Complete and balance the precipitation reactions. Include physical states. Refer to the solubility rules as necessary

Question

precipitation reaction:

AgNO3(aq)+NaCl(aq)⟶

precipitation reaction:

K3PO4(aq)+MgCl2(aq)⟶

Answer 1

I will solve the first equation for you:

AgNO₃ (aq) + NaCl (aq) -------> AgCl (s) + NaNO₃ (aq)

How did I get the products? The positive part of AgNO₃ i.e. Ag⁺ ion combines with the negative part of NaNO₃ i.e nitrate or NO₃^- Such reactions are called double- displacement reactions.

The solubility chart tells us that AgCl is insoluble so it is labeled s

In the second problem, we need to realize that each ionic compound produces more than one of some ions.

K₃PO₄ -------> 3 K⁺ ions and one PO₄ ^3- ion

MgCl₂ ------> one Mg²⁺ ion and and 2 Cl^- ions

Now to find the products, swap the ion "partners" . Combine K and Cl to form KCl which is one of the products. The other is Mg₃(PO₄)₂ which is the solid since it is insoluble in water.

Hope this helps you get the equation. Make sure to balance it!