I seriously don't understand this...i cant even begin to think of what to do please help...
How many moles of Ba(OH)2 does it take to neutralize 2.5 moles of HNO3?
First you write the equation, then balance it.
Ba(OH)2(aq) + 2HNO3(aq) ==> Ba(NO3)2)aq) + 2H2O(l)
Next you use the coefficients in the balanced equation (that's why you write and balance the equation FIRST) to convert mols HNO3 to mols Ba(OH)2.
2.5 mol HNO3 x [1 mol Ba(OH)2/2 mol HNO3] = 2.5 x (1/2) = ? mols Ba(OH)2
To determine the number of moles of Ba(OH)2 needed to neutralize 2.5 moles of HNO3, we need to use the balanced chemical equation for the reaction between Ba(OH)2 and HNO3.
The balanced 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.
To find the number of moles of Ba(OH)2, we can set up a ratio using the information from the balanced equation.
Given:
- Moles of HNO3 = 2.5 moles
Using the ratio: 2 moles HNO3 : 1 mole Ba(OH)2
Moles of Ba(OH)2 = (2.5 moles HNO3) * (1 mole Ba(OH)2 / 2 moles HNO3)
Moles of Ba(OH)2 = 1.25 moles
Therefore, it takes 1.25 moles of Ba(OH)2 to neutralize 2.5 moles of HNO3.