What volume of 5% NaOH are required to neutralize 2 litre of decinormal H2SO4?
Answers
Answer:
Start with the easy part. How many mols of acid do you have? You’ll need that many moles of OH to neutralize it.
2 L x 0.1 mol/L = 0.200 moles of H2SO4 (I’m treating H2SO4 as a strong monoprotic acid)
Now we need the moles of OH-, but we’d need the molarity. So we need to convert from % to M.
For 5% solution, you’d have 5 g of NaOH per 100 g of solution.
That 5.00 g of NaOH is 0.125 moles of NaOH (converting 5.00 g x 1 mol / 40 g).
The 0.125 moles of NaOH would be contained in a volume of 0.100 L (assuming density is 1 g/ ml and converting the 100 g to 100 mL, and then 100 mL to 0.100 L)
The molarity of the NaOH would be 1.25 mol/L
We know we need 0.200 moles of OH. We have moles, and a concentration in mols/L, so we can find the requisite volume that contains that number of moles using the concentration.
0.200 mols x (1 L / 1.25 moles) = 0.160 L of 5% NaOH are needed.
Explanation:
I hope it's help you.
Answer:
what volume of five percent
