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Environmental Chemistry- Analysis of an Acid Rain Solution:

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Introduction

Environmental Chemistry- Analysis of an Acid Rain Solution: Purpose: To prepare a standard solution of sodium hydroxide and to use that solution in a titration to analyze a solution of acid rain and to calculate the concentration of the sulfuric acid it contains. Apparatus: 1. 250 ml Erlenmeyer flask 2. Electronic Balance 3. 100 ml Beaker 4. 100 ml Conical Flask 5. 10 ml Pipette and Filler 6. Burette 7. Stirring rod Materials: * Solution of Acid Rain * Sodium hydroxide solution (0.5 mol dm-3) * Distilled Water * Phenolphthalein Indicator Procedure: 1. Use a pipette and pipette filler to transfer 25 ml of the 'acid rain' sample to a 100 ml conical flask. ...read more.

Middle

Run in the small volumes of sodium hydroxide solution until you first observe a permanent color change in the titration mixture. 5. Your first attempt will be a rough titration; you will have gone beyond the end-point and added more sodium hydroxide than is needed to react with all the acid in the flask. You should, however, now have an idea of what the end-point is. Do several more titrations until you record two volumes that agree within 0.1 ml. When you get near the end-points of these titrations, you should add the sodium hydroxide carefully, adding only one drop of solution at a time until new permanent color is produced. ...read more.

Conclusion

Concentration of Sulphuric Acid: Moles= Concentration x Volume * Volume must be in dm3 Concentration == Concentration of sulphuric acid= 0.11mol dm-3 pH of Sulphuric Acid: pH= -log10 [H2SO4] pH= -log10 [ 0.11] pH= 0.96 The stronger the concentration of the acid, the smaller the pH value. Hence, a strong acid of concentration greater than 1 mol dm-3 will have a pH value less than 0. Looking at the above calculation, sulphuric acid has a concentration of 0.11mol dm-3 and a pH of 0.96. Hence, it will have a concentration less than 1 mol dm-3 and a pH value greater than 0. ...read more.

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