Chemical Analysis
- Created by: Joe Clarkson
- Created on: 26-04-13 22:07
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- Chemical Analysis and (Gases, reversible reactions and Ammonia
- Chemical Analysis
- Qualitative
- Uses:- Blood tests and water tests
- Each result must be different so that you have a definite result
- Testing for ions
- Flame test
- Dip clean wire in compound then put above flame
- Calcium = brick-red flame
- Sodium = yellow/orange flame
- Flame test
- Dip clean wire in compound then put above flame
- Calcium = brick-red flame
- Sodium = yellow/orange flame
- Potassium = lilac flame
- Copper = blue-green flame
- Copper = blue-green flame
- Copper = blue-green flame
- Potassium = lilac flame
- Sodium = yellow/orange flame
- Potassium = lilac flame
- Flame test
- Sodium = yellow/orange flame
- Positive ions test (precipitate)
- Add few drops of sodium hydroxide (NaOH) to the compound solution
- Hydroxide reacts with metal and turns them into an insoluble metal hydroxide
- Results:
- Calcium = white
- Copper = blue
- Iron 2 = green
- Iron 3 = brown
- Aluminium = White but then redissolves
- Ammonium = No precipitate but gives off ammonia
- Flame test
- Quantitative Analysis
- Measuring amounts
- THE MOLE
- Molar mass = mass of one mole
- Mass in g = no. moles x Mr
- No. moles = mass in g/ Mr
- Solutions and concentrations
- Find out how much substance is dissolved by evaporating the solution
- THE MOLE
- Hard Water
- Forms soap scum = wasted water
- Caused by calcium and magnesium ions
- Obtained by water flowing over rocks
- 2 types :
- Temporary
- Caused by calcium carbonate (chalk)
- Temporary
- Removed by Boiling
- Temporary
- Caused by calcium carbonate (chalk)
- Temporary
- Removed by an ion exchange column (swaps ions with sodium ions)
- Permenant
- 2 types :
- Caused by calcium sulfate
- 2 types :
- Permenant
- Titrations
- Used to find out concentrations
- Neutralization reaction to show how much acid is needed to neutralize an alkali (or vice versa)
- Instructions
- 1. Use pipette filler to add alkali to a conical flask with drops of indicator
- 2. Fill a burette with acid
- 3. Add the acid to the alkali slowly and swirl the flask every now and again
- 4. The indicator will become colourless when all of the alkali has been neautralized
- 1. Use pipette filler to add alkali to a conical flask with drops of indicator
- 2. Fill a burette with acid
- 3. Add the acid to the alkali slowly and swirl the flask every now and again
- 4. The indicator will become colourless when all of the alkali has been neautralized
- 4. The indicator will become colourless when all of the alkali has been neautralized
- 3. Add the acid to the alkali slowly and swirl the flask every now and again
- 2. Fill a burette with acid
- 1. Use pipette filler to add alkali to a conical flask with drops of indicator
- 4. The indicator will become colourless when all of the alkali has been neautralized
- 3. Add the acid to the alkali slowly and swirl the flask every now and again
- 2. Fill a burette with acid
- 1. Use pipette filler to add alkali to a conical flask with drops of indicator
- Used to find out concentrations
- Preparing soluble salts
- Made using an acid and insoluble reactant
- Add base to acid
- Filter out excess solid
- Evaporate the water and crystalise the salt
- Filter out excess solid
- Add base to acid
- Made using an acid and soluble reactant
- Reacting acid and alkali
- Titratiion needs to be performed to know how much to add
- Reacting acid and alkali
- Made using an acid and insoluble reactant
- Measuring amounts
- Qualitative
- Gases, Reversible reactions and ammonia
- The Haber Process (Reversible reaction)
- Nitrogen and hydrogen are needed to make ammonia
- Nitrogen extracted from air (78% nitrogen)
- Hydrogen obtained from natural gases
- Creates dynamic equilibrium as not all oxygen and hydrogen is changed into ammonia
- Conditions used:
- High pressure to increase percentage yield of ammonia without increasing expenses to much
- High temperature to increase the rate of reaction as there is a higher yield in a shorter length of time
- Iron catalyst is used
- Ammonia is collected as a gas but cools to liquid in the condenser
- Ammonia is used to make nitrogenous fertilisers
- Increase plant growth
- Ammonia is used to make nitrogenous fertilisers
- Nitrogen and hydrogen are needed to make ammonia
- The Haber Process (Reversible reaction)
- Chemical Analysis
- Halide test
- Testing for ions
- Positive ions test (precipitate)
- Add few drops of sodium hydroxide (NaOH) to the compound solution
- Hydroxide reacts with metal and turns them into an insoluble metal hydroxide
- Results:
- Calcium = white
- Copper = blue
- Iron 2 = green
- Iron 3 = brown
- Aluminium = White but then redissolves
- Ammonium = No precipitate but gives off ammonia
- Positive ions test (precipitate)
- Add nitric acid(HNO3) then silver nitrate(AgNO3)
- Acid gets rid of carbonates
- Results:
- Chloride = white precipitate
- Bromide = cream precipitate
- Iodide = Yellow
- Bromide = cream precipitate
- Bromide = cream precipitate
- Iodide = Yellow
- Chloride = white precipitate
- Testing for ions
- 6.023 x 10(power of 23)
- THE MOLE
- Molar mass = mass of one mole
- Mass in g = no. moles x Mr
- No. moles = mass in g/ Mr
- No. of particles (compound or element) with the same no. grams as the relative mass
- THE MOLE
- Concentration = Mass/ volume
- Solutions and concentrations
- Find out how much substance is dissolved by evaporating the solution
- Measured in g/dm(3)-mass concentration or mol/dm(3)- mole concentration
- Mole concentration = mass-concentration / Mr
- Mass concentration = mole-concentration x Mr
- Solutions and concentrations
- Calculating volumes
- Gases, Reversible reactions and ammonia
- The Haber Process (Reversible reaction)
- Nitrogen and hydrogen are needed to make ammonia
- Nitrogen extracted from air (78% nitrogen)
- Hydrogen obtained from natural gases
- Creates dynamic equilibrium as not all oxygen and hydrogen is changed into ammonia
- Conditions used:
- High pressure to increase percentage yield of ammonia without increasing expenses to much
- High temperature to increase the rate of reaction as there is a higher yield in a shorter length of time
- Iron catalyst is used
- Ammonia is collected as a gas but cools to liquid in the condenser
- Ammonia is used to make nitrogenous fertilisers
- Increase plant growth
- Ammonia is used to make nitrogenous fertilisers
- Nitrogen and hydrogen are needed to make ammonia
- The Haber Process (Reversible reaction)
- Avogadro's law - One mole of any gas occupies 24dm(3)
- Volume of gas (dm) =Mass of gas/Mr of gas X 24
- You can calculate volumes in reactions
- Gases, Reversible reactions and ammonia
- Reversible reactions
- Where the products of a reaction can react with each other to turn back tot eh original reactants
- Reversible reactions will reach dynamic equilibrium
- Closed system - no products or reactants can escape
- Position of equilibrium is dependent on the temperature and pressure
- Raise pressure = increase the reaction with less volume
- Lower pressure = increase reaction with more volume
- Raise pressure = increase the reaction with less volume
- Catalysts do not alter the position of equilibrium but speed up the reaction
- Lower temp = exothermic reaction increase
- Position of equilibrium is dependent on the temperature and pressure
- Lower pressure = increase reaction with more volume
- Catalysts do not alter the position of equilibrium but speed up the reaction
- Lower temp = exothermic reaction increase
- Raise temp =endothermic reaction increase
- Raise temp =endothermic reaction increase
- Lower temp = exothermic reaction increase
- Catalysts do not alter the position of equilibrium but speed up the reaction
- Lower pressure = increase reaction with more volume
- Raise temp =endothermic reaction increase
- Position of equilibrium is dependent on the temperature and pressure
- Lower temp = exothermic reaction increase
- Both reactions are still happening but are equal
- Reversible reactions will reach dynamic equilibrium
- Closed system - no products or reactants can escape
- Reversible reactions will reach dynamic equilibrium
- Entering rivers can cause eutriphication
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