The charge balance equation of species in 0.100 M acetic acid solution is given by

Question

The charge balance equation of species in 0.100 M acetic acid solution is given by (A)  [H+]=[OH-] (B) [ H +]=[ CH 3 COO -] (C) [ H +]=[ OH -]+[ CH 3 COO -] (D) 2[ H +]=[ OH -]+[ CH 3 COO -]

Tardigrade Admin · Accepted Answer

CH 3 COOH leftharpoons CH 3 COO -+ H + [ CH 3 COO -]=[ H +] ...(i) H 2 O leftharpoons H ++ OH - [ H +]=[ OH -] ...(ii) From Eq. (i) and (ii), we get [ H +]+[ H +] =[ CH 3 COO -]+[ OH -] 2[ H +] =[ CH 3 COO -]+[ OH -]

Q. The charge balance equation of species in $0.100 M$ acetic acid solution is given by

$[H^{+}] = [O H^{-}]$

$[H^{+}] = [C H_{3} CO O^{-}]$

$[H^{+}] = [O H^{-}] + [C H_{3} CO O^{-}]$

$2 [H^{+}] = [O H^{-}] + [C H_{3} CO O^{-}]$

$C H_{3} COO H ⇌ C H_{3} CO O^{-} + H^{+}$
$[C H_{3} CO O^{-}] = [H^{+}]$ ...(i)
$H_{2} O ⇌ H^{+} + O H^{-}$
$[H^{+}] = [O H^{-}]$ ...(ii)
From Eq. (i) and (ii), we get
$[H^{+}] + [H^{+}] = [C H_{3} CO O^{-}] + [O H^{-}]$
$2 [H^{+}] = [C H_{3} CO O^{-}] + [O H^{-}]$

Q. The charge balance equation of species in 0.100M acetic acid solution is given by

[H+]=[OH−]

[H+]=[CH3​COO−]

[H+]=[OH−]+[CH3​COO−]

2[H+]=[OH−]+[CH3​COO−]