What mass of manganese(ii) chloride must react with sulfuric acid to release 52.5 ml of hydrogen chloride gas at stp?
mncl2(s)+h2so4(aq)→mnso4(aq)+2hcl(g )

The balanced chemical reaction is written as:

MnCl2(s)+H2SO4(aq)→MnSO4(aq)+2HCl(g)

We are given the amount of hydrochloric acid to be produced in the reaction. This value will be the starting point for the calculations.We do as follows:

.0525 L HCl ( 1 mol / 22.4 L ) ( 1 mol MnCl2 / 2 mol HCl ) (125.84 g / 1 mol ) = 0.15 g MnCl2

Butterfly wingspan is 7.7

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.