Asked by livingstone
how to calculate the ph level of 2.5g NaOH, 2g H2SO4 and 1.5g ethenoic acid in water? Each compound being put in a liter of water.
Answers
Answered by
DrBob222
NaOH ==> Na^+ + OH^-
mols NaOH = grams/molar mass
mols OH^- = mols NaOH
(OH^-) = mols/L
Convert to pOH and pH.
Ethanoic (note the spelling) I will call HAc. It is a weak acid and ionizes only partially. mols HAc = grams/molar mass.
(HAc) = mols/L. Estimated 0.03
...............HAc ==> H^+ + Ac^-
I..............0.03....0......0
C...............-x.....x.......x
E.............0.03-x...x.......x
Ka = (H^+)(Ac^-)/(HAc)
Substitute into the Ka expression and solve for (H^+), then convet to pH.
H2SO4 isn't that simple. If you still have a problem with it tell us what level this is; i.e., beginning, AP,?
mols NaOH = grams/molar mass
mols OH^- = mols NaOH
(OH^-) = mols/L
Convert to pOH and pH.
Ethanoic (note the spelling) I will call HAc. It is a weak acid and ionizes only partially. mols HAc = grams/molar mass.
(HAc) = mols/L. Estimated 0.03
...............HAc ==> H^+ + Ac^-
I..............0.03....0......0
C...............-x.....x.......x
E.............0.03-x...x.......x
Ka = (H^+)(Ac^-)/(HAc)
Substitute into the Ka expression and solve for (H^+), then convet to pH.
H2SO4 isn't that simple. If you still have a problem with it tell us what level this is; i.e., beginning, AP,?
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