Iron(lab 7) - Standard/Sample averaging Fit type Weight and volume corrections Min R Concentration units OFF Linear OFF 0.95000 mg/L The

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Standard/Sample averaging OFF Fit type Linear Weight and volume corrections OFF Min R² 0.95000 Concentration units mg/L Calibration Standard Concentration F Readings mg/L ________________________________________________ Std 1 0.102 0.0113 Std 2 0.502 0.0783 Std 3 1.02 0.1688 Std 4 2.502 0.4329 Calibration eqn Abs = 0.1762*Conc +0.0089 Correlation Coefficient 0.99999 Analysis Sample Concentration F Readings mg/L ________________________________________________ LB samp1 2.092 0.3603 unk well samp2 1.242 0.2102 The Determination of Iron in Natural Water By Joel I. Eldridge Abstract Determining the Fe(III) concentration level in natural well water is the purpose of  this experiment.   The red-orange complex that forms between Fe(III) and 1,10- phenanthroline (orthophenanthroline) is useful in determining iron in water supplies.  The reagent is a weak base that reacts to form phenanthrolinium ion, phenH + , in acidic  media.  
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  INTRODUCTION The red-orange complex that forms between Fe(III) and 1,10-phenanthroline  (orthophenanthroline) is useful in determining iron in water supplies. The reagent  is a weak base that reacts to form phenanthrolinium ion, phenH + , in acidic media.  The complex used during this experiment, [(C12H8N2) 3 Fe] 2+ , is 11,100 at 600 nm.  Fe(III) is quantitatively complexed in the pH range between 3 and 9. A pH of  about 3.5 is ordinarily recommended to prevent precipitation of iron salts, such as  phosphates. An excess of a reducing reagent, such as hydroxylamine or  hydroquinone, is needed to maintain iron in the +3 oxidation state. The complex,  once formed, is very stable.  Beer’s law is obeyed; however, iron must be in the  ferrous state and thus a reducing agent can be added. Principle There are a plethora of methods used to determine the amount of iron in natural  water. The red-orange complex that forms between Fe(II) and 1,10-phenanthroline  (orthophenanthroline) is useful in determining iron in water supplies. The reagent  is a weak base that reacts to form phenanthrolinium ion, phenH + , in acidic media. 
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This note was uploaded on 04/18/2011 for the course CHEMISTRY 210 taught by Professor Dr.han during the Spring '11 term at Fayetteville State University.

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Iron(lab 7) - Standard/Sample averaging Fit type Weight and volume corrections Min R Concentration units OFF Linear OFF 0.95000 mg/L The

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