Question

a 0.2 mole of solid nh4cl is placed in one beaker and 0.1 mol of solid agno3 is placed in a second beaker. then, 100 ml of water is added to each beaker. finally, both beakers are mixed in a titration. (a) will both solids, one solid or no solid dissolve when the water is added to each beaker? (b) what type(s) of reaction, if any, will occur when the two chemicals come into contact with each other? (c) write the balanced, net - ionic equation for the reaction or write “n/a” if no reaction occurs. (d) draw a diagram to illustrate the resulting solution that is formed at the end of the reaction.

Explanation:

Step1: Solubility of solids

Both $NH_4Cl$ and $AgNO_3$ are soluble in water. When water is added to each beaker, both solids will dissolve.

Step2: Identify reaction type

When the two solutions are mixed, the reaction is a double - displacement reaction. The chemical reaction is $NH_4Cl(aq)+AgNO_3(aq)
ightarrow NH_4NO_3(aq) + AgCl(s)$. The net - ionic equation is $Ag^+(aq)+Cl^-(aq)
ightarrow AgCl(s)$.

Step3: Draw diagram

The resulting solution will contain $NH_4^+$, $NO_3^-$ ions in solution and solid $AgCl$ precipitated out. A diagram could show a beaker with a layer of solid $AgCl$ at the bottom and a clear solution above it with water molecules, $NH_4^+$ and $NO_3^-$ ions represented as small particles dispersed in the solution.

Answer:

(a) Yes, both solids will dissolve when water is added to each beaker.
(b) Double - displacement reaction occurs when the two chemicals come into contact with each other.
(c) $Ag^+(aq)+Cl^-(aq)
ightarrow AgCl(s)$
(d) A beaker with solid $AgCl$ at the bottom and a solution containing $NH_4^+$ and $NO_3^-$ ions above it.