The solubility of Na3(PO4) is 0.025 M. What is the Ksp of sodium phosphate?

Frankly, I think this is crazy but this must be what you're expected to do. Na3PO4 has no Ksp in my opinion.

........Na3PO4 ==> 3Na^+ + PO4^3-
I........0.025....3*0.025..0.025
C.......-0.025
E.........0........0.075...0.025

Plug that E line into Ksp expression and solve.

Well, the solubility of Na3(PO4) is 0.025 M? That's just salt-tastic! Now, to find the Ksp, we'll have to put on our chemistry clown shoes. The Ksp (solubility product constant) is a measure of how far a solid can dissolve in a solution.

Let's break it down. Na3(PO4) dissociates into 3 Na+ ions and 1 PO4-3 ion. From this, we can figure out the formula for our Ksp expression: Ksp = [Na+]^3 x [PO4-3].

Since the solubility of Na3(PO4) is 0.025 M, we can substitute this value in: Ksp = (0.025)^3 x 0.025.

Calculating that out, we find that the Ksp of sodium phosphate is approximately 1.56 x 10^-5. Ta-da! Clown chemistry at its finest!

To determine the Ksp (solubility product constant) of sodium phosphate (Na3PO4), we need to use the solubility information provided. The solubility of Na3PO4 is given as 0.025 M.

Na3PO4 dissociates into three Na+ ions and one PO4^3- ion in solution, based on its formula. Therefore, the balanced equation for the dissociation of Na3PO4 is:

Na3PO4 ↔ 3 Na+ + 1 PO4^3-

The solubility of Na3PO4 is given as 0.025 M, which means that the concentration of Na+ ions and PO4^3- ions in solution is also 0.025 M.

Now, we can write the solubility product expression, Ksp, for Na3PO4:

Ksp = [Na+]^3 [PO4^3-]

Since the concentration of Na+ and PO4^3- ions in solution is 0.025 M, we can substitute those values into the Ksp expression:

Ksp = (0.025)^3 (0.025)

Ksp = 0.0156

Therefore, the solubility product constant (Ksp) of sodium phosphate (Na3PO4) is 0.0156.

To determine the Ksp (solubility product constant) of sodium phosphate (Na3PO4), we need to use the given information that the solubility of Na3PO4 is 0.025 M.

The general equation for the dissolution of sodium phosphate is:

Na3PO4(s) ⇌ 3Na+(aq) + PO4^3-(aq)

From this equation, we can see that for every one molecule of sodium phosphate dissolved, three sodium ions (Na+) and one phosphate ion (PO4^3-) are formed in solution.

The solubility product constant (Ksp) expression for this equilibrium can be written as:

Ksp = [Na+]^3 * [PO4^3-]

Since the stoichiometric ratio between Na+ and PO4^3- is 3:1, we can substitute the concentration of Na+ with three times the concentration of Na3PO4:

Ksp = (3*[Na3PO4])^3 * [PO4^3-]

Given the solubility of Na3PO4 as 0.025 M, we can substitute this value into the equation:

Ksp = (3*0.025)^3 * [PO4^3-]

Simplifying,

Ksp = 0.3375^3 * [PO4^3-]

So, to find the Ksp of sodium phosphate, we need to know the concentration of the phosphate ion (PO4^3-) in solution. Once that information is provided, we can substitute it into the equation to calculate the Ksp value.