## Chemistry: Molecular Approach (4th Edition)

a. $K_2CO_3$ b. $K_3PO_4$ c. $K_2HPO_4$ d. $KC_2H_3O_2$
Use table 3.4 (Page 100) and figure 3.7 (Page 98) to see the charges and the formula of the ions. - Potassium has a charge of $1+$, and its symbol is $K$: $K^{+}$ ------- a. Carbonate ion is: $CO_3^{2-}$ (See table 3.4). Potassium : $K^+$ Put these two together, where the subscript number will be the charge of the other ion. Potassium will receive 2, and the carbonate will receive 1. $K_2(CO_3)_1$: $K_2CO_3$ b. Phosphate ion is: $PO_4^{3-}$ (See table 3.4). Potassium : $K^+$ Put these two together, where the subscript number will be the charge of the other ion. Potassium will receive 3, and phosphate will receive 1. $K_3(PO_4)_1: K_3PO_4$ c. Hydrogen phosphate ion is: $HPO_4^{2-}$ (See table 3.4). Potassium : $K^+$ Put these two together, where the subscript number will be the charge of the other ion. Potassium will receive 2, and the hydrogen phosphate will receive 1. $K_2(HPO_4)_1$: $K_2HPO_4$ d. Acetate ion is: $C_2H_3O_2^{-}$ (See table 3.4). Potassium : $K^+$ Put these two together, where the subscript number will be the charge of the other ion. Potassium will receive 1, and the acetate will receive 1. $K(C_2H_3O_2)_1: KC_2H_3O_2$