If it requires 38.5 milliliters of 0.85 molar nitric acid to neutralize 20.0 milliliters of barium hydroxide, solve for the molarity of barium hydroxide. show all of the work used to solve this problem. (4 points) unbalanced equation: ba(oh)2 + hno3 yields ba(no3)2 + h2o

M of Ba(OH)₂ = 0.818 M.

Explanation:

Ba(OH)₂ + 2HNO₃ → Ba(NO₃)₂ + 2H₂O,

It is clear that every 1.0 mol of Ba(OH)₂ needs 2 mol of HNO₃ to be neutralized completely.

∴ (nMV) of Ba(OH)₂ = (nMV) for HNO₃.

where, n is the no. of producible H⁺ or OH⁻ of the acid or base, respectively.

M is the molarity of the acid or base.

V is the volume of the acid or base.

For Ba(OH)₂:

n = 2, M = ??? M, V = 20.0 mL.

For HNO₃:

n = 1, M = 0.85 M, V = 38.5 mL.

∴ M of Ba(OH)₂ = (nMV) of HNO₃ / (MV) for Ba(OH)₂ = (1)(0.85 M)(38.5 L)/(2)(20.0 mL) = 0.818 M.