Explain what percent of the total available oxygen-carrying

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Reference no: EM13673849

The formation constant of the complex ion [Fe(CN)6]4- is4.21*10^45. This complex ion is formed by the reaction of Fe2+with a solution of sodium cyanide, NaCN. It is this reaction that makes sodium cyanide extremely toxic to human beings and other animals. The cyanide ion, CN-, binds to the iron that red blood cells use to carry oxygen around the body, therefore interfering with the blood's ability to deliver oxygen to the tissues. It is this toxicity that has made the use of sodium cyanide in gold mining controversial. Most states now ban the use of this chemical in leaching gold out of low-grade ore.

Consider that the body contains 6.30L if blood, and the concentration of [Fe^2+] in the blood is 1.90*10^-5M. If a person ingested 7.00mL if a 15.0mM solution if NaCN, Explain what percent of the total available oxygen-carrying iron in the blood would be sequestered by the cyanide ion?

Reference no: EM13673849

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