4a. Look up the Ksp for Mn(OH)2 and provide the reference: 200x10-13 Reference: wirdchemist com b....
It's part k and calculation 0.4067×0.4067=0.165 also I dont understand questions 1-4 k. Calculate the Ksp of KHP in 0.5 M KCl solution. Is there a difference between the Ksp in 0.5 M KCl and the Ksp in purified water (calculation d)? [K] = [HP] = - Calculation Ksp = D=0.165 4a. Look up the Ksp for Mn(OH)2 and provide the reference: 1.6 X10 reference: /.6 X10-13 Reference b. The pH of a saturated solution of Mn(OH)2 is 9.90. Calculate...
5a. Write a balanced equilibrium equation for Cas(PO4)2 going into solution. b. The CRC Hand book gives the solubility of Cas(PO4)2 at 25°C as 0.0012 g/100 mL. Determine the molar solubility of Cas(PO4)2. This is the molarity of a saturated solution. c. Determine Ksp for Ca3(PO4)2.
Find the literature ksp value for Mn(OH )2 . ph of saturated solution mn(Oh )2 is 9.90 calculate oh ,mn, mnoh2 concentration and , ksp .compare calculated ksp value from the literature ksp value . are the two values close or different .
The value for Ksp for manganese (II) hydroxide (Mn(OH)2) is 1.6x10^-13. Calculate the molar solubility of Mn(OH)2 in a solution containing 0.020M NaOH
RUESLIon (points) For manganese(II) hydroxide, Mn(OH)2, Ksp = 1.6 x 10-13. Calculate the molar solubility of Mn(OH)2 in a solution that contains 0.158 M NaOH. (Hint: this involves calculating the effect of a common ion on solubility.)