Question

A solution composed of 5.00 mL of 0.0120 M Pb(NO3)2, 3.00 mL of 0.0300 M KI, and 2.00 mL of 0.20 M KNO3 is determined spectroscopically to have [1'] = 6.25 x 10 Show all steps of your calculations. Credit will not be given if work is not shown. (2 pt) a). How many moles of l' is present initially? OIL OB S+3+2=10nL M = a. 1o-s b). How many moles of I should precipitate from the solution? " Xo noles (2 pt) 3. A student performed Experiment 4 and found that K, for HAC was 2.59 x 10-5. What was the pH after addition of 3 mL of Solution A (0.160 M HAc) to 50 mL of Solution B (6.40 x 10-3M Ac)? Show all calculations. (2 pt)

Answer 1

solution 5.00 ml of 0 0100M Pb(NO3). 300 ml of 0 0300M KI 200 ml of 0.20 M KNO₃ [1] . 6.25 X10-3M Moles of I present initially Volume & Molarity 0.0030 L x 0. 030 mol/L - 9.0 x 10-5 mol I Moles of I precipitated - Initial moles - Equilibrium moles. Equilikium moles die Total volume = 5.00ml + 5:00 ml + 2.00 ml = 10.00 mL = 0.012: kgruilibrium volume of I (0.0100) L (5.4X105 mol/L) e 5.4810-5 mol I Moles of I precipitated: - 9.0x10-5 und – 5.4X10 mol 36x10 - Smel I