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# Investigation into the dibasicty of sulphuric acid

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Introduction

OCR (2812/03/PLAN) Practical Examination 1 (Part A - Planning Exercise) Aim The aim is to prove that Sulphuric acid is a dibasic (diprotic) acid. Dibasic (diprotic) means that the acid in this instance H2SO4 contains two hydrogen atoms that can be ionized [http://www.thefreedictionary.com/dibasic] Experiments In order to prove its dibasicity I have to plan out two different methods, the first will include gas collection as the other will be a titration Hazard and safety precaution H2SO4 is very corrosive and can burn the skin therefore I shall wear gloves when handling the concentrated acid, also incase there is any spillage of the acid I shall clean it up with plenty of water or I shall use a weak alkali to neutralise the acid. Gas Collection The first experiment that I will be doing will be a gas collection I will be reacting magnesium with a monobasic acid (hydrochloric acid) and a dibasic acid (sulphuric acid), and will be measuring the amount of H2 gas being produced. To do this experiment I will need to use the apparatus shown in the picture below. ...read more.

Middle

To calculate the % error I must do the accuracy of the equipment over the mass of the Mg times 100 (0.01 � 0.070874) x 100 = 14% (This is an estimate) If I was using a more accurate method of weighing the mass using scales that had and accuracy of 0.001g I'd have a lower % error. (0.001 � 0.070874) x 100 = 1.4% (This is an estimate) I now need to calculate the minimum volume of H2SO4 required to produce 0.002916 moles of H2. Using the molar ratio of 1:1 I know I need 0.002916 moles of H2SO4. To work out the volume I will use the formula Volume = Moles � Concentration (The initial concentration of H2SO4 is 1moldm-3) 0.002916 � 1 = 0.002916 0.002916 x 1000 = 2.916cm3 For the actual experiment I will use 5cm3 of the H2SO4 to ensure there is excess acid to react with the Mg (0.07g). To prove that the H2SO4 is dibasic I am going to use the ionic equation which is 2H+ + 2e- --> H2 This is in consideration that I have collected approximately 70cm3 of H2 gas, I can show that I have collected 2 moles of H2 gas. ...read more.

Conclusion

Then silver nitrate solution is added. Various precipitates may be formed from the reaction between the silver and halide ions. To check that you have got bromoethane a very pale cream precipitate will have formed * Test for butan-1-ol To test for a primary alcohol you must oxidise the alcohol by heating with acidified aqueous potassium dichromate (VI), on gentle heating the primary alcohol will produce aldehydes . While the aldehyde is formed it must be separated by distillation as they are formed seeing as their more volatile than their corresponding alcohol. Upon stronger heating under reflux with an excess of acidified dichromate (VI), they aldehydes are oxidised to carboxylic acids. To see if you have a primary alcohol you would notice a distinct change to a very dark shade of brown/green. * Test for 2-methylpropan-2-ol To test for this secondary alcohol you would add a couple of drops of the alcohol into a test tube containing potassium dichromate (VI) solution acidified with dilute sulphuric acid. The tube would be warmed in a hot water bath. After heating over a sufficient period of time the tertiary alcohol should turn orange. ?? ?? ?? ?? WTFCOURSEWORKINGO Candidate Number: 5621 Centre Number: 12828 Page | 1 ...read more.

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