Asked by Anonymous
The molarity of an aqueous solution of barium hydroxide is determined by titration against a 0.335 M nitric acid solution.
If 32.8 mL of the base are required to neutralize 21.5 mL of nitric acid, what is the molarity of the barium hydroxide solution?
If 32.8 mL of the base are required to neutralize 21.5 mL of nitric acid, what is the molarity of the barium hydroxide solution?
Answers
Answered by
DrBob222
Ba(OH)2 + 2HNO3 ==> Ba(NO3)2 + 2H2O
mols HNO3 = M x L = ?
mols Ba(OH)2 = 1/2 that from the coefficients in the balanced equation.
Then M Ba(OH)2 = mols Ba(OH)2/L Ba(OH)2. YOu know mols and L, solve for M.
mols HNO3 = M x L = ?
mols Ba(OH)2 = 1/2 that from the coefficients in the balanced equation.
Then M Ba(OH)2 = mols Ba(OH)2/L Ba(OH)2. YOu know mols and L, solve for M.
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