1.0dm3 of distilled water was used to wash 2.0g of a precipitate of Agcl. If the solubility product of Agcl is 2.0x10^-10mol^2dm^-6 what quantity of silver was lost in process?
To find the quantity of silver lost in the process, we need to calculate the amount of silver chloride (AgCl) that dissolved in the water.
First, we need to calculate the concentration of AgCl in the water using the solubility product constant (Ksp) for AgCl.
Ksp = [Ag+][Cl-]
Since the solubility product of AgCl is given as 2.0x10^-10 mol^2dm^-6, this means that the concentration of Ag+ and Cl- ions in the solution is equal to the square root of the solubility product constant.
[Ag+] = [Cl-] = √(2.0x10^-10 mol^2dm^-6)
Next, we need to calculate the volume of the water used to wash the precipitate. Given that 1.0 dm^3 of distilled water was used, the volume of the water is 1.0 dm^3.
Now, we can find the number of moles of AgCl that dissolved in the water by multiplying the concentration of Ag+ (or Cl-) by the volume of the water.
Number of moles of AgCl = [Ag+] x volume of water
Now we can substitute the value of [Ag+] into the equation:
Number of moles of AgCl = √(2.0x10^-10 mol^2dm^-6) x 1.0 dm^3
Finally, to find the quantity of silver lost, we need to multiply the number of moles of AgCl by the molar mass of silver (Ag). The molar mass of Ag is 107.87 g/mol.
Quantity of silver lost = Number of moles of AgCl x molar mass of Ag
Now you can substitute the calculated values into the equation to find the quantity of silver lost.