Chemistry: Titration of of a base to solve for the mass of an unknown acid.

[Hemolymph]

A student titrated a .4630g of unknown monoprotic acid with .1060M NaOH. The equivalance point volume is 28.70mL.
a) Calculate the number of moles of NaOH used.
Im pretty sure I got this one
I did .1060 M X .02870L to equal 3.04E-3 mol
b)how many equivalents of unknown acid were titrated? no clue

c) Determine the equivalent mass of the unknown acid
Which is the moles times MM


There is also a table given of acids and there pKa and equivalent masses. If I can figure out what Pka is I should be fine.

 

[sjb-2812]

A student titrated a .4630g of unknown monoprotic acid with .1060M NaOH. The equivalance point volume is 28.70mL.
a) Calculate the number of moles of NaOH used.
Im pretty sure I got this one
I did .1060 M X .02870L to equal 3.04E-3 mol
b)how many equivalents of unknown acid were titrated? no clue

c) Determine the equivalent mass of the unknown acid
Which is the moles times MM


There is also a table given of acids and there pKa and equivalent masses. If I can figure out what Pka is I should be fine.

If the unknown acid is HA, can you write a balanced equation for the titration?

 

[Hemolymph]

would it be

NaOH + HA= H_2_O+ NaA?

 

[sjb-2812]

Yes, so if you have 3.04 mmol of NaOH, how many moles of acid do you have?

 

[Hemolymph]

Well since its one to one it would be the same so 3.04mmol of acid. So would that just be the answer for part b? If so I did not think it could be that simple.

 

[sjb-2812]

Part b is more about the recognition that it's 1:1, rather than an actual number.

 

[Hemolymph]

Would part c be .4630g/ .00304moles? Which I got to be 161.03