Core Practicals
- Created by: EllenPlay
- Created on: 27-05-18 11:59
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- Core Practicals
- Electrochemical cells
- Ecell= Erhcell-Elhcell
- Standard Conditions not maintained temparature not 298K not standard concetration 1moldm-3
- slver nitrate is weekened as its highly oxidising and expensive
- The oxidation of ethanol
- Reflux and distillation
- Acidified sodium dichromate highly oxidising
- Gloves
- Ph using indicator paper goes red
- Forming a carboxylic acid
- Calcium carbonate effervescence shows acid product ( gas turns lime water cloudy)
- Magneesium followed by squeaky pop test (acid)
- Fehlings solution no reaction means no aldehyde left
- Determining Ka for a week acid
- pH=-log[H+]
- measurements with a pH meter calilbrated
- Ka found by titrating known volume against NaOH using phenolphthalein, a further equal vol of acid added then pH measured
- Uncertainty inaccuracy of burette readings difficulty identifying end-point. Read from the bottom of the meniscus; white tile can see colour change clearly.
- Finds half equivalence point pH=pKa
- The hydrolysis of halogenoalkanes
- Rates of hydrolysis of Chloro-Bromo-Iodoalkanes
- Also rates of primary secondary and tertiary
- Secondary and tertiary faster rate
- Less time to form a ppt
- Secondary and tertiary faster rate
- Also rates of primary secondary and tertiary
- Further down the group = more reactive
- Less time to form a ppt
- Water in the presence of AgNo3
- Nucleophillic Substitution
- Halogeno- alkanes insoluble in water so ethanol ensures dissolves so it can then react
- Water used instead of hydroxide as hydroxide would form silver hydroxide
- Rates of hydrolysis of Chloro-Bromo-Iodoalkanes
- Find the concentration of a solution of HCl
- Phenolphthalein indicatior
- End point when idicator goes pink
- Pink colour may fade on standing as CO2 in the air neutralises any excess NaOH
- Concordant results within o.02cm3 of each other
- Using Standard NaOH solution
- Phenolphthalein indicatior
- Rate of iodine propanone reaction. Titrimetric method
- Continuous monitoring method
- Concentration time graph
- To determine order of reaction
- Pippette 10cm3 samples
- Add NaHCO3 to quench note time
- Titrate remaining solution against Na2S2O8 with starch indicator
- Add NaHCO3 to quench note time
- Activation energy bromide Vs bromste(V) ion reaction
- time taken for a reaction to happen at different temperatures
- Arrhenius equation
- Chlorination f 2-methylpropan-2-ol
- Producing a pure sample of 2-Chloro-2-methyl-propane
- Add HCl in a conical flask then anhydrous calcium carbonate takes unreacted alcohol
- Continually remove bung and release pressure whilst swirling
- Transfer to separating funnel. Seperate layers formed by pouring off bottom layer/ decanting
- Add sodium hydrogen arbonate to remove acid washing.
- add anhydrous sodium sulfate drying agent
- Decant and distil between small range
- add anhydrous sodium sulfate drying agent
- Add sodium hydrogen arbonate to remove acid washing.
- Transfer to separating funnel. Seperate layers formed by pouring off bottom layer/ decanting
- Continually remove bung and release pressure whilst swirling
- Add HCl in a conical flask then anhydrous calcium carbonate takes unreacted alcohol
- Lower boliling point than reactant
- Cannot form hydrogen bonds
- Producing a pure sample of 2-Chloro-2-methyl-propane
- Find the concentration of a solution of sodium hydroxide
- Known concentration of acid titrated against sodium hydroxide
- Dissolve known mass of salfamic acid into 250cm3 volumetric flask
- Methyl orange indicator
- Clock reaction rate equation
- varying changes on peroxodisulfate and iodide ions
- Rate vs Conc graph plotted
- Enthalpy change for thermal decomposition of potassium hydrogencarbonate
- Uses Hess's law cannot be measured directly
- High reacting temperature means water no longer under standard conditions
- High temp beraks down Na2CO3 the product
- Using HCl in excess
- Polystyrene cup to redduce temperature loss or gain improving accuracy
- Uses Hess's law cannot be measured directly
- Preparing a transition metal complex
- hydrated copper sulfate to tetraammine copper(ii) sulfate
- React in ethanol and buchner funnel with cold ethanol
- Iron in iron tablet, Redox titration
- Iron Fe2+ against MnO4-
- Colourless to pink
- Crush tablet and react with H2SO4
- Filter wash add to volumetric flask
- Pipette titrate until just pink
- Filter wash add to volumetric flask
- Iron Fe2+ against MnO4-
- Identifying unknowns
- Potassium chromate oxidises
- Orange to green
- Aldehyde / alcohol
- Silver Nitrate
- Chloride / Bromide / Iodide
- Precipitate white cream yellow
- Nitric acid added
- Destroys carbonate ions
- Chloride / Bromide / Iodide
- Fehilings
- Blue to red
- Aldehyde
- Blue to red
- Bromine water
- Decolourises
- Alkene
- Decolourises
- Flame test
- E=hf
- Ba Green Na Yellow K Lilac Li Red Cu Green Ca Red Sr Red Mg Be N/A
- E=hf
- Chlorine water
- Decolourise
- Shows bromine ion
- Decolourise
- Barium Chloride
- Insoluble ppt
- Test for sulphate ion
- BaSO3 dissoleves in excess HCl
- Test for sulphate ion
- Insoluble ppt
- Sodium hydroxide
- Identifies metal ion colour ppt
- In excess Cr redisolves
- Identifies metal ion colour ppt
- Potassium chromate oxidises
- Measure the molar volume of a gas
- Volume of 1mol gas
- Gas collection in water with measuring cylinder
- Collection with gas syringe
- Physical divide between reactants before combining in tube
- Error from not getting lid on in time
- Cakcium calbonate vs volume produced graph
- Ethanoic acid and Calcium carbonate
- Volume of 1mol gas
- Synthesise aspirin
- Reaction of ACID ANHYDRIDE
- from 2-hydroxybenzoic acid
- Warm using water bath
- Add ice to break down unreacted anhydride
- Form ppt then buchner funnel
- wash crystals min amount of water
- Filter and dry
- wash crystals min amount of water
- Measure melting temp and range
- impurities wet
- Reaction of ACID ANHYDRIDE
- Electrochemical cells
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