Calculate the number fo moles of NaOH(aq) needed to react completely with 125 mL fo 6.00 M H2SO4(aq)
H2SO4 + 2NaOH ==> Na2SO4 + 2H2O
mols H2SO4 = M x L = ?
mols NaOH = twice that.
Well, it seems like we have a reaction on our hands! To calculate the number of moles of NaOH(aq) needed to react completely with the 6.00 M H2SO4(aq), we need to use the equation:
NaOH(aq) + H2SO4(aq) -> Na2SO4(aq) + H2O(l)
Now, let's start by finding the number of moles of H2SO4(aq) present in 125 mL of a 6.00 M solution. To do this, we'll use the formula:
moles = Molarity × Volume
So, moles of H2SO4 = 6.00 M × 0.125 L = 0.75 moles
Since the reaction between NaOH(aq) and H2SO4(aq) is in a 1:1 mole ratio, we need an equal number of moles of NaOH to react completely. Therefore, we'll need 0.75 moles of NaOH(aq) to react with the 0.75 moles of H2SO4(aq).
Remember, though, that calculations are serious business. While reactions can be full of surprises, when it comes to moles, we have to be precise. Hope this helps, and let the chemistry fun begin!
To calculate the number of moles of NaOH needed to react completely with 125 mL of 6.00 M H2SO4, we can use the stoichiometry of the balanced chemical equation.
The balanced chemical equation for the reaction between NaOH and H2SO4 is:
2 NaOH(aq) + H2SO4(aq) -> Na2SO4(aq) + 2 H2O(l)
From the balanced equation, we can see that 2 moles of NaOH react with 1 mole of H2SO4.
Given that the concentration of H2SO4 is 6.00 M, we can calculate the number of moles of H2SO4 using the equation:
moles of H2SO4 = concentration of H2SO4 * volume of H2SO4
= 6.00 mol/L * 0.125 L
= 0.75 moles
Since the ratio of NaOH to H2SO4 is 2:1, the number of moles of NaOH needed will be half of the moles of H2SO4:
moles of NaOH = 0.75 moles / 2
= 0.375 moles
Therefore, 0.375 moles of NaOH(aq) are needed to react completely with 125 mL of 6.00 M H2SO4(aq).
To calculate the number of moles of NaOH(aq) needed to react completely with 125 mL of 6.00 M H2SO4(aq), you will need to use the balanced chemical equation and the molarity (M) of H2SO4.
The balanced chemical equation for the reaction between NaOH and H2SO4 is as follows:
2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(l)
From the equation, you can see that 2 moles of NaOH react with 1 mole of H2SO4.
First, calculate the number of moles of H2SO4 using the given molarity and volume:
moles of H2SO4 = molarity × volume
= 6.00 M × 0.125 L
= 0.75 moles
According to the balanced equation, 2 moles of NaOH react with 1 mole of H2SO4. Therefore, the number of moles of NaOH needed can be calculated using the ratio:
moles of NaOH = 2 × moles of H2SO4
= 2 × 0.75 moles
= 1.5 moles
So, 1.5 moles of NaOH(aq) are needed to react completely with 125 mL of 6.00 M H2SO4(aq).