Calculate the solubility of mgoh2 in a buffer solution

Reference no: EM13228018

I know it's a lot but you don't need to answer all the questions if you don't want to spend the time-

thanks for your time and any help :)

1. A saturated solution of unknown metal hydroxide M(OH)2 has a measured pH of 8.31. Determine the value of Ksp for the compound.

2. How much potassium oxalate can be added to 97 mL of 0.35 M [Cu(NH3)4]Cl2 before a precipitate of CuC2O4 begins to form? Ksp(CuC2O4)=2.9x10-8 and Kf(Cu(NH3)42+)=1.1x1012

3. A solution contains 0.5 M Pb(NO3)2 and 0.24 M AgNO3. As solid KI is slowly added to the solution, one of the metal iodides begins to precipitate. What is the concentration of Ag+(aq) remaining in solution when the second metal iodide begins to precipitate from the solution? Ksp1(AgI)=1.5E-16 and Ksp2(PbI2)=1.4E-8

4. The acid ionization constant of Fe(H2O)62+(aq) is 3E-6. Compute the pH of a 0.2 M aqueous solution of Fe(NO3)2.

5. Compute the solubility of Mg(OH)2 in a buffer solution at pH=10.31. The solubility product of magnesium hydroxide is 1.2E-11

6. How many mg of CuNO3 can be dissolved in 179.0 mL of 0.018 M RbBr before a precipitate forms? Ksp(CuBr)=4.2x10-8

7. How many mg of Hg2Br2(s) can be dissolved in 1330.0 mL of water? Ksp(Hg2Br2)=1.3E-21

8. Determine the solubility of aluminum hydroxide, Al(OH)3, in a buffer solution at a pH of 7. Ksp = 3.7E-15

9. Ksp for BaSO4 is 1.07E-10. What is the molar solubility of BaSO4?

10. Ksp for AgCl is 1.77E-10. What is the molar solubility of AgCl in a solution of 0.43 M NaCl?

Reference no: EM13228018

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