If the concentration of a saturated solution of SrCO3 is 0.000040 mol*L^-1, what is the value for the solubility product constant of this salt.
How do I start this please
SrCO3 ==> Sr^+2 + CO3^=
write the Ksp expression.
Substitute 4.0 x 10^-5 M. Solve for Ksp.
Ksp = 4.0E-5 = (x)(3x)
is the (3x) squared ??
I think you are having a tough time understanding the concept of solubility product. Perhaps you need to read some more in your text/notes.
SrCO3 ==> Sr^+2 + CO3^=
Ksp = (Sr^+2)(CO3^=) = ??
Solubility from the problem of SrCO3 = 4 x 10^-5 M and since 1 mol SrCO3 gives 1 mol Sr^+2 and 1 mol SO4^=, then those ions = 4 x 10^-5 M also. So
(Sr^+2) = 4 x 10^-5 M
(CO3^=) = 4 x 10^-5 M
Ksp = (4 x 10^-5)(4 x 10^-5) = ??
I have no idea where you obtained x and 3x OR why you asked the question about cubing something. There is nothing to cube BECAUSE there is no coefficient of 3 anywhere in the equation.
where i am pulling this is if you pull up google and type in molar solubility the first website shows you how to do it... that is what i am following and it shows me that in the book too
If you want to type in the web address I will look at it but I know what Ksp is. I'm sure those sites, and your text, are correct. I'm also relatively sure that you are misinterpreting it. Let me cite the solubility product principle to(for) you.
The product of the molar solubility of the ions of a slightly soluble material, each ion raised to a power indicated by its coefficient in the dissociation reaction, is equal to a constant, called solubility product constant, at a constant temperature.
Here is a site on SrCO3^= that I found. (Broken Link Removed)
well i do understand what you did to solve the problem... and i did find the answer... its just that all this stuff im looking at is sqrt everything that's all and i didn't see you do that
When you are looking for the solubility when Ksp is given, square roots and cube roots (sometimes fourth and fifth roots) are the order of the day. But when we are given the solubility, as in SrCO3, then we simply multiply (4x10^-5)(4x10^-5) and its just the multiplication of those two numbers or I could have written it as
(4.0 x 10^-5)^2 = ??
that makes better sense now
thank you
To start solving this problem, it is important to understand the concept of solubility product constant (Ksp). The Ksp represents the equilibrium constant for the dissolution of a sparingly soluble salt in water. It is determined by the concentrations of the ions present in the saturated solution.
For the given problem, we are dealing with SrCO3, which dissociates as follows:
SrCO3(s) ⇌ Sr2+(aq) + CO32-(aq)
The molar solubility of SrCO3 represents the concentration of Sr2+ and CO32- ions in a saturated solution. We will need this value to calculate the Ksp.
Given:
Concentration of a saturated solution of SrCO3 = 0.000040 mol/L
Since SrCO3 dissociates into one Sr2+ ion and one CO32- ion, the molar solubility of the salt is equal to the concentration of both ions in the solution.
Therefore, the molar solubility of SrCO3 = 0.000040 mol/L
The Ksp expression for SrCO3 is:
Ksp = [Sr2+][CO32-]
To find the value of Ksp, we substitute the molar solubility of SrCO3 as the concentration of both ions in the Ksp expression.
Ksp = (0.000040 mol/L) * (0.000040 mol/L)
Simplifying, we multiply the two concentrations together:
Ksp = 0.000040 * 0.000040 = 0.0000000016
Therefore, the value for the solubility product constant (Ksp) of SrCO3 is 0.0000000016.