Calculate the amount (volume) of 6.25% (wt./vol.) NaOCl solution (commercial bleach)
required to oxidize 150 mg of 9-fluorenol to 9-fluorenone. Whenever appropriate, use
balanced chemical equations as a part of your calculation.

Any help is appreciatede.

  1. 👍
  2. 👎
  3. 👁
  1. Do you go to UCI by any chance? Anyway, this is how the TA helped me:

    6.25% w/vol
    1000 g/L

    62.5 g/L

    150 mg/ 182.2 = 0.82 mmol x 74 (the NaOCl MW) = 60.92 mg

    62.5 mg/mL x (x)mL = 60.92 mg

    60.92 mg/ 62.5 = 0.97 mL which is roughly 1

    and we know that our calculation is correct because the procedure asks for 1.2 mL, so it's fairly close!

    Hope that helps!!

    1. 👍
    2. 👎
  2. I go to UCI, and this helped a lot. Thank you!

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    what volume (in L) of 0.150 M KCl solution is required to completely react with 0.150 L of a 0.175 M Pb(NO3)2 solution according to the following balanced chemical equation? 2KCl (aq) + Pb(NO3)2 (aq) --> PbCl2 (s) + 2 KNO3 (aq)

  2. Chemistry: please double check...

    Please double check one last time have to hand it in tomorrow.Thank-You in Advance. This was the lab experiment: ------------------------------------------- A. Standardization of the Sodium Thiosulfate Solution Make up a standard

  3.!! =)

    One brand of laundry bleach is an aqueous solution containing 4.00% sodium hypochlorite (NaOCl) by mass What is the molarity of this solution? (Assume a density of 1.02 g/mL .)

  4. Chemistry

    Hello, So I have recently done a lab with cobalt(II) nitrate and NaOCl (bleach) and our objective was to determine if colbalt or the bleach is part of the rate determining step. With the lab we have done trials by diluting the

  1. Chemistry

    A solution household bleach contains 5.25% NaClO, by mass. Assuming that the density of bleach is the same as water(1.0g/ml). Calculate the volume in mL of household bleach that should be diluted with water to make 500.0 ml of a

  2. Math

    A bookworm finds itself on page 1 of volume 1 and begins eating straight through to the last page of volume 5.If each book is 6 centimeters thick,including the front and back covers,which are half a centimeter each what is the

  3. Chemistry

    Commercial bleach contains 5.25% (by mass) of NaClO in water. It has a density of 1.08 g/mL. Calculate the molarity of this solution. (Hints: assume you have 1 L of solution (mass 1080 g); molar mass of NaClO is 74.4 g/mol)

  4. chemistry

    Would the following procedural errors result in an incorrectly high or low calculated percent NaOCl in commercial bleach solution? A student failed to allow the volumetric pipet to drain completely when transferring the diluted

  1. Chemistry

    Calculate [ClO^-] in a 6% bleach solution. A 6% bleach solution contains 6 grams of NaClO per 100 grams bleach. The density of 6% bleach is 1.07g/mL.

  2. Chemistry

    When dilute nitric acid was added to a solution of one of the following chemicals, a gas was evolved. This gas turned a drop of limewater, Ca(OH)2, cloudy, due to the formation of a white precipitate. The chemical was.... a. the

  3. Chemistry

    Calculate the mass in grams of the undiluted bleach that was in the sample of bleach titrated. Given: Density of undiluted bleach unkown is 1.042 g/mL. 14.44 mL of .100 M Na2S2O3. .0537 grams of NaClO. Each sample should conain

  4. Chemistry

    4.80 dm^3 of chlorine gas was reacted with NaOH solution. a) how many moles of Cl2 reacted b) what mass of NaOCl was formed? c) if the concentration of the NaOH was 2.00 mol/dm^3. What volume of sodium hydroxide solution was

You can view more similar questions or ask a new question.