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

To determine if a precipitate will form, compare the reaction quotient (Q) to the solubility product constant (Ksp).

Step-by-step explanation:

When mixing two solutions, we can determine whether or not a precipitate will form by comparing the reaction quotient (Q) to the solubility product constant (Ksp) for the compound.

In this case, the compound of interest is Ag2SO4. If the Q value is greater than the Ksp value, a precipitate will form.

Using the given concentrations of Na2SO4 and AgNO3, we can calculate the Q value and compare it to the Ksp value to determine if a precipitate will form.

Answer 2

No precipitate will be formed.

Step-by-step 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^+] = (0.05*150)/((150+150))`

`[Ag^+] = (7.5)/((300.0))`

`[Ag^+] = 0.025 \ M`

`[SO_4^(2-)] = (0.15*150.0)/(150.0+150.0)`

`[SO_4^(2-)] = (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.