How many moles of H2SO4 are required to react with 50 mL of NaOH solution? NaOH is 1M.
2NaOH + H2SO4 ==> Na2SO4 + 2H2O
How many mols H2SO4 do you have? That's mols H2SO4 = M x L = 1M x 0.050L = ?
From the equation you know that 2 mols NaOH are needed for 1 mol H2SO4; therefore, 2*0.050 = mols NaOH needed.
To determine the number of moles of H2SO4 required to react with 50 mL of NaOH solution, you need to first calculate the number of moles of NaOH in the given volume and concentration, and then use the balanced chemical equation to determine the mole ratio between H2SO4 and NaOH.
Step 1: Calculate the number of moles of NaOH
Given that the NaOH solution has a concentration of 1M and a volume of 50 mL, you can use the formula:
Moles = Concentration (mol/L) * Volume (L)
Converting 50 mL to L:
Volume (L) = 50 mL / 1000 = 0.050 L
Moles of NaOH = 1M * 0.050 L = 0.050 moles
Step 2: Determine the mole ratio
The balanced chemical equation for the reaction between H2SO4 and NaOH is:
H2SO4 + 2NaOH -> Na2SO4 + 2H2O
From the balanced equation, you can see that 1 mole of H2SO4 reacts with 2 moles of NaOH. Therefore, the mole ratio of H2SO4 to NaOH is 1:2.
Step 3: Calculate the moles of H2SO4
Since the mole ratio is 1:2, the number of moles of H2SO4 will be half of the moles of NaOH:
Moles of H2SO4 = 0.050 moles / 2 = 0.025 moles
Therefore, 0.025 moles of H2SO4 are required to react with 50 mL of 1M NaOH solution.