A 0.250 g sample of a magnesium-alumnium alloy dissolves completely in an excess of HCL(aq). When the liberated H2(g) is collected over water at 29 deg C and 752 torr, the volume is found to be 307 mL. The vapor pressure of water at 29 deg C is 30.0 torr. How many moles of H2 can be produces from x grams of Mg in Magnesium-aluminum alloy? The molar mass of Mg is 24.31 g/mol. Express your answer in terms of x to four decimal places. Thanks for your help in advance!

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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.