Answer
a. $K_2CO_3$
b. $K_3PO_4$
c. $K_2HPO_4$
d. $KC_2H_3O_2$
Work Step by Step
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 $K$: $K^{+}$
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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.
$K(C_2H_3O_2)_1: KC_2H_3O_2$
