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Posted by on Monday, October 25, 2010 at 2:29pm.

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 - , Monday, October 25, 2010 at 2:34pm

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

  • College Chemistry - , Monday, October 25, 2010 at 2:35pm

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

  • College Chemistry - , Monday, October 25, 2010 at 3:29pm

    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 - , Tuesday, October 26, 2010 at 10:31pm

    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 - , Tuesday, October 26, 2010 at 10:32pm

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

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