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Chemistry Practical Plan

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Introduction

Chemistry Practical Plan. Aim: The aim of this experiment is to identify the chemicals below in the solutions A to F using suitable reactants, and also carry out a titration procedure to determine the concentration of aqueous nitric acid. *Aqueous calcium hydroxide *Ethanoic acid *Nitric acid *Aqueous Potassium Bromide *Aqueous Sodium Chloride Safety: Wear goggles to avoid chemicals getting into eyes. Immediately clean up spills that might occur. Use gloves if handling strong chemicals. Aqueous sodium hydroxide: Apparatus: Solutions A to E Calcium Carbonate Bunsen burner Stand and Clamp Test tube Conical Flask Stopper with tube. Diagram: Method: I will set up the apparatus as shown as above. When heating calcium carbonate carbon dioxide gas is released; this gas will go down the tube to the solutions. ...read more.

Middle

When Nitric acid is added to Magnesium, Magnesium nitrate and hydrogen if formed. We can test for hydrogen gas by lighting up a splinter, and putting it in the conical flask full of hydrogen gas really quickly (to stop hydrogen escaping), and see if it 'pops'. Equation: Mg(s) + 2HNO(aq) --> Mg(NO)(aq) + H(g) Word Count: 146 Aqueous potassium bromide: Apparatus: Solutions A to E Aqueous Chlorine solution Test tubes. Plastic Pasteur pipettes Diagram: Method: The apparatus will be set up the way it is shown above. Potassium bromide can be tested by adding aqueous chlorine solution, some of the bromide ions are oxidized to bromine. Some of the bromine molecules combine with the bromine ions to give tribromide ion. ...read more.

Conclusion

Add exactly 25cm of aqueous Sodium Carbonate into the pipette and into the conical flask. Add three drops of Methyl Orange indicator to the flask. Using the funnel pour the nitric acid solution into a burette, and take off the funnel. Titrate the nitric acid slowly into the conical flask until colour change appears. Do 1 rough titration, and 3 final titrations. Equation: NaOH(aq) + HNO3(aq) --> NaNO3(aq) + H2O(l) Calculations: Calculating the average titration volume: (Titration Volume 1 + Titration Volume l 2 + Titration Volume 3) / 3 Number of moles in Sodium Carbonate: Moles = concentration x volume / 1000 Moles = 0.500 x 25 / 1000 = 0.0125 mol From the equation we can see that the ratio is 1:1, therefore the number of moles in nitric acid = 0.0125 mol. Concentration = (Moles/Volume) x 1000. Concentration of nitric acid = (0. ...read more.

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