Question - 1) A mixture of equal volumes of equimolar solutions of acetic acid and sodium acetate is made in 1 L flask. Calculate the pH of the solution.
2) A sample of 10.0 mL solution of 0. 100 M acetic acid is titrated with 0.100 M NaOH solution. Calculate the pH of the solution when exactly 5.00 mL of the base has been added.
3) Calculate the solubility in molarity of Cu(OH)2, (a) In pure water and in (b) 0.010M Cu(NO3)2 solution. The Ksp for Cu(OH)2 is 2.2O x 10^-20.
4) (a) Calculate the value for Ksp for CaSO4 that has the solubility of 0.67 g/L in water.
(b) If we mix 50.0 mL of 0.100 M Na2SO4 with 5.00 mL 0f 0.100 M BaCl2, will there be any precipitation of BaSO4? Look up for Ksp value for BaSO4.
I'm seeking good explanation please be as thorough as possible.
Explicate the each step. Explicate the process and each step.