Question

13) We often think of HO, in terms of tropospheric ozone formation, but it can also be important in aqueous phase acid/base chemistry. Consider a mixing ratio for HO, at sea level of 4.0 x 10 a) The Henry's law equilibrium constant for HO, dissolving in water is 2000 M/atm. Calculate the concentration, in M, of HO, in the aqueous phase. b) HO, can act as an acid in water according to the reaction HO2 + H2O → H3O + O2 with a Ka=2.05 x 10M. Calculate the pH of a rain droplet assuming HO, is the only acid present.

Answer 1

Simple equation of Henry's law has been used to solve the problem.
SUYU Here mixing xatto for Ho, at sea level = 4.0x 1õ? >> partiel počessure, due to H0, mixing xation x total amoophone pressure = 4.0 x16?x i atm = 40x10 am According to Henryl law Concentration of HO2 diasoved water = pestral pres use of HO2 x Henry's law = 4:0x100 atm x 2000 m/ atm = 8.0x10CM o Conerdes the reaction - HO₂ + H2O - H₂ot to let a be concentration of H30t and or during equlibrium Nowo, we know ka for given reaction so CSscanned with CamScalicer = [hzot] [07] - as ka very small Now, we know I

ka = [1408] [03] as ka very small 2-05 x 108 M = xxx me = R05X108 * = V2-05X108 = 1.43X104 m. Here we know [H3O+] = 1.43X10" M olso [H30+] - [H+] ay H+ dous not exist separately in aqeous solution We komen pH = -log(t)) => pl = -log (143 2104) = 384 - pH of a sain droplet assuming Hoe is the only and present is 3.84. 3 = 3.84 csscanned with CamScanner