Which of the following substances has the greatest solubility in water?
A. Ca(OH)2, Ksp = 6.5 × 10-6
B. Ag2SO4, Ksp = 1.5 × 10-5
C. PbI2, Ksp = 7.9 × 10-9
D. Zn(IO3)2, Ksp = 3.9 × 10-6
E. BaF2, Ksp = 1.5 × 10-6
B. Ag2SO4, Ksp = 1.5 × 10-5
Well, when it comes to solubility in water, it's like having a dance party. Everyone's trying to get their groove on and mingle with the water molecules. So, let's see who's going to be the life of the party!
First up, we have Ca(OH)2 with a Ksp of 6.5 × 10-6. Hmm, not too shabby, but let's keep going.
Next, we have Ag2SO4 with a Ksp of 1.5 × 10-5. Ooh, silver wants to make a statement! Good for you, silver!
Now, we have PbI2 with a Ksp of 7.9 × 10-9. PbI2 seems a bit shy, but don't worry, you'll find your place on the dance floor!
Zn(IO3)2 is up next with a Ksp of 3.9 × 10-6. Zn(IO3)2, you're not too far behind. Keep on grooving!
Finally, we have BaF2 with a Ksp of 1.5 × 10-6. BaF2, you're matching the same Ksp as Ag2SO4. Looks like we have a tie!
So, out of all the substances, Ag2SO4 and BaF2 have the greatest solubility in water. They're really rocking the dance floor and getting cozy with those water molecules. Keep up the great moves, you two!
To determine which substance has the greatest solubility in water, we need to compare their solubility product constants (Ksp) values. The greater the Ksp value, the more soluble the substance is in water.
Now let's compare the Ksp values of each substance:
A. Ca(OH)2, Ksp = 6.5 × 10^-6
B. Ag2SO4, Ksp = 1.5 × 10^-5
C. PbI2, Ksp = 7.9 × 10^-9
D. Zn(IO3)2, Ksp = 3.9 × 10^-6
E. BaF2, Ksp = 1.5 × 10^-6
Comparing the values, we can see that:
- PbI2 has the smallest Ksp value.
- BaF2 and Zn(IO3)2 have similar but slightly higher Ksp values.
- Ca(OH)2 has a higher Ksp value than BaF2 and Zn(IO3)2.
- Ag2SO4 has the highest Ksp value.
Therefore, the substance with the greatest solubility in water is Ag2SO4, with a Ksp value of 1.5 × 10^-5. So the correct answer is B.
To determine which substance has the greatest solubility in water, we need to compare the solubility product constants (Ksp) of each substance. The higher the Ksp value, the more soluble the substance is.
Let's compare the Ksp values of each substance:
A. Ca(OH)2, Ksp = 6.5 × 10^-6
B. Ag2SO4, Ksp = 1.5 × 10^-5
C. PbI2, Ksp = 7.9 × 10^-9
D. Zn(IO3)2, Ksp = 3.9 × 10^-6
E. BaF2, Ksp = 1.5 × 10^-6
Comparing the values, we can see that:
- Ag2SO4 has the highest Ksp value, followed by Ca(OH)2, Zn(IO3)2, BaF2, and PbI2.
Therefore, the substance with the greatest solubility in water among the given options is Ag2SO4 (silver sulfate).
A grossly mis-leading question. The question should state if the solubility is to be compared by molarity or grams. If we assume it is to be molar (which is a little easier);
The only way to really do this is to calculate the solubility of each.
Set up an ICE chart for each, substitute into the Ksp expression, and solve for solubility. Then compare.
I can save you some time. All of them will be 4S^3 = Ksp. Solve for S where S stands for solubility in mols/L. You may wish to confirm that each is 4S^3 = Ksp.