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What is the pH of the solution created by combining 2.00 mL of the 0.10 M base[ammonia] with 8.00 mL of the 0.10 M acid[acid acid]?

I tried this problem so many times, but always got it wrong. It's a weak base and acid titration. but i don't know the method of do this type of proble

  • Chemistry -

    It's done with moles.
    You have acid acid for the acid so I don't know which acid you are using.
    mols base = M x L = 0.1 x 0.002 L = xx
    mols acid = M x L = 0.1 x 0.008 L = yy
    There will be xx mols salt formd.
    There will be xx mols acid - yy mols base = excess acid unreacted. All of the base will be gone.
    The pH will be that of the acid/salt system but we need to know the acid to proceed.

  • Chemistry -

    I believe he was referring to hydrochloric acid

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