Asked by Anonymous
Each of the following solutions has a concentration of 0.1 mol/L. Compare the hydronium-ion concentration and pH in each pair, and explain why they are different.
a) H2SO4(aq) vs. H2SO3(aq)
b) H2S(aq) vs. NH3(aq)
a) H2SO4(aq) vs. H2SO3(aq)
b) H2S(aq) vs. NH3(aq)
Answers
Answered by
DrBob222
a) H2SO4 is a strong acid (at least the first H is) and H2SO3 is a weak acid (both H are weak).
The H3O^+ of H2SO4 is essentially the molarity. For H2SO3, you must set up an ICE chart from
H2SO3 ==> H^+ + HSO3^-
and solve for H^+
For H2S,
H2S ==> H^+ + HS^-
Set up ICE chart and solve for H^+.
For NH3,
NH3 + HOH ==> NH4^+ + OH^-
Set up ICE chart and solve for OH^- and convert to pH.
There isn't anything difficult about this question but it's a lot of leg work to get it done.
Post your work if you get stuck.
The H3O^+ of H2SO4 is essentially the molarity. For H2SO3, you must set up an ICE chart from
H2SO3 ==> H^+ + HSO3^-
and solve for H^+
For H2S,
H2S ==> H^+ + HS^-
Set up ICE chart and solve for H^+.
For NH3,
NH3 + HOH ==> NH4^+ + OH^-
Set up ICE chart and solve for OH^- and convert to pH.
There isn't anything difficult about this question but it's a lot of leg work to get it done.
Post your work if you get stuck.