Equations: CaOH(aq) + CO(g)→ CaCO(aq) + H0(l) Word Count: 134
Ethanoic acid:
Apparatus:
Solutions A to E
Ethanol
Concentrated Sulphuric acid
Bunsen Burner
Stand
Water supply
Round bottom flask
Condenser
Tubes
Diagram:
Method:
I will set up the apparatus as shown above. Warming ethanol with ethanoic acid, and a strong acid catalyst (concentrated sulphuric acid), it forms an ester. The O-H bond in ethanol is broken in the esterification reaction. Equation: CHCOOH(aq) + CHOH(aq) → CHCOOCHCH(aq) + HO(l)
Nitric acid:
Apparatus:
Solutions A to E
Magnesium nitrate
Bunsen burner
Stand and Clamp
Test tube
Conical Flask
Stopper with tube.
Wooden Splint
Diagram:
Method:
I will set up the apparatus as it is shown above. 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. This is a displacement reaction, causing the solution to decolorize.
Equation: 2KBr(aq) + Cl(aq) → 2KCl(aq) + Br(aq)
Aqueous Sodium Chloride:
Apparatus:
Solutions A to E
Silver nitrate
Test tubes.
Diagram:
Method:
The apparatus will be set up as shown above.
Aqueous sodium chloride can be tested by adding silver nitrate to the aqueous solution of sodium chloride. We will know that this is sodium chloride when the white precipitate is formed.
Equation: AgNO(aq) + NaCl(aq) --> AgCl(s) + NaNO(aq)
Word Count: 126
Results table:
Tick the Solution if any of the listed changes occur:
Titration Procedure:
Apparatus:
Aqueous nitric acid
Aqueous Sodium Carbonate
Methyl Orange indicator
Burette
Conical Flask
Pipette
Clamp and stand
White tile
Funnel
Diagram:
Method:
Set up apparatus as above. 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 = (0.0125/average titration volume) x 1000
Word Count: 86
References: