The solubility of sodium floride, NaF, is 4.06 g NaF/100 g H2O at 20ºC. What mass of NaF would you have to dissolve in 1000 g H2O to make a saturated solution?
4.06 g x (1000/100) = ??
Wouldn't you expect to dissolve 10 times more NaF in 10 x more water?
To find out the mass of NaF required to make a saturated solution, we can use the given solubility of sodium fluoride.
The solubility of sodium fluoride (NaF) is given as 4.06 g NaF/100 g H2O at 20ºC. This means that in 100 grams of water, 4.06 grams of NaF can dissolve to form a saturated solution.
To calculate the mass of NaF required to make a saturated solution in 1000 grams of water, we can set up a proportion:
(4.06 g NaF) / (100 g H2O) = (x g NaF) / (1000 g H2O)
Cross-multiplying, we get:
1000 g H2O * 4.06 g NaF = 100 g H2O * x g NaF
4060 g NaF = 100 g H2O * x g NaF
Dividing both sides of the equation by 100 g H2O, we have:
x g NaF = (4060 g NaF) / (100 g H2O)
Calculating this expression, we get:
x g NaF = 40.6 g NaF
Therefore, to make a saturated solution in 1000 grams of water, you would have to dissolve 40.6 grams of NaF.
To find the mass of NaF required to make a saturated solution in 1000 g of water, we need to use the solubility information provided.
The given solubility of NaF is 4.06 g NaF per 100 g H2O. This means that 100 g of water can dissolve 4.06 g of NaF at 20ºC.
To determine the mass of NaF required to make a saturated solution in 1000 g of water, we can set up a proportion using the solubility information:
4.06 g NaF / 100 g H2O = x g NaF / 1000 g H2O
Now, we can solve for x (mass of NaF):
x = (4.06 g NaF / 100 g H2O) * 1000 g H2O
x = 40.6 g NaF
Therefore, you would need to dissolve 40.6 grams of NaF in 1000 grams of water to make a saturated solution.