What mass of NaCl should be found in 0.51 L of a saturated solution of sodium chloride if the Ksp of NaCl is assumed to be 1.5 x 10-5?
The problem with this problem is that NaCl does not have a Ksp; therefore, I don't know the meaning of a Ksp for NaCl of 1.5 x 10^-5.
sorry Ksp of PbCl2 is 1.6 x 10-5
PbCl2 ==> Pb^+2 + 2Cl^-
Ksp = (Pb)(Cl^-)^2 = 1.5 x 10^-5
If we let y = solubility of PbCl2, then y = (Pb^+2) and 2y = (Cl^-).
Substitute y and 2y in the Ksp expression, solve for y and that will be the solubility of PbCl2 in mols/L. Multiplying by molar mass will give you the grams/L and multiplying that by 0.51/1 will give you the grams in 0.51 L.
To determine the mass of NaCl in a saturated solution, we need to use the solubility product constant (Ksp) of NaCl.
Step 1: Write the balanced equation for the dissociation of NaCl.
NaCl ⇌ Na+ + Cl-
Step 2: Construct the expression for the solubility product constant (Ksp).
Ksp = [Na+][Cl-]
Since NaCl fully dissociates into Na+ and Cl- ions, the concentration of Na+ and Cl- in the saturated solution will be the same. Let's assume x is the molar solubility of NaCl, which represents the concentration of Na+ and Cl- ions in the solution.
Ksp = x * x = x^2
Step 3: Calculate the molar solubility (x) of NaCl using the given Ksp value.
x^2 = 1.5 x 10^(-5)
x = √(1.5 x 10^(-5))
x ≈ 1.22 x 10^(-2) M
Step 4: Determine the moles of NaCl per liter of the saturated solution.
The molar solubility of NaCl (x) is approximately 1.22 x 10^(-2) M, which means there are 1.22 x 10^(-2) moles of NaCl per liter of the saturated solution.
Step 5: Calculate the mass of NaCl in 0.51 L of the saturated solution.
Mass = moles * molar mass
The molar mass of NaCl is approximately 58.44 g/mol.
Mass = 1.22 x 10^(-2) moles * 58.44 g/mol
Mass ≈ 0.71 g
Therefore, the mass of NaCl in 0.51 L of the saturated solution is approximately 0.71 grams.