1 answer

#40*mL# of sulfuric acid with a concentration of #0.05*mol*L^-1# was titrated with #50*mL# volume of #NaOH(aq)#. What was the concentration

Question:

#40*mL# of sulfuric acid with a concentration of #0.05*mol*L^-1# was titrated with #50*mL# volume of #NaOH(aq)#. What was the concentration of #NaOH(aq)#?

Answers

We interrogate the chemical equation:

#2NaOH(aq) + H_2SO_4(aq) rarr Na_2SO_4(aq) + 2H_2O(l)#

Explanation:

And we write this equation in order to establish the molar equivalence...

We use a volume of #40*mL# of #0.05*mol*L^-1# concentration with respect to sulfuric acid....

And this is a molar quantity of #40*mLxx10^-3*L*mL^-1xx0.05*mol*L^-1=2.0xx10^-3*mol#.

And so the stoichiometry requires that FOR EQUIVALENCE there were TWICE this molar quantity with respect to #NaOH#..

#i.# #[NaOH(aq)]=(2xx2.0xx10^-3*mol)/(0.050*L^-1)=0.080*mol*L^-1#...you can check on the description of #"normality"# versus #"molarity"#...here, for #NaOH#, BUT NOT for sulfuric acid, they are the same....

#ii.# Now in aqueous solution....#pH+pOH=14#...here...#pOH=-log_10(0.080)=1.10#..

...but #pH=14-pOH=14-1.10=12.90#...

.

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