A solution is made initially with 0.200 M HIO₃ (Kc = 0.170). Once the equilibrium below is established, what is the equilibrium concentration of H⁺ ions? HIO₃ (aq) ⇌ H+ (aq) + IO₃⁻ (aq)

Question

A solution is made initially with 0.200 M HIO₃ (Kc = 0.170). Once the equilibrium below is established, what is the equilibrium concentration of H⁺ ions? HIO₃ (aq) ⇌ H+ (aq) + IO₃⁻ (aq)

Answer 1

HIO₃ (aq) ⇌ H+ (aq) + IO₃⁻ (aq)

0.200...........0................0

-x................+x................+x

0.2-x...........x..................x+

K=^([H+][IO3-])/_([HIO3])

0.170=x²/(0.2-x)

x=0.118

[H+]=x=0.118