A. Calculate the pH of a solution formed by combining 0.125 mLof 0.55 M HI with 0.400 mL of 0.14 M KOH at25°C.
B. Calculate the pH of a solution formed by combining 0.125 mL of0.55 M HI with 0.400 mL of 0.18 M KOH at25°C.
C. A 50.00-mL sample of 0.0750 M HCN was titrated with0.3995 M NaOH. What is the pH of the resulting solutionafter 5.00 mL of NaOH were added at 25°C? Ka for HCN is6.2x10–10 at 25°C.
D. A 50.00-mL sample of 0.225 M HCO2H wastitrated with 0.1125 M NaOH. What is the pH at theequivalence point at 25°C?  Ka forHCO2H is 1.8x10–4 at 25°C.
E. A 25.00-mL sample of 0.225 M HNO2 wastitrated with 0.1111 M NaOH. What is the pH at theequivalence point at 25°C? Ka for HNO2 is7.2x10–4 at 25°C.
F. A solution of 0.600 g of diprotic acid in 100.0 mL of water wastitrated with 0.300 M NaOH to the second equivalence point. Thevolume of the base used was 34.5 mL. What is the molar mass of acidin g/mol?
G. The solubility of Gd2(SO4)3 is4.0 g/100 mL. What is the Ksp?
H. What is the molarity of Ba2+ in a saturated solutionof Ba3(AsO4)2? (Ksp = 1.1 x10-13)
I. What is the concentration of Mg2+ whenMgF2 (Ksp = 6.4 x 10-9) begins to precipitatefrom a solution that is 0.20 M F-?
J. What is the pH of a saturated solution of Pb(OH)2(Ksp = 1.2 x 10-5)?
please answer showing steps ( A to J )
