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March 29, 2017

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19 mL of 0.50 mool/L NaOH which is standardized becomes titrated alongside 24 mL of 0.44 mol/L acetic acid. Determine the pH of the solution

Please judge my work:

Becasue NaOH and acetic acid react in a 1:1 ratio,

initital moles of acetic acid
=0.0019 L x 0.44M
= 0.000836 mols

mols of acetic acid neutralized is
= 0.0024 L x 0.44 M
=0.0019 L

molfs of acetic acid is 0.0019-0.000836 =0.001064

Whats my next steps?

  • chemistry - ,

    19 mL of 0.50 mool/L NaOH which is standardized becomes titrated alongside 24 mL of 0.44 mol/L acetic acid. Determine the pH of the solution

    Please judge my work:

    Becasue NaOH and acetic acid react in a 1:1 ratio, OK to here but check your numbers. They don't make sense.

    initital moles of acetic acid
    =0.0019 L x 0.44M It's 19 mL of NaOH which is 0.44 M. You've mixed up mL and component, I believe.
    = 0.000836 mols

    mols of acetic acid neutralized is
    = 0.0024 L x 0.44 M The one above also says acaeitic acid so which is which?
    =0.0019 L Liters???. You started out by saying this was mols. Is molarity measured in L?

    molfs of acetic acid is 0.0019-0.000836 =0.001064

    Whats my next steps?

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