Consider a salt of the composition, A2B3. For this salt, pKsp=82.55. What is the logarithm of the molar concentrtion of this salt?
I'm really at a loss of where to begin. We didn't have any examples like this in class. Thanks!
You just need to get started.
A2B3 ==> 2A^+3 + 3B^-2
If pKsp = 82.55, then take the antilog of both sides which is
antilog pKsp = antilog 82.55
Ksp = 3.548 x 10^82
(Do you know how to do that. Punch in 82.55 on your calculator, then hit the 10^x key and that will give you the antilog 82.55 which is 3.548 x 10^82.)
I suspect you can take it from here. If not, tell us what you don't understand and show your work to the point at which you don't know what to do next.
Ksp = (A)^2(B)^3 = 3.548 x 10^82.
Then set and solve for (A2B3).
step 1:[2A^+3][3B^-2]/[A2B3]=82.55=Ksp
step 2:total concentration of the top part is [3.548E82]/x=82.55
step 3:[3.548E82]x 82.55=x
step 4: x=2.92E84
Can you please check this if am correct and am in the right path...am just not good with this chemisty stuff...forgive my incorrect assumpions if any.
I wouldn't do it that way.
A2B3 ==> 2A^+2 + 3B^-3
Ksp = (A)^2(B)^3
Let X = (A2B3) which is what you want to solve for.
If X = (A2B3), then (A^+2) = 2X and (b^-3) = 3X. Now substitute that into the Ksp expression.
Ksp = (2X)^2((3X)^3 = 3.548E82
Now solve for X which is the molar concentration of (A2B3).
Then the problem asks you to take the log of that
Assuming the final concentration of chloride anion after the addition of HCl (precipitation step) was 0.1M, what is the remaining concentration of Ag+ in the solution? (pKsp for AgCl = 9.74)
To find the logarithm of the molar concentration of the salt A2B3, we need to know the value of the molar concentration itself. Unfortunately, the given information does not directly provide the molar concentration of the salt. However, we can use the concept of the solubility product constant (Ksp) to calculate the molar concentration indirectly.
The solubility product constant (Ksp) is a measure of the maximum extent to which a compound can dissolve in water. It is defined as the product of the molar concentrations of the ions involved in the equilibrium expression for the dissolution of the compound.
For the salt A2B3, the dissolution equation can be written as:
A2B3(s) ⇌ 2A+(aq) + 3B-(aq)
The corresponding equilibrium expression is:
Ksp = [A+]^2 [B-]^3
Given that the value of pKsp is 82.55, we can convert it to Ksp using the following formula:
Ksp = 10^(-pKsp)
Substituting the given value:
Ksp = 10^(-82.55)
Now, since we are looking for the logarithm of the molar concentration, we can rewrite the equilibrium expression as:
log[Ksp] = log([A+]^2 [B-]^3)
Using the properties of logarithms, we can rewrite the equation as:
log[Ksp] = 2log[A+] + 3log[B-]
Now, let's assume that the molar concentration of A+ is [A+], and the molar concentration of B- is [B-]. We can substitute these values into the equation:
log[Ksp] = 2log[A+] + 3log[B-]
Therefore, the logarithm of the molar concentration of the salt A2B3 can be calculated using the solubility product constant and the above equation. You can substitute the calculated value of Ksp into the equation and determine the logarithm of the molar concentration.