# If each of the following were placed in water, identify the ions (if any) that would exist in solution and specify concentration of each. a) 2.4mol (NH4)2CO3 b) 0.2 mol HClO2 c) 2.00 mol AgCl...

If each of the following were placed in water, identify the ions (if any) that would exist in solution and specify concentration of each.

a) 2.4mol (NH4)2CO3

b) 0.2 mol HClO2

c) 2.00 mol AgCl

d) 4.5 mol HBr

I am stuck on this homework problem and would appreciate if you would help explain it to me.

gsenviro | Certified Educator

When dissolved in water, compounds tend to dissociate into ions. Some compounds do it faster than others. Let us assume that these compounds were dissolved in 1 lt of water.

a) 2.4 mol (NH4)2CO3: This will dissociate into ammonium ion (`NH4^+` ) and carbonate ions (`CO_3^(2-)` ). The concentration of ammonium ion would be 4.8 mole (= 2 x 2.4) per liter and that of carbonate is 2.4 moles/lt.

b) 0.2 mol HClO2: Chlorous acid will dissociate into H+ and ClO2- ions, the concentration of each would be 0.2 mol/lt.

c) 2 mol AgCl: silver chloride will dissociate into silver ion (Ag+) and chloride ion (Cl-). The concentration of each species would be 2 mol/lt.

d) 4.5 mol HBr: Hydrobromic acid dissociates into hydrogen ion (H+) and bromide ion (Br-). Concentration of each species is 4.5 mol/lt.

Hope this helps.