How many moles of HNO3 are present if 0.116mol of Ba(OH)2 was needed to neutralize the acid solution?
To determine the number of moles of HNO3 present, we need to use the balanced chemical equation for the reaction between HNO3 and Ba(OH)2.
The balanced chemical equation is:
2 HNO3 + Ba(OH)2 -> Ba(NO3)2 + 2 H2O
From the equation, we can see that 2 moles of HNO3 react with 1 mole of Ba(OH)2. This means that the stoichiometric ratio is 2:1 between HNO3 and Ba(OH)2.
Given that 0.116 mol of Ba(OH)2 was needed to neutralize the acid solution, we can use this information to calculate the number of moles of HNO3.
Since the stoichiometric ratio is 2:1 between HNO3 and Ba(OH)2, the number of moles of HNO3 will be half of the moles of Ba(OH)2 used. Therefore, we can calculate it as follows:
Number of moles of HNO3 = 0.116 mol / 2
Number of moles of HNO3 = 0.058 mol
So, there are 0.058 moles of HNO3 present in the acid solution.
2HNO3 + Ba(OH)2 ==> Ba(NO3)2 + 2H2O
Look at the coefficients in the balanced equation. mols HNO3 = 2 x mols Ba(OH)2