Arrhenius (1 Viewer)

Dubble-u25 · Jan 24, 2012

Using arrhenius' definition of an acid, what would NaHCO₃be classified as?
Would it be an acid because it releases H⁺ ions in solution?

NaHCO_{3 (s)}→ Na⁺_(aq) + H⁺_(aq)+ CO₃^2-_(aq)

nightweaver066 · Jan 24, 2012

kingkong123 · Feb 29, 2012

nightweaver066 said:
$NaHCO_{3(aq)} \rightarrow Na^+_{(aq)} + HCO^-_{3(aq)}$

$HCO^-_{3(aq)} + H_2O_{(l)} \rightarrow H_2CO_{3(aq)} + OH^-_{(aq)}$

$So $ NaHCO_3 $ is not an Arrhenius acid/base but $ HCO^-_{3(aq)} $ is the Arrhenius base forming hydroxide ions in solution$

how do u know water will act as an acid the second reaction? couldnt it act as a base and the reaction be

$HCO^-_{3(aq)} + H_2O_{(l)} \rightarrow H_3O^+_{(aq)} + CO_3^{2-}$ ???

Arrhenius (1 Viewer)

Dubble-u25

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