The formation constant of CoY2− is 1016.45. Calculate the concentration of free Co2+ in a solution of 0.10 M CoY2− buffered at pH 9.00.  = 0.041 at pH 9.00. x 10^ M Co2+

Which compound CANNOT be used as a primary standard in the titration of an acid or a base?

A 100.0-mL sample of a solution containing copper(II) (FM 63.546) is treated with excess sodium carbonate (FM 105.988 8) to precipitate 3.605 5 g of copper(II) carbonate (FM 123.55). What is the molarity of the solution?

A 25.00-mL aliquot of 0.100 M sodium acetate (pKb = 9.244) is titrated with 0.125 M HCl. Calculate the pH after 10.00 mL of 0.125 M HCl has been added.

Calculate pPb2+ when 25.00 mL of 0.150 M  is titrated with 17.00 mL of 0.150 M Pb2+. Ksp = 7.4 × 10−14 for PbCO3.

A 25.00-mL aliquot of 0.100 M KOH is titrated with 0.065 2 M HCl. Calculate the pH after 40.00 mL of 0.065 2 M HCl has been added.

Calculate pBa2+ after 35.00 mL of 0.100 M EDTA is added to 50.00 mL of 0.100 M Ba2+ in the presence of 0.100 M nitrilotriacetate. The solution is buffered at pH 10. = 1.48 × 10−4. = 0.30 at pH 10. Kf = 7.59 × 107 for BaY2−.

The Ka value for CH3CH2NO2 is 2.7 × 10−9. Calculate Kb for . Ans= x 10^

Calculate the pH of a 0.150 M maleic acid solution. pK1 = 1.92 and pK2 = 6.27 for maleic acid.

What is the molar solubility of brucite crystal, Mg(OH)2, in pure water. Ksp = 7.1 × 10−12 for brucite crystal, Mg(OH)2. Ans= x 10^