# College Chemistry

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1) A 25mL sample of the .265M HCI solution from the previous question is
titrated with a solution of NaOH. 28.25mL of the NaOH solution is required
to titrate the HCl. Calculate the molarity of the NaOH solution.

2) A 1.12g sample of an unknown
monoprotic acid is titrated with 29.15mL of .315M NaOH. Calculate the molar mass of the acid.

3) A student dissolves a 1.18g aspirin tablet in water and titrates the
solution with a .265M NaOH. 22.05mL of NaOH are required to reach the
equivalence point. Calculate the percentage of acetylsalicylic acid in the tablet.

• College Chemistry -

Wow,you are really wanting someone to do your homework for you. How many questions have you posted?!?!

• College Chemistry -

yea this is to help not do all your work for u

• College Chemistry -

The titration equation

Heqacid*Molarityacid*volumeacid=Heqbase*Molaritybase*volumebase

where Heqacid=1 for monoprotic acid, 2 for diprotic, and 3 for triprotic acid
Heqbase=1 for single OH, 2 for two OH, and 3 for three OH

• College Chemistry -

for your first question: first get a balanced equation, then calculate moles of HCl from that, then use the equation to get moles of NaOH and you use given information to get M NaOH

• College Chemistry -

for your third question try using the equation (mass of acid/mass of tablet)x 100

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