Asked by anonymous
Two aqueous solutions are mixed: 50.0 mL of 1.60×10−2 M H2SO4 and 50.0 mL of 3.75×10−2 M NaOH.
what is the PH of the following solution?
what is the PH of the following solution?
Answers
Answered by
DrBob222
The trick to these question is to recognize what you have in the final solution.
Write the equation.
H2SO4 + 2NaOH ==> Na2SO4 + 2H2O
moles H2SO4 = M x L = ??
moles NaOH = M x L= ??
moles H2SO4 required to use all of it will be moles H2SO4 x 2 (since there are two moles NaOH for every mole of H2SO4). Look at those numbers, see which is in excess and use that to calculate either the OH or the H depending upon the one in excess.
Post your work if you get stuck.
Write the equation.
H2SO4 + 2NaOH ==> Na2SO4 + 2H2O
moles H2SO4 = M x L = ??
moles NaOH = M x L= ??
moles H2SO4 required to use all of it will be moles H2SO4 x 2 (since there are two moles NaOH for every mole of H2SO4). Look at those numbers, see which is in excess and use that to calculate either the OH or the H depending upon the one in excess.
Post your work if you get stuck.
Answered by
Anonymous
so what the h is the answer
There are no AI answers yet. The ability to request AI answers is coming soon!