3. Write a balanced equation for the reaction between Ca(OH)2 and HNO3. Use this equation to answer problems a-c. a) If it takes 50.0 mL of 0.5 M Ca(OH)2 solution to completely neutralize 125 mL of HNO3solution, what is the concentration of the HNO3 solution?
b) How many mL of 0.50 M HNO3 is necessary to titrate 25.0 mL of 0.05 M Ca(OH)2 solution to the endpoint?
c) If it takes 75.0 mL of 1.5 M HNO3 solution to completely neutralize 125 mL of Ca(OH)2what is the concentration of the Ca(OH)2 solution?

C) the increase in atmospheric pressure pushes the walls of the balloon outward thus making it  is the answer.hope i you.

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.