value and formula Ksp Of :
-PbI2
-CdS
-Ca(OH)2
-Ag2CrO4
-Cu2S
Ksp values vary with temperature, so you have to specific on the temperature of the system. Also, you can search for Ksp values of each in google or from your textbook.
For the formulas, write first the balanced reaction. For example, for the first one, PbI2:
PbI2 <---> Pb(+) + 2 I(-)
Thus, its Ksp formula would be:
Ksp = [ Pb+ ] [ I- ] ^ 2
For CdS:
CdS <---> Cd(2+) + S(2-)
Thus,
Ksp = [ Cd(2+) ] [ S(2-) ]
Now try doing the others.
hope this helps~ `u`
(I apologize if someone already posted an answer/solution before me. My internet had become slow again and I can't seem to post a comment right away.)
To determine the value and formula for the Ksp (solubility product constant) of the given compounds, we need to know the solubility information of these compounds.
The Ksp of a compound is a measure of its solubility in water. It represents the equilibrium constant for the dissociation of the compound into its constituent ions when it is in a saturated solution.
Let's go through each compound and find their respective Ksp values and formulas:
1. PbI2 (Lead(II) iodide):
The solubility of PbI2 can be determined experimentally or by looking it up in reference sources. Let's assume its solubility is "x" mol/L.
The balanced equation for the dissociation of PbI2 is:
PbI2 (s) ⇌ Pb2+ (aq) + 2I- (aq)
The Ksp expression for PbI2 is:
Ksp = [Pb2+][I-]^2 = x(2x)^2 = 4x^3
2. CdS (Cadmium sulfide):
Similarly, let's assume the solubility of CdS is "y" mol/L.
The balanced equation for the dissociation of CdS is:
CdS (s) ⇌ Cd2+ (aq) + S2- (aq)
The Ksp expression for CdS is:
Ksp = [Cd2+][S2-] = y*y = y^2
3. Ca(OH)2 (Calcium hydroxide):
The solubility of Ca(OH)2 can also be determined experimentally or from reference sources. Let's assume its solubility is "z" mol/L.
The balanced equation for the dissociation of Ca(OH)2 is:
Ca(OH)2 (s) ⇌ Ca2+ (aq) + 2OH- (aq)
The Ksp expression for Ca(OH)2 is:
Ksp = [Ca2+][OH-]^2 = z(z)^2 = z^3
4. Ag2CrO4 (Silver chromate):
Similarly, let's assume the solubility of Ag2CrO4 is "w" mol/L.
The balanced equation for the dissociation of Ag2CrO4 is:
Ag2CrO4 (s) ⇌ 2Ag+ (aq) + CrO4^2- (aq)
The Ksp expression for Ag2CrO4 is:
Ksp = [Ag+]^2[CrO4^2-] = (2w)^2 * (w) = 4w^3
5. Cu2S (Copper(II) sulfide):
Let's assume the solubility of Cu2S is "v" mol/L.
The balanced equation for the dissociation of Cu2S is:
Cu2S (s) ⇌ 2Cu+ (aq) + S2- (aq)
The Ksp expression for Cu2S is:
Ksp = [Cu+]^2[S2-] = (v)^2 * (v) = v^3
Please note that these assumed solubilities are fictitious, and actual solubility values should be determined using appropriate experimental methods or reference sources. Using the given solubility values, you can compute the Ksp values for each compound.