Question

20.00 mL of a 0.077 M solution of silver nitrate, AgNO3, is mixed with 30.00 mL of a 0.043 M solution of sodium acetate, NaC2H3O2. Does a precipitate form? The Ksp of AgC2H3O2 is 2.5*10^-3.

Answer 1

Answer:

No, no precipitate is formed.

Explanation:

Hello there!

In this case, since the reaction between silver nitrate and sodium acetate is:

$AgNO_3(aq)+NaC_2H_3O_2(aq)\rightarrow AgC_2H_3O_2(s)+NaNO_3(aq)$

In such a way, we can calculate the concentration of silver and acetate ions in the solution as shown below, and considering that the final total volume is 50.00 mL or 0.0500 L:

$[Ag^+]=\frac{20.00mL*0.077M}{50.00mL}=0.0308M$

$[C_2H_3O_2^-]=\frac{30.00mL*0.043M}{50.00mL}=0.0258M$

In such a way, we can calculate the precipitation quotient by:

$Q=[Ag^+][C_2H_3O_2^-]=0.0308*0.0258=7.95x10^{-4}$

Which is smaller than Ksp and meaning that the precipitation does not occur.

Regards!