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.

Unbalanced equation: Ba(OH)2 + HNO3 Ba(NO3)2 + H2O
( I already balanced the equation)

Question

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.

Unbalanced equation: Ba(OH)2 + HNO3  Ba(NO3)2 + H2O
( I already balanced the equation)

jfraser · Answer

the reaction's not balanced

anonymous · Answer

Ba(OH)2 + 2 HNO3 = Ba(NO3)2 + 2 H2O

anonymous · Answer

we are given
Ba(OH)2: Vol = 0.02 (have to write in litres), M (conc.) = y (what we're finding out)

HNO3: Vol. = 0.0385, M = 0.85

n (moles) = MxV
n(HNO3) = 0.85 x 0.0385 = 0.032725

The mole ratio is 2 : 1 
since HNO3 has one H+ and Ba(OH)2 has two OH-

Therefore n(Ba(OH)2) = 0.032725 / 2 = 0.0163625

M = n / v
therefore y = 0.0163625 / 0.020 = 0.818125

roughly = 0.82M :) any doubt??

anonymous · Answer

Thankk you so much

anonymous · Answer

yw but its a humbly request frnd plz dont post qn on math sec as i really dont belong to this subject so it just screw wen i see this sec :P

anonymous · Answer

OHhh I see sorry! I still thought I was in chemistry. it must have took me here