Question

2 hno 3 (aq) ba(oh) 2 (aq) 2 h 2 o(l) ba(no 3 ) 2 (aq) a 0.110 l sample of an unknown hn*o_{2} solution required 40.5 of 0.200 m ba(oh) 2 for complete neutralization what is the concentration of the hn*o_{5} solution?

Answer 1

To find the concentration of the unknown HNO3 solution after titration with Ba(OH)2, the number of moles of Ba(OH)2 used in the reaction (0.0081 moles) is determined and doubled due to the stoichiometry of the reaction (0.0162 moles). The concentration of the HNO3 solution is then calculated by dividing the moles of acid by the volume of the solution (0.147 M).

Step-by-step explanation:

The question involves calculating the concentration of an unknown HNO3 (nitric acid) solution using a titration method with Ba(OH)2 (barium hydroxide) as the titrant. The balanced chemical equation for the reaction is:

2 HNO3 (aq) + Ba(OH)2 (aq) → 2 H2O (l) + Ba(NO3)2 (aq)

First, we calculate the number of moles of Ba(OH)2 used:

moles Ba(OH)2 = Molarity × Volume = 0.200 M × 0.0405 L = 0.0081 moles

According to the balanced equation, 2 moles of HNO3 react with 1 mole of Ba(OH)2, therefore:

moles HNO3 = 2 × moles Ba(OH)2 = 2 × 0.0081 moles = 0.0162 moles

Now, we find the concentration of the HNO3 solution:

Concentration of HNO3 = moles HNO3 / Volume of solution = 0.0162 moles / 0.110 L = 0.147 M HNO3