Asked by Xisca
The pH of a sample of base is 12.7. The amount of crystalline oxalic acid required to react with 2 l of this solution is-
Answers
Answered by
DrBob222
Is this a multiple choice question? What are the choices. It's done this way. You don't say what the base is but I will assume it is a strong base; therefore,
pH = - log (H^+)
12.7 = -log(H^+)
(H^+) = 2E-13. Then
(OH^-) = Kw/(H^+) = 1E-14/2E-13 = 0.05 molar base.
How many moles do you have in 2 L? That's mols = M x L = 0.05 x 2 = 0.1
Oxalic acid = H2Ox
...........H2Ox + 2OH^- ==> 2H2O + Ox^2-
........Y mols...+ 0.1 mol...............................
Therefore, mols H2Ox needed = 0.05 mol
mols H2Ox = grams H2Ox/molar mass. You know molar mass and mols, solve for grams H2Ox.
Post your work if you get stuck.
pH = - log (H^+)
12.7 = -log(H^+)
(H^+) = 2E-13. Then
(OH^-) = Kw/(H^+) = 1E-14/2E-13 = 0.05 molar base.
How many moles do you have in 2 L? That's mols = M x L = 0.05 x 2 = 0.1
Oxalic acid = H2Ox
...........H2Ox + 2OH^- ==> 2H2O + Ox^2-
........Y mols...+ 0.1 mol...............................
Therefore, mols H2Ox needed = 0.05 mol
mols H2Ox = grams H2Ox/molar mass. You know molar mass and mols, solve for grams H2Ox.
Post your work if you get stuck.
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