Bronsted-Lowry acids and bases?

Question

label the Bronsted-Lowry acids & bases in the following equations, and tell which substances r conjugate acid-base pairs:

2-
a. CO3 (aq)+ HCL (aq)---> HCO3-(aq)+Cl-(aq)

b. H3PO4(aq)+NH4(aq)--->H2PO4-(aq)+NH4+(aq)

c. NH4+(aq)+CN-(aq)<--->NH3(aq)+HCN(aq)

d.HBr(aq)+OH-(aq)--->H2O(l)+Br-(aq)

2-
e.H2PO4-(aq)+N2H4(aq)<--->HPO4 (aq)+N2H5+(aq)

Answer 1

Look at which species have lost a proton, and which have ganied one.

In (a) carbonate ion is the base, and hydrogencarbonate its conjugate acid.

In (b) I think you have made a mistake. NH3 should be on the left hand side, and it is a base, and NH4+, its conjugate acid, is on the other side, which you didn't type out.

In (c) ammonium is the acid, and ammonia is its conjugate base.

In (d) HBr is the acid, and Br- its conjugate base.

in (e) hydrazine is the base, and hydrazinium ion is its conjugate acid.

Now you can work out the other pairs.

Answer 2

water can act as the two bronsted lowry acid and base bear in mind lowry-bronsted acid donates hydrogen lowry-bronsted base accepts hydrogen mnemonic - undesirable H2O + NaOH - H3O+(ion) + NaO-(ion) acid1 base2 base1 acid2 lowry-bronsted acid base fprmation continually includes formation of ions you're able to attempt the above same rxn with acid subsequently water reacts the two with acid and base to fulfill the circumstances of lowry-bronsted yet HCl, NH3, NaOH do no longer.