Answer:
Kc> 1, because [tex]H_2SO_3[/tex] is a stronger acid than [tex]H_2SeO_3[/tex]
Explanation:
We have to start analyzing the reaction:
[tex]HSeO_3^-~+~H_2SO_3~<->~H_2SeO_3~+~HSO_3^-[/tex]
When we search the pKa values for each we will find:
pKa of [tex]H_2SO_3[/tex]= 1.81
pKa of [tex]H_2SeO_3[/tex]= 2.62
When we have a smallest pKa value we will have more acidity, therefore [tex]H_2SO_3[/tex] is a stronger acid than [tex]H2SeO3[/tex]. Additionally, if we have his behavior the reaction would be displaced to the right side due to the strong acid (the strong acid is placed in the reactives side), so we will have a K greater than 1.
The answers are:
a) Kc< 1, because [tex]H_2SO_3[/tex] is a stronger acid than [tex]H_2SeO_3[/tex]
b) Kc< 1, because [tex]H_2SO_3[/tex] is a weaker acid than [tex]H_2SeO_3[/tex]
c) Kc> 1, because [tex]H_2SO_3[/tex] is a weaker acid than [tex]H_2SeO_3[/tex]
d) Kc> 1, because [tex]H_2SO_3[/tex] is a stronger acid than [tex]H_2SeO_3[/tex]
The answer that fits with the previous analysis is "d". The molecule [tex]H_2SO_3[/tex] is the strongest acid and K is greater than one
