Which of the follow which of the following mixtures would result in a buffered solution? a. mixing 100.0 ml of 0.100 m hcl with 100.0 ml of 0.100 m naoh. b. mixing 100.0 ml of 0.100 m nh (k) = 1.8 x 10-5) with 100.0 ml of 0.100 m naoh. c. mixing 100.0 ml of 0.10 m hcl with 100.0 ml of 0.100 m nh3(k) = 1.8 x 10-5). d. mixing 50.0 ml of 0.100 m hcl with 100.0 ml of 0.100 m nh (kb = 1.8 x 10-5).

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1.75 is the weight of one medium egg

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.