C=0.01MKb=1×10−12 at 25∘CBOH⇌B++OH−C00 at eq. C−CαCαCα [OH−][OH−]=Cα=KbC=1×10−12×10−2 [OH−]=10−7 mol L−1 Related Theory The activities of the solutes are approximated with molarities. The dissociation constant is an immediate consequence of the law of mass action which describes equilibria in a more general way. The dissociation constant is also sometimes called ionization constant when applied to salts.
At 25° C, the dissociation constant of a base, BOH, is 1.0 × 10^-12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would…
NEET UG 2005 — Chemistry Physical Chemistry
2005mcqmedium
At 25∘C, the dissociation constant of a base, BOH, is 1.0×10−12. The concentration of hydroxyl ions in 0.01M aqueous solution of the base would be:
Official previous-year question
Held on 30 Apr 2005 · Verified 9 Jul 2026.
Options
- A
1.0×10−5 mol L−1
- B
1.0×10−6 mol L−1
- C
2.0×10−6 mol L−1
- D
1.0×10−7 mol L−1
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