Term
What is the colour of:
VO3- (+5) |
|
Definition
|
|
Term
What is the colour of:
VO2+ (+5) |
|
Definition
|
|
Term
What is the colour of:
VO2+ (+4) |
|
Definition
|
|
Term
What is the colour of:
V3+ (+3) |
|
Definition
|
|
Term
What is the colour of:
V 2+ (+2) |
|
Definition
|
|
Term
What is the colour of:
Cr2O7 2- (+6) |
|
Definition
|
|
Term
What is the colour of:
CrO42- (+6) |
|
Definition
|
|
Term
What is the colour of:
Cr 3+ |
|
Definition
|
|
Term
What is the colour of:
Cr 2+ |
|
Definition
|
|
Term
What is the colour of:
[Cr(H2O)6]3+ |
|
Definition
|
|
Term
What is the colour of:
[Cr(H2O)3(OH)3] |
|
Definition
|
|
Term
What is the colour of:
[Cr(H2O)2(OH)4]- |
|
Definition
|
|
Term
What is the colour of:
[Cr(NH3)6]3+ |
|
Definition
|
|
Term
What is the colour of:
MnO4- (+7) |
|
Definition
|
|
Term
What is the colour of:
Mn 2+ |
|
Definition
|
|
Term
What is the colour of:
Fe 2+ |
|
Definition
|
|
Term
What is the colour of:
Fe 3+ |
|
Definition
|
|
Term
What is the colour of:
[Fe(H2O)3(OH)3] |
|
Definition
|
|
Term
What is the colour of:
[Fe(H2O)4(OH)2] |
|
Definition
|
|
Term
What is the colour of:
FeCO3 |
|
Definition
|
|
Term
What is the colour of:
[Co(H2O)6]2+ |
|
Definition
|
|
Term
What is the colour of:
CoCO3 |
|
Definition
|
|
Term
What is the colour of:
[Co(H2O)4(OH)2] |
|
Definition
|
|
Term
What is the colour of:
[Co(H2O)3(OH)3] |
|
Definition
|
|
Term
What is the colour of:
[Co(NH3)6]2+ |
|
Definition
| Pale yellow (precipitate) |
|
|
Term
What is the colour of:
[Co(NH3)6]3+ |
|
Definition
|
|
Term
What is the colour of:
CoCl42- |
|
Definition
|
|
Term
What is the colour of:
Cu 2+ |
|
Definition
|
|
Term
What is the colour of:
Cu+ |
|
Definition
|
|
Term
What is the colour of:
Cu2O (+1) |
|
Definition
|
|
Term
What is the colour of:
[Cu(H2O)4(OH)2] |
|
Definition
|
|
Term
What is the colour of:
[Cu(NH3)4(OH)2] |
|
Definition
|
|
Term
What is the colour of:
CuCO3 |
|
Definition
|
|
Term
What is the colour of:
CuCl42- |
|
Definition
|
|
Term
What is the colour of:
[Al(H2O)3(OH)3] |
|
Definition
|
|
Term
What is the colour of:
[Al(OH)4]- |
|
Definition
|
|
Term
| Lattice enthalpy of formation |
|
Definition
| Enthalpy change for 1 mol of a molecule from its ions in the gaseous state |
|
|
Term
|
Definition
| Enthalpy change when 1 mol of gaseous ions is converted into aqueous ions (or converted to an aqueous solution) |
|
|
Term
|
Definition
| Only ionic bonds between atoms and ions are perfect spheres |
|
|
Term
|
Definition
| Enthalpy change for the formation of 1 mol of gaseous atoms from the element in their standard states |
|
|
Term
| Enthalpy of lattice dissociation |
|
Definition
| Enthalpy change to separate 1 mol of an ionic lattice into its gaseous ions |
|
|
Term
|
Definition
| Enthalpy change when 1 mol of gaseous atoms become negatively charged ions |
|
|
Term
| Bond dissociation enthalpy as applied to chlorine |
|
Definition
| Enthalpy change to break the bond in 1 mole of chlorine molecules to form 2 moles of gaseous chlorine atoms |
|
|
Term
Why is the enthalpy of atomisation of chlorine is exactly half the bond
dissociation enthalpy of chlorine? |
|
Definition
For atomisation, only 1 mole of chlorine atoms, not 2 moles as in
bond enthalpy. |
|
|
Term
Why is the lattice dissociation enthalpy of magnesium chloride is greater than that
of calcium chloride? |
|
Definition
| The magnesium ion is smaller so attraction to the chloride ion stronger |
|
|
Term
Why is the lattice dissociation enthalpy of magnesium oxide is greater than that of
magnesium chloride? |
|
Definition
| The oxide ion has a greater charge so attracts the magnesium ion more strongly |
|
|
Term
how can the quantities of enthalpy change (ΔH), entropy change (ΔS) and
temperature (T) be used to predict whether a change is feasible. |
|
Definition
∆G = ∆H – T∆S
If ∆G is less than or equal to 0 reaction is feasible |
|
|
Term
Explain why the evaporation of water is spontaneous even though this change is
endothermic.
In your answer, refer to the change in the arrangement of water molecules and the
entropy change. |
|
Definition
The molecules become more disordered when water changes from a liquid to a gas therefore the entropy change is positive
T∆S>∆H
∆G<0 |
|
|
Term
| What would you observe when Silver ions react with Fluoride ions? |
|
Definition
| No visible change (no ppt formed). |
|
|
Term
| What would you observe when Silver ions react with Chloride ions? |
|
Definition
|
|
Term
| What would you observe when Silver ions react with Bromide ions? |
|
Definition
|
|
Term
| What would you observe when Silver ions react with iodide ions? |
|
Definition
|
|
Term
Is Silver Chloride soluble in ammonia?
If yes, what concentration of ammonia is it soluble in? |
|
Definition
|
|
Term
Is Silver Bromide soluble in ammonia?
If yes, what concentration of ammonia is it soluble in? |
|
Definition
Yes.
Concentrated ammonia. |
|
|
Term
Is Silver Iodide soluble in ammonia?
If yes, what concentration of ammonia is it soluble in? |
|
Definition
|
|
Term
What reagent would you add to test for Sulphate ions?
And what would you observe? |
|
Definition
Barium Chloride.
White ppt. |
|
|
Term
How would you test for Carbonate ions?
What reagents would you use? |
|
Definition
Acid is added to the solution containing carbonate ions.
The Carbon Dioxide bubbles that are released is then passed through limewater.
The limewater then turns from clear to cloudy. |
|
|
Term
How would you test for a primary/secondary alcohol.
What would you observe? |
|
Definition
Acidified Potassium Dichromate.
Colour change from orange to green. |
|
|
Term
How would you test for Aldehydes?
What would you observe? |
|
Definition
Tollen's Reagent: Silver mirror formed.
Heat with Fehling's Solution: Red ppt. |
|
|
Term
How would you test for Ammonia?
What would you observe? |
|
Definition
Damp litmus paper.
Colour changes to blue (from red). |
|
|
Term
How would you test for Carboxylic acids?
What would you observe? |
|
Definition
Add Sodium Carbonate solution.
Effervescence (of Carbon Dioxide). |
|
|
Term
How would you test for Magnesium ions?
What would you observe? |
|
Definition
Add Sodium Hydroxide.
White ppt |
|
|
Term
How would you test for Barium ions?
What would you observe? |
|
Definition
Add Sulphuric acid.
White ppt. |
|
|
Term
How would you test for Ammonium ions?
What would you observe? |
|
Definition
Add Sodium hydroxide (To produce ammonia).
Then test for ammonia using damp litmus paper. |
|
|
Term
| What reagent would you add to a solution including halide ions, to distinguish which halide ion it is? |
|
Definition
| Add dilute nitric acid, followed by silver nitrate solution. |
|
|
Term
How would you test for Chloride ions (solid)?
What would you observe? |
|
Definition
Add concentrated Sulphuric acid.
Misty fumes. |
|
|
Term
How would you test for Bromide ions (solid)?
What would you observe? |
|
Definition
Add concentrated Sulphuric acid.
Orange fumes and a choking gas. |
|
|
Term
How would you test for Iodide ions (solid)?
What would you observe? |
|
Definition
Add concentrated Sulphuric acid.
Purple fumes, black solid, choking gas and smell of bad eggs. |
|
|
Term
How would you test for Hydroxide ions?
What would you observe? |
|
Definition
Add Magnesium chloride solution.
White ppt. |
|
|
Term
| What can be added to sulphate ions to test for them? What would be observed? |
|
Definition
BaCl2
White precipitate formed |
|
|
Term
| What can be used to test for ammonia? What would be observed? |
|
Definition
Damp litmus paper
Colour change from red to blue |
|
|
Term
| What precipitate is formed and what is the colour of it when NaOH is added to Iron (II) chloride? |
|
Definition
|
|
Term
| How could a test to time the colour change of a solution be improved from looking at the solution in a flask? |
|
Definition
-Keep the solution at a constant temp because reaction rate is influenced by temp
-Use a colorimeter to monitor colour change which gives a more accurate time of colour change |
|
|
Term
| How could H2O2 be separated from Ba(NO3)2? |
|
Definition
| By fractional distillation |
|
|
Term
| Why would it be better to react sulphuric acid with BaO2 rather than nitric acid? |
|
Definition
| BaSO4 is insoluble so easier to separate from H2O2 |
|
|
Term
| Why can't infrared spectroscopy be used to identify H2O in a solution of H2O2? |
|
Definition
| They both contain an OH group |
|
|
Term
| Why does hydrogen peroxide decompose more quickly if it is kept in a clear glass bottle rather than a brown one? |
|
Definition
| Decomposition is accelerated by light |
|
|
Term
| Even if hydrogen peroxide is corrosive, why does a spillage not have long term effects on the environment? |
|
Definition
| Decomposition products are harmless |
|
|
Term
| What arrangement, reflux or distillation, should be used for the formation of ethanal and why? |
|
Definition
Distillation
If reflux, further oxidation would occur and ethanoic acid would be formed |
|
|
Term
| How would you ensure a reading from a pH meter is accurate? |
|
Definition
| Collaborate with a solution of a known pH and plot a collaboration curve |
|
|
Term
| How could the melting point of asprin be measured? |
|
Definition
| Put sample in capillary tube and heat in melting point apparatus |
|
|
Term
| Why should a pH meter be collaborated before use? |
|
Definition
| pH meter may get less accurate over time |
|
|
Term
| What substance is most likely to oxidise Iron (II) ions when Iron (II) sulphate is used as a weed killer? |
|
Definition
|
|
Term
| Suggest a value for the pH of a 0.100 mol dm-3 solution of Iron (II) sulphate? |
|
Definition
| Anything in the range 4.0 - 6.9 |
|
|
Term
| What is a chemical hazard when using H2SO4 and what is a safety precaution? |
|
Definition
Acid is corrosive
Use gloves or eye protection |
|
|
Term
| Why is it an advantage to add thiocyanate ions to the iron (III) sulphate solution before measuring percentage absorbance? |
|
Definition
|
|
Term
| Why is it necessary to maintain a constant temperature in an experiment to measure the equilibrium constant? |
|
Definition
| Temperature affects the equilibrium constant |
|
|
Term
| What is one method for maintaining a constant temperature in an experiment? |
|
Definition
|
|
Term
| What is observed when 1-chloropropane and ethanoyl chloride are separately added to an aqueous solution of silver nitrate? |
|
Definition
1-chloropropane - no visible change
ethanoyl chloride - white precipitate |
|
|
Term
| What equation links hydration enthalpy of Mg2+ ions and Cl- ions, lattice enthalpy and enthalpy of solution? |
|
Definition
| ∆Hsolution = ∆HL + Σ∆Hhyd Mg2+ ions + Σ∆Hhyd Cl– ions |
|
|
Term
| Using lattice enthalpy, enthalpy of solution of MgCl2 and hydration of Cl- ions, what is the equation to find the enthalpy of hydration of Mg2+ ions? |
|
Definition
| Σ∆Hhyd Mg2+ ions = ∆Hsolution - ∆HL + Σ∆Hhyd Cl– ions |
|
|
Term
| What is the equation used to calculate standard entropy change? |
|
Definition
| ∆S = ES Products - ES reactants |
|
|
Term
| What is the equation to calculate Gibbs free energy? |
|
Definition
|
|
Term
| What is the overall reaction for the Contact Process that is catalysed by Vanadium oxide? |
|
Definition
|
|
Term
| What are the two reactions for the Contact Process that is catalysed by Vanadium oxide? |
|
Definition
V2O5 + SO2 → V2O4 + SO3
V2O4 + ½O2 → V2O5 |
|
|
Term
| What two equations show how the autocatalyst is involved in the oxidation of C2O42– ions by MnO4– ions? |
|
Definition
4Mn2+ + MnO4– + 8H+ → 5Mn3+ + 4H2O
2Mn3+ + C2O42– → 2Mn2+ + 2CO2 |
|
|
Term
| Reacton for Sodium with Oxygen |
|
Definition
|
|
Term
| Reaction for Magnesium with Oxygen |
|
Definition
|
|
Term
| Reaction for Aluminium with Oxygen |
|
Definition
| 4Al(s) + 3O2 --> 2Al2O3(s) |
|
|
Term
| Reaction for Silicon with Oxygen |
|
Definition
|
|
Term
| Reaction for Phosphorus with Oxygen |
|
Definition
|
|
Term
| Reaction for Sulfur with Oxygen |
|
Definition
|
|
Term
| Reaction for Sodium Oxide with water. |
|
Definition
| Na2O(s) + H2O --> 2NaOH(aq) |
|
|
Term
| Reaction for Magnesium Oxide with water. |
|
Definition
| MgO(s) + H2O --> Mg(OH)2(s) --> Mg(OH)2 (aq) |
|
|
Term
| Reaction for Phosphorus Oxide with water. |
|
Definition
| P4O10 + 6H2O --> 4H3PO4(aq) |
|
|
Term
| Reaction for Sulfur Dioxide with water |
|
Definition
|
|
Term
| Reaction for Sulfur Trioxide with water |
|
Definition
|
|
Term
| What would be observed when Sodium burns in oxygen? |
|
Definition
|
|
Term
| What would be observed when Magnesium burns in oxygen? |
|
Definition
white flame / white light
solid / powder / smoke / ash / white fumes |
|
|
Term
| What would be observed when Aluminium burns in oxygen? |
|
Definition
|
|
Term
| What would be observed when Silicon burns in oxygen? |
|
Definition
|
|
Term
| What would be observed when Phosphorus burns in oxygen? |
|
Definition
|
|
Term
| What would be observed when Sulphur burns in oxygen? |
|
Definition
blue flame
fumes or misty or pungent/choking/smelly gas |
|
|
Term
| What is the equation for the reaction that takes place when Sodium burns in oxygen? |
|
Definition
|
|
Term
| What is the equation for the reaction that takes place when Magnesium burns in oxygen? |
|
Definition
|
|
Term
| What is the equation for the reaction that takes place when Aluminium burns in oxygen? |
|
Definition
|
|
Term
| What is the equation for the reaction that takes place when Silicon burns in oxygen? |
|
Definition
|
|
Term
| What is the equation for the reaction that takes place when Phosphorus burns in oxygen? |
|
Definition
|
|
Term
| What is the equation for the reaction that takes place when Sulphur burns in oxygen? |
|
Definition
|
|
Term
| What is the bonding in Sodium oxide? |
|
Definition
|
|
Term
| What is the bonding in Magnesium oxide? |
|
Definition
|
|
Term
| What is the bonding in Aluminium oxide? |
|
Definition
|
|
Term
| What is the bonding in Silicon oxide? |
|
Definition
|
|
Term
| What is the bonding in Phosphorus oxide? |
|
Definition
|
|
Term
| What is the bonding in Sulphur dioxide? |
|
Definition
|
|
Term
| What are the properties of Sodium? |
|
Definition
Soft, silver, shiny
Conducts electricity |
|
|
Term
| What are the properties of Magnesium? |
|
Definition
Soft, silver, shiny
Conducts electricity |
|
|
Term
| What are the properties of Aluminium? |
|
Definition
Easily malleable, silver, shiny
Conducts electricity |
|
|
Term
| What are the properties of Silicon? |
|
Definition
Hard, grey-blue solid
Partial conductor of electricity (check this) |
|
|
Term
| What are the properties of Phosphorus? |
|
Definition
Red or white solid, low melting and boiling point
Doesn't conduct electricity |
|
|
Term
| What are the properties of Sulphur? |
|
Definition
Yellow solid, low melting and boiling point
Doesn't conduct electricity |
|
|
Term
| What are the properties of Chlorine? |
|
Definition
Green gas, low melting and boiling point
Doesn't conduct electricity |
|
|
Term
| What are the properties of Argon? |
|
Definition
Colourless, odourless gas
Unreactive |
|
|
Term
| What are the observations when Sodium reacts with water? |
|
Definition
Violent reaction
Hydrogen released |
|
|
Term
| What are the observations when Magnesium reacts with water? |
|
Definition
Slow reaction
Hydrogen released |
|
|
Term
| What are the observations when Magnesium reacts with steam? |
|
Definition
Fast reaction
Hydrogen released |
|
|
Term
| What are the observations when Chlorine reacts with water? |
|
Definition
Chlorine dissolves
Hydrochloric acid formed
Chloric acid formed |
|
|
Term
| What is the equation for the reaction of Sodium with water? |
|
Definition
| 2Na(s) + 2H2O(l) -> 2NaOH(aq) + H2(g) |
|
|
Term
| What is the equation for the reaction of magnesium with water? |
|
Definition
| Mg(s) + 2H2O(l) -> Mg(OH)2(aq) + H2(g) |
|
|
Term
| What is the equation for the reaction of magnesium with steam? |
|
Definition
| Mg(s) + H2O(g) -> MgO(s) + H2(g) |
|
|
Term
| What is the equation for the reaction of Chlorine with water? |
|
Definition
| Cl2(aq) + H2O(l) <=> HClO(aq) + HCl(aq) |
|
|
Term
| What are the properties of sodium oxide? |
|
Definition
White
High melting point (1548K) |
|
|
Term
| What are the properties of the magnesium oxide? |
|
Definition
White
High melting point (3125K) |
|
|
Term
| What are the properties of the Aluminium oxide? |
|
Definition
White
High melting point (2345K) |
|
|
Term
| What are the properties of the Silicon oxide? |
|
Definition
White
High melting point (1883K) |
|
|
Term
| What are the properties of the Phosphorus oxide? |
|
Definition
|
|
Term
| What are the properties of the Sulphur oxide? |
|
Definition
| Low melting point (200 for SO2, 290K for SO3) |
|
|
Term
| What is the structure of the sodium oxide? |
|
Definition
|
|
Term
| What is the structure of the magnesium oxide? |
|
Definition
|
|
Term
| What is the structure of the aluminium oxide? |
|
Definition
|
|
Term
| What is the structure of the silicon oxide? |
|
Definition
| Giant covalent / Macromolecular |
|
|
Term
| What is the structure of the phosphorus oxide? |
|
Definition
|
|
Term
| What is the structure of the sulphur oxide? |
|
Definition
|
|
Term
| What is observed when the sodium oxide is reacted with water? |
|
Definition
Strongly alkaline solution formed
pH 13-14 |
|
|
Term
| What is observed when the magnesium oxide is reacted with water? |
|
Definition
Weakly alkaline solution formed
pH 10 |
|
|
Term
| What is observed when the aluminium oxide is reacted with water? |
|
Definition
|
|
Term
| What is observed when the silicon oxide is reacted with water? |
|
Definition
|
|
Term
| What is observed when the phosphorus oxide is reacted with water? |
|
Definition
Strongly acidic solution produced
pH 0-1 |
|
|
Term
| What is observed when sulphur dioxide is reacted with water? |
|
Definition
| Acidic solution produced pH 2-3 |
|
|
Term
| What is observed when sulphur trioxide is reacted with water? |
|
Definition
| White foggy droplets of acid form pH 0-1 |
|
|
Term
| What is the equation for reaction of water with the sodium oxide? |
|
Definition
|
|
Term
| What is the equation/s for reaction of water with the magnesium oxide? |
|
Definition
MgO + H2O -> Mg(OH)2
Mg(OH)2 -> Mg2+ + 2OH- |
|
|
Term
| What is the equation for reaction of water with the Aluminium oxide? |
|
Definition
|
|
Term
| What is the equation for reaction of water with the silicon oxide? |
|
Definition
|
|
Term
| What is the equation for reaction of water with the phosphorus oxide? |
|
Definition
|
|
Term
| What is the equation/s for reaction of water with sulphur dioxide? |
|
Definition
SO2 + H2O -> H2SO3
H2SO3 -> H+ + HSO3- |
|
|
Term
| What is the equation/s for reaction of water with sulphur trioxide? |
|
Definition
SO3 + H2O -> H2SO4
H2SO4 -> H+ + HSO4- |
|
|
Term
| What is the equation for the reaction that occurs when sodium oxide reacts with hydrochloric acid? |
|
Definition
| Na2O + 2HCl -> 2NaCl + H2O |
|
|
Term
| What is the equation for the reaction that occurs when magnesium oxide reacts with sulphuric acid? |
|
Definition
| MgO + H2SO4 -> MgSO4 + H2O |
|
|
Term
| What is the equation for the reaction that occurs when aluminium oxide reacts with sulphuric acid? |
|
Definition
| Al2O3 + 3H2SO4 -> Al2(SO4)3 + 3H2O |
|
|
Term
| What is the equation for the reaction that occurs when aluminium oxide reacts with hot, concentrated sodium hydroxide (and water)? |
|
Definition
| Al2O3 + 2NaOH + 3H2O -> 2NaAl(OH)4 |
|
|
Term
| What is the equation for the reaction that occurs when aluminium oxide reacts with hydrochloric acid? |
|
Definition
| Al2O3 + 6H+ -> 2Al3+ + 3H2O |
|
|
Term
| What is the equation for the reaction that occurs when aluminium oxide reacts with sodium hydroxide? |
|
Definition
| Al2O3 + 2OH– + 3H2O -> 2Al(OH)4– |
|
|
Term
| What is the equation for the reaction that occurs when silicon oxide reacts with hot, concentrated sodium hydroxide? |
|
Definition
| SiO2 + 2NaOH -> Na2SiO3 + H20 |
|
|
Term
| What is the equation for the reaction that occurs when phosphorus oxide reacts with hot, concentrated sodium hydroxide? |
|
Definition
| 12NaOH + P4O10 -> 4Na3PO4 + 6H2O |
|
|
Term
| What is the equation/s for the reaction that occurs when sulphur dioxide reacts with sodium hydroxide? |
|
Definition
SO2 + NaOH -> NaHSO3
NaHSO3 + NaOH -> Na2SO3 + H2O |
|
|
Term
| What can be added to sulphate ions to test for them? What would be observed? |
|
Definition
BaCl2
White precipitate formed |
|
|
Term
| What can be used to test for ammonia? What would be observed? |
|
Definition
Damp litmus paper
Colour change from red to blue |
|
|
Term
| What precipitate is formed and what is the colour of it when NaOH is added to Iron (II) chloride? |
|
Definition
|
|
Term
| How could a test to time the colour change of a solution be improved from looking at the solution in a flask? |
|
Definition
-Keep the solution at a constant temp because reaction rate is influenced by temp
-Use a colorimeter to monitor colour change which gives a more accurate time of colour change |
|
|
Term
| How could H2O2 be separated from Ba(NO3)2? |
|
Definition
| By fractional distillation |
|
|
Term
| Why would it be better to react sulphuric acid with BaO2 rather than nitric acid? |
|
Definition
| BaSO4 is insoluble so easier to separate from H2O2 |
|
|
Term
| Why can't infrared spectroscopy be used to identify H2O in a solution of H2O2? |
|
Definition
| They both contain an OH group |
|
|
Term
| Why does hydrogen peroxide decompose more quickly if it is kept in a clear glass bottle rather than a brown one? |
|
Definition
| Decomposition is accelerated by light |
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Term
| Even if hydrogen peroxide is corrosive, why does a spillage not have long term effects on the environment? |
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Definition
| Decomposition products are harmless |
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Term
| What arrangement, reflux or distillation, should be used for the formation of ethanal and why? |
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Definition
Distillation
If reflux, further oxidation would occur and ethanoic acid would be formed |
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Term
| How would you ensure a reading from a pH meter is accurate? |
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Definition
| Collaborate with a solution of a known pH and plot a collaboration curve |
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Term
| How could the melting point of asprin be measured? |
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Definition
| Put sample in capillary tube and heat in melting point apparatus |
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Term
| Why should a pH meter be collaborated before use? |
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Definition
| pH meter may get less accurate over time |
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Term
| What substance is most likely to oxidise Iron (II) ions when Iron (II) sulphate is used as a weed killer? |
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Definition
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Term
| Suggest a value for the pH of a 0.100 mol dm-3 solution of Iron (II) sulphate? |
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Definition
| Anything in the range 4.0 - 6.9 |
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Term
| What is a chemical hazard when using H2SO4 and what is a safety precaution? |
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Definition
Acid is corrosive
Use gloves or eye protection |
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Term
| Why is it an advantage to add thiocyanate ions to the iron (III) sulphate solution before measuring percentage absorbance? |
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Definition
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Term
| Why is it necessary to maintain a constant temperature in an experiment to measure the equilibrium constant? |
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Definition
| Temperature affects the equilibrium constant |
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Term
| What is one method for maintaining a constant temperature in an experiment? |
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Definition
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Term
| What is observed when 1-chloropropane and ethanoyl chloride are separately added to an aqueous solution of silver nitrate? |
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Definition
1-chloropropane - no visible change
ethanoyl chloride - white precipitate |
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