Answer:
a) The predominant Brownstead-Lowry acid- base is perchloric acid
b) A conjugate acid base pair is HClO4 and ClO4^-
c) forward reaction is favored and equilibrium position lies towards the far right
Explanation:
The molecular equation is;
HClO4(aq) + NaH2PO4(aq) -----> H3PO4(aq) + NaClO4(aq)
The net ionic equation of the reaction is;
H^+(aq) + H2PO4^-(aq) ----> H3PO4(aq)
The predominant Brownstead-Lowry acid- base is perchloric acid .
A conjugate acid base pair is HClO4 and ClO4^-
Since the both species; perchloric acid and sodium dihydrogen phosphate are both highly soluble in water yielding ions and also dissociate to a large extent in solution, the forward reaction is favoured leading to the formation of phosphoric acid. Remember that phosphoric acid does not easily dissociate in solution hence the forward reaction is faster than the reverse reaction and the equilibrium position lies towards the far right.
