DQuestion 2 1 pts What is the pH of the solution that result

DQuestion 2 1 pts What is the pH of the solution that results from the addition of 12.5 mL of 0.500 M HC to 50.0 ml of 0.100 M NaCIO? K (HCIO)-2.9E-8 Please answer to two DECIMAL places. F10F11 F12 Prtscr Irvsert 5 6 78

Solution

50.0 ml of 0.100 M NaClO = 0.050 * 0.100 = 0.005 mole.

12.5 ml of 0.500 M HCl = 0.0125 * 0.500 = 0.00625 mole.

NaClO + HCl ..............> HClO + NaCl

so moles of excess acid = 0.00625 - 0.005 = 0.00125 mole.

volume of solution = (50.0 + 12.5) = 62.5 ml.

concentration of extra HCl = 0.00125 * 1000 / 62.5 = 0.02 M

PH = -log [H+] = -log[HCl] = -log (0.002) = 1.69

PH = 1.69