A→ B→H2CO3⇌H++HCO3−HCO3−⇌H++CO3−2K1=4.2×10−7 K2=4.8×10−11 As K2≪K1 All major [H+]todal ≈[H+]A and from I equilibrium, [H+]A≈[HCO3−]≈[H+]tocal [CO3−2] is negligible compared to [HCO3−]or [H+]total
JEE Main 2010 — Chemistry Physical Chemistry
In aqueous solution the ionization constants for carbonic acid are K1=4.2×10−7 and K2=4.8×10−11 Select the correct statement for a saturated 0.034M solution of the carbonic acid.
Held on 30 Apr 2010 · Verified 6 Jul 2026.
The concentration of CO32− is 0.034M.
The concentration of CO32− is greater than that of HCO3−.
The concentration of H+and HCO3−are approximately equal.
The concentration of H+is double that of CO32−.
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