Answer
a. $3Na^+(aq) + P{O_4}^{3-}(aq) 3Ag^+(aq) + 3N{O_3}^-\longrightarrow 3Na^+(aq) + 3N{O_3}^-(aq) + Ag_3P{O_4}(s)$ $ P{O_4}^{3-}(aq) + 3Ag^+(aq) \longrightarrow Ag_3P{O_4}(s)$
b. No solid forms
c. $Pb^{2+}(aq) + 2N{O_3}^-(aq) + 2Na^+(aq) + C{O_3}^{2-}(aq) \longrightarrow 2Na^+(aq) + 2N{O_3}^-(aq) + PbCO_3(s)$ $Pb^{2+}(aq)+C{O_3}^{2-}(aq) \longrightarrow PbCO_3(s)$
d. $Ba^{2+}(aq) + 2Cl^-(aq) + 2 K^+(aq) + 2OH^-(aq) \longrightarrow Ba(OH)_2(s) + 2Cl^-(aq) + 2K^+(aq)$
$Ba^{2+}(aq) + 2OH^-(aq) \longrightarrow Ba(OH)_2(s) $
Work Step by Step
1. Write the double replacement reactions, without specifying the physical states of the products.
a. $Na_3PO_4(aq) + 3AgNO_3(aq) \longrightarrow 3NaNO_3 + Ag_3PO_4$
b. $K_2SO_4(aq) + Na_2CO_3(aq) \longrightarrow K_2CO_3 + Na_2SO_4$
c. $Pb(NO_3)_2(aq) + Na_2CO_3(aq) \longrightarrow 2NaNO_3 + PbCO_3$
d. $BaCl_2(aq) + 2KOH(aq) \longrightarrow Ba(OH)_2 + 2KCl$
2. Predict if each product is soluble in water.
a. $NaNO_3$ contains the $Na^+$ ion: Soluble. $Ag_3PO_4$ does not contain any ion of the list on Table 9.7: Insoluble
b. $K_2CO_3$ contains the $K^+$ ion: Soluble. $Na_2SO_4$ contains the $Na^+$ ion: Soluble.
c. $NaNO_3$ contains the $Na^+$ ion: Soluble. $PbCO_3$ does not contain any ion of the list on Table 9.7: Insoluble
d. $Ba(OH)_2$ does not contain any ion of the list on Table 9.7: Insoluble. B$KCl$ contains the $K^+$ ion: Soluble.
3. For those reactions with an insoluble product, write the ionic equation:
a. $3Na^+(aq) + P{O_4}^{3-}(aq) 3Ag^+(aq) + 3N{O_3}^-\longrightarrow 3Na^+(aq) + 3N{O_3}^-(aq) + Ag_3P{O_4}(s)$
c. $Pb^{2+}(aq) + 2N{O_3}^-(aq) + 2Na^+(aq) + C{O_3}^{2-}(aq) \longrightarrow 2Na^+(aq) + 2N{O_3}^-(aq) + PbCO_3(s)$
d. $Ba^{2+}(aq) + 2Cl^-(aq) + 2 K^+(aq) + 2OH^-(aq) \longrightarrow Ba(OH)_2(s) + 2Cl^-(aq) + 2K^+(aq)$
4. Remove the repeated ions to get the net ionic equation.
a. $ P{O_4}^{3-}(aq) + 3Ag^+(aq) \longrightarrow Ag_3P{O_4}(s)$
c. $Pb^{2+}(aq)+C{O_3}^{2-}(aq) \longrightarrow PbCO_3(s)$
d. $Ba^{2+}(aq) + 2OH^-(aq) \longrightarrow Ba(OH)_2(s) $
