Question

150 mL of 0.15 M Na2SO4 is mixed with an equal volume of 0.050 M Agno3. Select all the options that correctly show the steps used to determine whether or not a precipitate will form, if Ksp for Ag2SO4

Answer 1

Answer:

No precipitate will be formed.

Explanation:

Given that ;

150 mL of 0.15 M $Na_2SO_4$ is mixed with an equal volume of 0.050 M $AgNO_3.$

Then;

$[Ag^+] = \frac{0.05*150}{(150+150)}$

$[Ag^+] = \frac{7.5}{(300.0)}$

$[Ag^+] = 0.025 \ M$

$[SO_4^{2-}] = \frac{0.15*150.0}{150.0+150.0}$

$[SO_4^{2-}] = \frac{22.5}{300.0}$

$[SO_4^{2-}] = 0.075 \ M$

For $Ag_2SO_4$ ; $[Ag^+]^2 [SO_4^{2-}]$

$=(0.025)^2 *(0.075)$

$=4.6875*10^{-5}$

The Ksp of $Ag_2SO_4$ = $1.5*10^{-5}$ ;

Therefore since $4.6875*10^{-5}$ is < Ksp of $Ag_2SO_4$ ; Then no precipitate will be formed.