An aqueous solution contains 0.10 M H₂S and 0.20 M HCl. If the equilibrium constants for the formation of HS^– from H₂S is 1.0 × 10^–7 and that of S²⁻ from HS^– ions is 1.2 × 10^–13 then the concentration of S²⁻ ions in aqueous solution is:

Equilibrium: JEE Main 2018 Chemistry question

JEE Main 2018 · Session, Shift 1 · Q1318

JEE Main 2018Session, Shift 1ChemistryHardEquilibrium123× since 2002

An aqueous solution contains 0.10 M H₂S and 0.20 M HCl. If the equilibrium constants for the formation of HS^– from H₂S is 1.0

\times

10^–7 and that of S²⁻ from HS^– ions is 1.2

\times

10^–13 then the concentration of S²⁻ ions in aqueous solution is :

JEE Main 2018 Equilibrium Question with Solution (Session Shift 1, Q1318) | JEE Arc

JEE Main 2018 · Session, Shift 1 · Q1318

JEE Main 2018Session, Shift 1ChemistryHardEquilibrium123× since 2002

An aqueous solution contains 0.10 M H₂S and 0.20 M HCl. If the equilibrium constants for the formation of HS^– from H₂S is 1.0

\times

10^–7 and that of S²⁻ from HS^– ions is 1.2

\times

10^–13 then the concentration of S²⁻ ions in aqueous solution is :