The products will be magnesium phosphate and potassium chloride. You then have to watch a solubility chart to see which one of these is not soluable. In this case it is magnesium phosphate.
I think its density is 850kg/m^3
Answer:
it is false
Explanation:
it goes in different ways not in order
Answer:
for given question is 2.79 and
is 0.52
{i- vant hoff’s constant ; Kb- constant ; m molarity }
M = no. of moles of the solute present in one kg of solution
Let the weight of amount of solute be “w” and its molecular mass be “M”
Let the mass of the solvent in the given question be “x”




a) PbCrO4:
according to the equation:
PbCrO4(s) → Pb2+(aq) + CrO42-(aq)
so, Ksp = [Pb2+][CrO42-]
by assuming [Pb2+] = [CrO42-] = X
and when S (the solubility) = 4 x 10^-5 g/L
we have first to convert solubility from g/L to mol/L by getting the molar mass of the salt
solubility mol/L = solubility g/L / molar mass of salt
= 4 x 10^-5g/L / 323.2 g/mol
= 1.24 x 10^-7 mol / L
by substitution in Ksp formula:
∴Ksp = X* X
= (1.24 x 10^-7)^2
= 1.54 x 10^-14
b) BaC2O4:
according to this equation:
BaC2O4(s)→ Ba 2+(aq) + C2O4 2- (aq)
So Ksp = [Ba2+][C2O42-]
Assume that [Ba2+] = [C2O42-] = X
when the solubility S = 0.29 g/L = X , so we need to convert S from g/L to
mol / L
solubility mol / L= solubility g/L / molar mass of salt
= 0.29 g/L / 225.34 g/mol
= 0.0013 mol/L
by substitution in ksp formula:
∴Ksp = X^2
= (0.0013)^2
= 1.69 x 10^-6
C) MnCO3:
according to this equation :
MnCO3(s)→ Mn2+(aq) + CO3 2-(aq)
so, Ksp = [Mn2+][CO32-]
assume [Mn2+] = [CO32-] = X
when the solubility s = 4.2 x 10^-6 g/L so we need to convert S from g/L to mol/L by dividing on molar mass.
the solubility mol/L = solubility g/L / molar mass g/mol
=.4.2 x 10^-6 /114.9
= 3.7 x 10^-8 mol/L
by substitution on ksp formula:
∴ Ksp = X*X
= (3.7 x 10^-8)^2
= 1.369 x 10^-15