Lab Ionic PDT past year PSPM II

Name        :  _________________________

Matrix No :  MS1123_______

Tutor         : DM_ P_

1.      What is the pH of a mixture of solutions containing 9.60 mL 0.1 M NaOH solution and 10.00 mL 0.1M HCl solution?

            n NaOH = MV/1000                                                n HCl = MV/1000 

         

            [ HCl] that remains  =  _______________                                                                  

                                               

                                                             =

            pH = - log [ H⁺]

                  =

                  = _____

      2. The solubility product, K_sp for AgCl is 1.0x10^-10 M². Calculate the solubility of AgCl in

  i. water                                                                                

            ii.   0.2 M HCl                                                            

            iii.0.1 M AgNO₃

3.  Calculate the acid  ionisation constant, K_a of ethanoic acid , CH₃COOH in a mixture of solution

    (pH = 5.44) containing 0.1 mol dm^-3 ethanoic acid solution and  0.5 mol dm^-3 sodium ethanoate.

4.  At 25°C, 2.20% of 0.125 M benzoic acid, C₆H₅COOH ionized.  Write the ionisation equation for benzoic

    acid in water.  Determine the acid ionisation constant, K_a for benzoic acid and calculate its pH value.

5. Write the solubility equilibrium equation and calculate the molar solubility for Hg(OH)₂

    if K_sp = 3.2x10^-26

      6. Write the equation for the base ionisation of 0.5 M aqueous solution of CH₃NH₂ and calculate its pH

          value.     [K_b = 3.7x10^-4 M]

         CH₃NH_2(aq)  + H₂O_(l)     CH₃NH₃⁺_(aq)  + OH^-_(aq)

7. Does a precipitate form when 1.0x10^-2 mol of Ba(NO₃)₂ and 2.0x10^-2 mol of NaF are dissolved in water and 

    made up to 1.0 L solution? [K_sp BaF₂ = 1.7x10^-6]

8. Explain how a 50-mL HCl solution with pH 1.25 can be prepared from 11.6 M HCl?

9. In an acid-base titration, 10 mL of 0.45 M HCl was added to 40 mL 0.10M NaOH. Determine the pH of the

    solution formed

10. Calculate the pH for 0.02 M Ba(OH)₂ solution.

11. The pH value for a solution containing 0.245 mol HF in 500 mL water is 1.88. Calculate the ionisation

     constant for HF.

Answer:

1) 2.69

2) H2O = 1 x 10-5

    HCl = 5 x 10-10

    AgNO3 = 1 x10-9

3) 1.82 x 10-5

4) 2.56 Ka = 6.12 x 10-5

5) 2 x 10-9

6) 12.13

7) Q=4 x 10-6

8) 0.24 mL

9) 2

10) 12.6

11) Ka=3.643 x 10-4