How do you balance the following reaction: $? K O H + ? H_{3} P O_{4} \to ? K_{3} P O_{4} + ? H_{2} O$ $?KOH + ?H_3PO_4 -> ?K_3PO_4 + ?H_2O$ ?

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Answer 1 · 2017-01-21T09:58:02

$Garbage in must equal garbage out........$ $"Garbage in must equal garbage out........"$

$H_{3} P O_{4} (a q) + 3 K O H (a q) \to K_{3} P O_{4} (a q) + 3 H_{2} O (l)$ $H_3PO_4(aq) + 3KOH(aq) rarr K_3PO_4(aq) + 3H_2O(l)$

This reaction is a bit of an idealization, inasmuch as phosphoric acid behaves as a diprotic acid in water.

A more realistic interpretation would be,

$H_{3} P O_{4} (a q) + 2 K O H (a q) \to K_{2} H P O_{4} (a q) + 2 H_{2} O (l)$ $H_3PO_4(aq) + 2KOH(aq) rarr K_2HPO_4(aq) + 2H_2O(l)$

In both cases, are mass and charge conserved? If they are not, then you know that the reaction does not reflect reality.

How do you balance the following reaction: ?KOH+?H3PO4→?K3PO4+?H2O?KOH + ?H_3PO_4 -> ?K_3PO_4 + ?H_2O?