Inaninsulatedcalorimeter,100.0gof1. 00MHN03ismixedwith100.0gof1.00MKOH. The temp went from 22.1° C to 28.6° C. Calculate the heat of reaction. C for water is 4.184 J/g °C and C for the calorimeter is 18.80 J/ °C a) -27.8 kJ/mol b) -55.6 kJ/mol c) 55.6 kJ/mol d) 54.4 kJ/mol

Compound with sulfer  is bright red 

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.

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