How Does Ksp Change With Temperature?

Does this affect the Ksp value of the Ca(OH)2?

Does adding boiled, deionized water to a titrating flask to wash the wall of the Erlenmeyer flask and the buret tip affect the Ksp value of the Ca(OH)2 inside? Why?

Ksp is temperature dependant. If you look at the list of Ksp values you should always see a note specifying that these values are determined at 25°C.
If you increase the temperature of the solvent water, as indicated by you, the Ksp value of the Ca(OH)2 will change - briefly because the compound is more soluble in hot water than in cold water.

What is the only thing that will change a Ksp?

And how could you increase the Ksp?

any change in temperature will change the Ksp value.
for every temperature, there is a different Ksp value.

How do i find the Ksp value?

The solubility of Cd(OH)2 in water at a certain temperature is 1.5 x 10^-5 mol/L. The Ksp value for Cd(OH)2 is what? The Ksp solubility product constant for Cd(OH)2 is 7.2 x 10^-15 The answer is 1.4 x 10^-14-How do I get there?

well the Ksp will be

Cd(OH)2 ------- Cd+2 + 2 OH^-1

so solid Cd (OH)2 will weakly dissolve ( an amount X ) to yield a solubility of 1.5 X 10^-5 M as given above so the x value is 1.5 X 10^-5 and that amount of Cd(OH)2 dissolving will give 1.5 X 10^-5 M Cd+2 and 3 X 10^-5 M OH plugging the values into the equation for the Ksp
Ksp = [Cd+2][OH^-1]^2 = (1.5 X 10^-5 ) ( 3 X 10^-5 )^2 =
1.5 x 9 x 10^-15 = 13.5 X 10^-15 = 1.35 x 10^-14 = 1.4 x10^-14

Chem Help: Ksp values?

If you were given a saturated solution of PbI2, and you want to find the Ksp. How would you proceed... do i start with finding the temperature, and then find concentration of the ions? so then i can say that at that temperature, the Ksp is....

Calculating the numerical value of Ksp involves several steps. The basic steps are:

write the equilibrium expression

write the ksp expression

calculate the molar concentration of the ions in solutions

substitute these concentrations into the Ksp.

though references rarely agree on Ksp's, your answers are cose to ...

Ksp value for Cu3(PO4)2
Ksp = 1.40×10-37 ....
from :

Ksp = 1.93 x 10¯37 ... from :

Ksp for Mg3(PO4)2 :
Ksp of Mg3(PO4)2 is 1 x 10-25

Ksp = 1 x 10^-25.


K2SO4 and KCl are extremely soluble

Hope that helps, Goodluck

calculating ksp question?

The solubility of sliver bromide at 100c is 0.00037 grams for 100 grams of water. Calculate Ksp for silver bromide at this temperature.

Ksp = [Ag+]*[Br-]

Molar mass AgBr = 107.87 + 79.904 = 187.774
0.00037g = 0.00037/187.774 = 1.97*10^-6 mol dissolved in 0.1 litre.
MolarityAgBr = 1.97*10^-6/0.1 = 1.97*10^-5M = [Ag+]
[Ag+] =[Br-]
Ksp = [Ag+]²
Ksp = (1.97*10^-5)²
Ksp = 3.88*10^-10

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