How many milliliters of 0.125 M H2SO4 are needed to neutralize 0.230g of NaOH ?
I've tried it a couple of times but I can't get the right answer and my final is tomorrow!
Thank you! (:
I've tried it a couple of times but I can't get the right answer and my final is tomorrow!
Thank you! (:
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Calculate moles of NaOH. Then it will take 1/2 that many moles of H2SO4 since
H2SO4 + 2NaOH ===> 2NaSO4 + 2H2O
moles of NaOH = 0.230 g x 1 mol/40 g = 0.00575 moles of NaOH
Therefore you need 0.00575 moles/2 moles H2SO4 = 0.002875
(xL)(0.125 moles/L) = 0.002875 moles
x = 0.023 liters = 23 mls
H2SO4 + 2NaOH ===> 2NaSO4 + 2H2O
moles of NaOH = 0.230 g x 1 mol/40 g = 0.00575 moles of NaOH
Therefore you need 0.00575 moles/2 moles H2SO4 = 0.002875
(xL)(0.125 moles/L) = 0.002875 moles
x = 0.023 liters = 23 mls
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Equation:
H2SO4 + 2NaOH → Na2SO4 + 2H2O
1mol H2SO4 reacts with 2 mol NaOH
Molar mass NaOH = 40.0g/mol
0.230g NaOH = 0.230/40 = 5.75*10^-3 moles NaOH
From the equation , this will react with (5.75*10^-3)/2 = 2.875*10^-3 mol H2SO4
1000mL H2SO4 solution contains 0.125 mol H2SO4
Volume that contains 2.875*10^-3 mol H2SO4 = 1000/0.125* (2.875*10^-3) = 23 mL
Answer: 23mL H2SO4 solution required.
H2SO4 + 2NaOH → Na2SO4 + 2H2O
1mol H2SO4 reacts with 2 mol NaOH
Molar mass NaOH = 40.0g/mol
0.230g NaOH = 0.230/40 = 5.75*10^-3 moles NaOH
From the equation , this will react with (5.75*10^-3)/2 = 2.875*10^-3 mol H2SO4
1000mL H2SO4 solution contains 0.125 mol H2SO4
Volume that contains 2.875*10^-3 mol H2SO4 = 1000/0.125* (2.875*10^-3) = 23 mL
Answer: 23mL H2SO4 solution required.