Please answer ANYTHING you can!!
2) The acid-dissociation constant for hypochlorous acid (HClO) is 3.0 x 10^-8. Calculate the concentrations of:
(a) H3O+
(b) ClO-
(c) HClO
at equilibrium if the initial concentration of HClO is 0.0075 M.
3) (a) Given that the Ka for acetic acid is 1.8 x 10^-5 and that for hypochlorous acid is 3.0 x 10^-8, which is the stronger acid;
(b) Which is the stronger base, the acetate ion or the hypochlorite ion?
(c) Calculate the Kb values for C2H3O2- and ClO-.
4) Atmospheric CO2 level seem to have risen by approximately 20% over the past 40 years from 315 ppm to 375 ppm.
(a) Given that the average pH of clean, unpolluted rain today is 5.4, determine the pH of unpolluted rain 40 years ago. You may assume that carbonic acid (H2CO3) formed by the reaction of CO2 and water is the only factor affecting pH by the reaction:
CO2(g) + H2O(l) <===> H2CO3(aq);
(b) What volume of CO2 at 25oC and 1 atm is dissolved in a 20.0-L bucket of today’s water?
THANK YOU!
2) The acid-dissociation constant for hypochlorous acid (HClO) is 3.0 x 10^-8. Calculate the concentrations of:
(a) H3O+
(b) ClO-
(c) HClO
at equilibrium if the initial concentration of HClO is 0.0075 M.
3) (a) Given that the Ka for acetic acid is 1.8 x 10^-5 and that for hypochlorous acid is 3.0 x 10^-8, which is the stronger acid;
(b) Which is the stronger base, the acetate ion or the hypochlorite ion?
(c) Calculate the Kb values for C2H3O2- and ClO-.
4) Atmospheric CO2 level seem to have risen by approximately 20% over the past 40 years from 315 ppm to 375 ppm.
(a) Given that the average pH of clean, unpolluted rain today is 5.4, determine the pH of unpolluted rain 40 years ago. You may assume that carbonic acid (H2CO3) formed by the reaction of CO2 and water is the only factor affecting pH by the reaction:
CO2(g) + H2O(l) <===> H2CO3(aq);
(b) What volume of CO2 at 25oC and 1 atm is dissolved in a 20.0-L bucket of today’s water?
THANK YOU!