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Planning Exercise: Prove sulphuric acid is dibasic

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Introduction

Bernadette Walsh April 2008 Planning Exercise You are required to plan two different experiments that would enable you to prove that sulphuric acid is dibasic. One of your experiments should involve a titration and the other should involve collection of a gas. Your planning must be based on the assumption that you are provided with the following: -Aqueous sulphuric acid of concentration 1.00 moldm-3 -Any chemicals (other than sulphuric acid) and equipment that you require from your school/college laboratory. Your plan should include the following: - Relevant chemical knowledge and understanding from the as part of your chemistry course, including balanced equations; - Detailed procedures that provide full instructions about how to obtain accurate results; - A diagram of the apparatus used in the gas collection experiment - Suitable quantities of chemicals to use in both of your experiments and calculations to show how you worked out these quantities; - A specimen calculation to show how the basicity of sulphuric acid would be worked out from the titration data - A hazard and a safety precaution for the use of the sulphuric acid provided All quotations direct from the work of others should be acknowledged by quotation marks, with page references and the sources should be included in the bibiliography. Introduction: The aim of this experiment is to demonstrate that sulphuric acid, H2SO4, is dibasic. Scientific Knowledge: Sulphuric acid, H2SO4, is a dibasic (diprotic) ...read more.

Middle

Spills Wear safety glasses. Clean up immediately so that people cant slip over or be harmed by it. Bibliography: http://www.btinternet.com/~chemistry.diagrams/titration.htm http://www.chemguide.co.uk/inorganic/period3/oxidesh2o.html Bernadette Walsh April 2008 Planning Exercise Introduction: The aim of this experiment is to demonstrate that sulphuric acid, H2SO4 is dibasic. Scientific Knowledge: Sulphuric acid, H2SO4, is a dibasic (diprotic) acid. This means that one mole of sulphuric acid can give off two moles of hydrogen ions, H+, when It reacts in aqueous solution. H2SO4 can be proven to be dibasic/diprotic with two methods, by gas collection and by titration. These methods will be explained in the next section. Methods: Method (a): by measurement of the gas: 1. Set up apparatus as shown below: Calculations for gas collection: Use Excess Mg. 0.35 100 cm cubed big Due to the fact that only 100cm3 gas syringes are available, the maximum amount of gas that can be produced in this experiment will be 0.042 moles of C02 (as 100/2400 = 0.42). For one mole of H2S04 the maxiumum volume is 0.0042 x 1000/10 = 4.2 cm3. to ensure that I do not go over this limit I will only use 3.5cm3 of sulphuric acid. To ensure that all of the H2SO4 reacts, I must use excess MgCO3 the minimum MgCO3 I can use is Mass if MgCO3 = 0.0042 x 84 = 0.35g of MgCO3. To ensure that I am in excess you could use 0.5 of MgCO3. ...read more.

Conclusion

of 1M HNO3; 1M HCl and 1M H2SO4 (separately of course), using 1M NaOH. -Record the volumes of NaOH needed to neutralise each. -As they are strong acids the monoprotic acids (hydrochloric and nitric) should be within a reasonable margin for error (5%-ish), but roughly the same, showing that they have an equal proportion of H+ ions to be neutralised. H+ + OH- > H2O -However the diprotic sulphuric acid (yes I'm English) should react with twice as much NaOH, showing it has twice as many H+ ions. 2H+ + 2OH- > 2H2O (^needs twice as many OH ions see) H2SO4 + X -> XSO4 + H2 "X" is any sutable metal. The volume of gas would be an indication of the number of moles, since at room temperature and pressure, 1 mole of any gas occupies 22.4 liters. Proving that sulphuric acid reacting with MgCO3 is dibasic in a gas experiment how do I do this? When a carbonate reacts with an acid, CO2 is produced. The ratio of acid used to CO2 produced is 1:1 for a diprotic acid, or 2:1 for a monoprotic acid, as the following equations demonstrate. MgCO3 + H2SO4 -> MgSO4 + H2O + CO2 (diprotic acid) MgCO3 + 2HCl -> MgCl2 + H2O + CO2 (monoprotic acid) Collect the CO2 produced and compare with the quantity of acid needed. To produce a similar amount of CO2, you'll find that you need half the amount of H2SO4 compared to HCl. ...read more.

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