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    kickatinalong's Avatar
    kickatinalong Posts: 1, Reputation: 1
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    #1

    Mar 8, 2009, 09:43 PM
    Molarity of NaOH
    27.80ml of 0.100 M HNO3 is titrated with 27.35ml of an NaOH solution.
    What is the molarity of the NaOH ?
    kp2171's Avatar
    kp2171 Posts: 5,318, Reputation: 1612
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    #2

    Mar 8, 2009, 09:49 PM
    We won't do your homework for you.

    This kind of problem makes you determine the moles of acid used... then the moles of base it reacted with... then determine molarity from that.

    So... how many moles of acid were used? Use the volume and molarity to determine this.

    This is a monoprotic acid, meaning it only gives off one H+... that simplifies things

    So for the moles of H+... determine the moles of HO-

    Then use moles of HO- and volume to determine molarity of base.

    Again... we won't do the work for you. Try it out, tell us what you get.
    Unknown008's Avatar
    Unknown008 Posts: 8,076, Reputation: 723
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    #3

    Mar 11, 2009, 04:03 AM

    Always write a chemical equation in tasks like this. Start by writing the equation between the reaction of HNO3 and NaOH and their products, then you'll see the mole ratio. From that, you'll be able to tell how many moles of NaOH was present, and the molarity (or concentration).
    Raysmommy's Avatar
    Raysmommy Posts: 3, Reputation: 3
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    #4

    Mar 11, 2009, 12:49 PM
    Quote Originally Posted by kickatinalong View Post
    27.80ml of 0.100 M HNO3 is titrated with 27.35ml of an NaOH solution.
    What is the molarity of the NaOH ?
    Use the formula
    M(acid) * V(acid) = M(base) * V(base)

    plug in your information and use algebra to solve for the molarity of the base.
    kp2171's Avatar
    kp2171 Posts: 5,318, Reputation: 1612
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    #5

    Mar 11, 2009, 01:25 PM
    Quote Originally Posted by Raysmommy View Post
    Use the formula
    M(acid) * V(acid) = M(base) * V(base)

    plug in your information and use algebra to solve for the molarity of the base.
    It is absolutely fine to show this formula, but also important to note that this only works when you have reactants that react in a 1:1 relationship, as seen in this problem.

    Relying strictly on this formula would often throw wrong answers with students on tests or quizzes who didn't understand that stoichiometry needed to be considered. We'd always give a few problems that would deliberately cause the "plug it into m1v1=m2v2" answers to fail without thinking about stoichiometric ratios. Standardized tests also tend to do this.

    But all that said... its still a great formula to use when you keep the need for 1:1 in mind.

    All this said, the OP'er hasn't still tried to answer the question... fishing for easy answers perhaps?
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