00:01
To calculate the molar solubility, we recognize that barium fluoride as a solid is going to dissociate in water into one barium ion and two fluoride ions according to its ksp.
00:19
Ksp will be equal to the concentration of barium multiplied by the concentration of fluoride squared because of its two coefficients.
00:29
And they tell us that value is 1 .7 times 10 to the negative 6.
00:37
Molar solubility is the moles of solid that dissolve in a liter of solution.
00:42
So when one mole of the solid dissolves in a liter, we get one mole of barium ion in a liter.
00:48
So we can state the molar solubility is equal to the barium concentration.
00:52
But because we get twice as much fluoride, then the fluoride concentration is going to be equal to two times molar solubility.
01:02
Plugging these back into the ksp expression, we can solve for molar solubility.
01:09
1 .7 times 10 to the negative 6 equals the barium concentration, which is molar solubility, multiplied by the fluoride concentration, 2s squared...