ANSWER ALL OF THEM PLEASE! :) 1) How many grams in total are in 0.5689 mol of sulfuric acid?
2) How many moles are equal to 1410 g of magnesium oxide?
3) Calculate the number of grams contained in 1.6 mol of calcium
carbonate.
4) How many mol is equal to 500.75 g of iron(II) fluoride?
5) What is the GFM of sodium phosphide?
6) What is the molar mass of sodium phosphate?
7) How many grams are in a mole of sodium phosphite?
8) Calculate the number of moles of 700.0 g of oxygen gas.
9) Convert 2.33 moles of carbon dioxide to g of carbon dioxide.
10) Convert 250 grams of water to moles.

Your question is not clear but if you can explain yourself i would be glad to .  just trying to : ))

Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.