrate solution ksp= 1.8 * 10^-10 (AgCl molecular mass is 143.3g) any idea on how to do this this is what i tried> AgCl--> Ag + Cl I 6.5*10^-3 0 C same x E same x …
10. ### chemistry

In quality control of raw materials for pharmaceutical production often used foul reactions to prove that raw materials in salt form containing the appropriate salt. Hydrochloride (eg. Amitriptyline hydrochloride) can be detected for …

More Similar Questions