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anonymous

  • one year ago

Check work? I suppose I would do this with the proper sig figs? A buret containing NaOH solution has an initial volume reading of 0.14 mL. A 25.00 mL solution of 0.1000 M HCl is titrated to a phenolphthalein end point, which occurs at a final buret reading of 27.16 mL of NaOH. What is the molarity of the NaOH titrant? My work: http://imgur.com/tBITDwk

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  1. anonymous
    • one year ago
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    @Vocaloid

  2. anonymous
    • one year ago
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    *actually, I think I made a mistake with sig figs

  3. anonymous
    • one year ago
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    *0.027

  4. anonymous
    • one year ago
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    You did the steps to the answer correctly. But there were some mistakes There should be a parentheses like this to avoid confusion. \[(27.16-0.14) \times \frac{ 1L }{ 1000mL }\] Since your teacher might think you multiplied it tje 0.14 by 1/1000. Second you do not need to round your significant figures until it is your final answer. (27.16-0.14) x (1/1000) should not be in significant figure. I saw that you rounded the 0.02702 into 0.03. It is not necessary.

  5. anonymous
    • one year ago
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    You are right that your answer is in 2 significant figures.

  6. anonymous
    • one year ago
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    0.14mL has the least significant figures and your final equation is dividing. Dividing would be the lowest significant figure in the question.

  7. anonymous
    • one year ago
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    0.093 M NaOH

  8. anonymous
    • one year ago
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    0.003mol NaOH/0.02702L NaOH=0.11M

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