Chapter 7.8, Problem 13P

Commercial bleach contains either chlorine or oxygen as an active ingredient.  A commercial oxygenated bleach is much safer to handle and less likely to ruin your clothes.  It is possible to determine the amount of active ingredient in an oxygenated bleach product by performing a redox titration.  The balance reaction for such a titration is: 6H+ +5H2O2 +2MnO4- à 5O2 + 2Mn2+ + 8H2O If you performed the following procedure: “First, dilute the Seventh Generation Non-Chlorine Bleach by pipetting 10 mL of bleach in a 100 mL volumetric flask and filling the flask to the mark with distilled water. Next, pipet 10 mL of the diluted bleach solution into a 250 mL Erlenmeyer flask and add 20 mL of 1.0 M H2SO4 to the flask. This solution should be titrated with 0.0100 M KMnO4 solution.”  It took 18.47mL of the KMnO4 to reach the endpoint on average.  What was the concentration of H2O2 in the original bleach solution in weight % assuming the density of bleach is 1g/mL?

10.

Proper care of pH electrodes: Why can you not store a pH electrode in distilled water?  What must you instead store it in?  Why?

Write the electron configuration of an atom of the element highlighted in this outline of the Periodic Table: 1 23 4 569 7 He Ne Ar Kr Xe Rn Hint: you do not need to know the name or symbol of the highlighted element! §

Identify the amino acids by name. Illustrate a titration curve for this tetrapeptide indicating the pKa's for each ionizable groups and identify the pI for this tetrapeptide. please help

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A common buffer for stabilizing antibodies is 100 mM Histidine at pH 7.0. Describe the preparation of this buffer beginning with L-Histidine monohydrochloride monohydrate and 1 M NaOH. Be certain to show the buffering reaction that includes the conjugate acid and base.

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Is the structural form shown possible given the pKa constraints of the side chains?