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Chemistry

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Suppose you have two solutions to titrate with NaOH: (a) 10 ml of.1M HCL (b) 10 ml of .1M CH3COOH
would you expect either of the solutions to require different volumes of NaOH in order to reach an end point? Explain

  • Chemistry - ,

    Do I need to first figure out the PH?
    I believe that a= 3
    and b=2.87
    therefore it will require more naoh to titrate the acetic acid.

    I am not sure i figured the ph of acetic acid correctly, or if i am on the correct path here...

  • Chemistry - ,

    No, you don't need to calculate pH. What is the concept of titrating an acid with a base; i.e., when does the indicator show you have reached the end point? The answer to that is that when moles of acid = moles base the indicator tells you to quit adding base. So how many moles are in the 10 mL of 0.1M HCl? That is 0.01 x 0.1 = 0.001 moles HCl.
    How many moles are in the 10 mL of 0.1M CH3COOH? That is 0.01 x 0.1 = 0.001. So the end point will be the same no matter which acid is used. What counts is how many moles of the acid you have.

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