Question

what is the pH of a 0.315 M solution of H2SO4 Ka2= 1.20 x 10^-2

1 Question (3 points) 3rd attempt What is the pH of a 0.315 M solution of H2SO4? Ka2 = 1.20x10-2 2nd attempt

Answer 1

Answer. - Let consider that tsoo is very dissociate completely by losing all very easily Groong its acid, proton It's dissociation are as follows.al First dissociation. losing its proton is the equilibrium ty soleaas HSO4 + spea) ] Ka, = [4sozi] [4 [th sca] Second dissociation of Soup as a solo cajt it can - Ką = [sof [H] Lesey g . .20 x 102 0.315 Let's calculate LH+] for the first proton [H+] = [tysop] = 0.315M and work this into our second proton calculation se(0:315 + de) dissociation 9.215 = 1.20x10 e = 0.012

Hence, the pH g solution is - - pH -log[H+1 -- dog (0:315) = -logo (3.1 x17) - - logo 3.1+1 - 1 - logo 3.1 1-0.491 a 0.sol ... pH g 0.315 M aq. soup is = 0.501 |