NaOH+H2SO4-> H2o+Na2SO4?
How many moles of NaOH required to neutralize 1 mole H2SO4?
1. Balance the equation.
2. mols NaOH = M x L = ?
3. Convert mols NaOH to mols H2SO4.
4. M H2SO4 = moles H2SO4/L H2SO4.
5. 2 moles
I believe, NOT COMPLETLY SURE???
Write and balance the equation. Then look at the coefficients.
2NaOH + H2SO4 = Na2SO4 + 2H2O
It takes 2 mols NaOH to = 1 mol H2SO4.
To determine the number of moles of NaOH required to neutralize 1 mole of H2SO4, we can use the balanced chemical equation.
The balanced equation for the reaction between NaOH and H2SO4 is:
2 NaOH + H2SO4 -> 2 H2O + Na2SO4
From the balanced equation, we can see that the stoichiometric ratio between NaOH and H2SO4 is 2:1. This means that for every 2 moles of NaOH, 1 mole of H2SO4 is neutralized.
Therefore, to neutralize 1 mole of H2SO4, we would need half the amount of the stoichiometric ratio, which is 1/2 of 2 moles of NaOH.
So, 1 mole of H2SO4 would require 1/2 mole of NaOH.
To determine the number of moles of NaOH required to neutralize 1 mole of H2SO4, we need to consider the balanced chemical equation:
NaOH + H2SO4 → H2O + Na2SO4
The balanced equation tells us that one mole of H2SO4 reacts with two moles of NaOH. In other words, the stoichiometric ratio of NaOH to H2SO4 is 2:1.
So, for every 1 mole of H2SO4, we need 2 moles of NaOH to completely neutralize it.