Unit 1 Flashcards
Homogenous mixture
- Uniform and evenly distributed structure of composition
- Components not separated or distinguished
Heterogenous mixture
- Distinct substances without uniform composition
- Components remain separate from each other
Reaction of metal and water
Metal + Water -> Metal Hydroxide + H2
Reaction of Metal and acid
Metal + Acid -> Salt + H2
Reaction of Metal oxide and water
Metal Oxide + Water -> Metal hydroxide
Reaction of Metal oxide and acid
Metal oxide + Acid -> Salt + Water
Decomposition of carbonic acid
Carbonic Acid -> Water + Carbon Dioxide
Thermal decomposition of metal carbonate
Metal Carbonate -> CO2 + Metal Oxide
Thermal decomposition of Metal bicarbonate
Metal Bicarbonate -> H2O + CO2 + Metal Carbonate
Reaction of Metal Carbonate and Acid
Metal Carbonate + Acid -> Salt + H2O + CO2
Reaction of Metal Bicarbonate and Acid
Metal Bicarbonate + Acid -> Salt + H2O + CO2
Titration steps
1) Measuring a known volume of one of the solutions and placing into conical flask
2) Other solution placed in burette
3) A few drops of the indicator are added
4) The tap on the burette is carefully opened and the solution added to the conical flask until the indicator just changes colour
5) Multiple trials are carried out until concordant results are obtained
Back titration purpose
To find % purity of a substance from impure material using titration
Given:
- Mass of a substance
- Initial volume and concentration of analyte
Back titration steps
1) Initial volume of Analyte = Concentration * Volume of Analyte
2) Titrate remaining moles of analyte, after reacting with impure substance
3) Moles of analyte reacted with the impure substance (Initial mole of analyte - Remaining mole of analyte)
4) Moles of substance in impure material, reacted with the titrant = mole of analyte reacted * mole ratio between analyte and substance
Limiting / Excess Reactant
Limiting: Reactant used up first and determines amount of product produced
Excess: A reactant that remains after reaction is finished
Conditions of ideal gases
- No interaction between gas particles
- Ideal gases are point particles (no volume)
- No energy loss after ideal gases collide with each other
- Real gases show ideal behavior at low pressure, high temp
Avogadro’s law
Under same temperature and pressure, volume of gas is proportional to the moles
Elements
substances made from one kind of atom, they take part in chemical reactions in which new substances are made in processes that most often involve an energy change
Compounds
made from two or more elements chemically combined, atoms combine together in fixed ratios that will give them full outer shells of electrons, producing compounds
Mixtures
elements and compounds are interspersed with each other, but are not chemically combined. Components of a mixture retain the same characteristic properties as when they are in their pure form
Solvation / Filtration
Used to separate an undissolved solid from a mixture of the solid and a liquid / solution
1) Filter paper is placed in a filter funnel above another beaker
2) The mixture of insoluble solid and liquid is poured into the filter funnel
3) Filter paper will only allow small liquid particles to pass through in the filtrate
4) Solid particles are too large to pass through the filter paper so will stay behind as a residue
Crystallization
Used to separate a dissolved solid from a solution
1) The solution is heated, allowing the solvent to evaporate and leaving a saturated solution behind
2) You can test if the solution is saturated by dipping a clean, dry, cold glass rod into the solution. If saturated, crystals will form on glass rod
3) allowed to cool slowly and solids will come out of the solution as the solubility decreases, and crystals will grow
4) Crystals are collected by filtering the solution
5) Washed with distilled water to remove any impurities
Recrystalization
used to purify impure solids
1) hot solvent is used to dissolve both the organic solid and the impurities and then as the solution cools the solid crystallizes out and leaves behind the impurities in the solution
2) minimum amount of solvent to dissolve the solid and avoid loss of the product
3) If any solid impurities remain in the solution, a hot filtration can be carried out
4) once the solution has cooled down to room temperature and crystallised then the product crystals can be recovered by filtration
Simple Distillation
Used to separate a liquid and soluble solid from a solution
1) The solution is heated and pure water evaporates producing a vapour which rises through the neck of the round-bottomed flask
2) The vapour passes through the condenser, where it cools and condenses, turning into pure water which is collected in a beaker
3) After all the water is evaporated from the solution, only the solid solute will be left behind
