A concentrated solution of nitric acid (HNO3) with a concentration of 2.0 M is used to neutralize a 17.1 g sample of barium hydroxide (molar mass is 171 g/mol). The unbalanced equation representing this reaction is below.

HNO3 + Ba(OH)2 á Ba(NO3)2 + H2O

What volume of nitric acid was used to react completely with the sample of barium hydroxide?

Ithink the answer is a or d.

Show and image of the mixtures or write them

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.