the anions we were testing for could only be determined from one specific result for example if a black precipitate formed following the tests the substance is therefore a sulphide however the same result would also show the presence of carbonate and hydrogen carbonate this therefore means that it is difficult to distinguish between the two and therefore further tests would need to be carried out this test enables you to distinguish clearly between the two and includes adding a drop of phenolphthalein
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Salts – Reactions with Acids: Learn these General Equations and their Examples: 1. ACID + METAL –––––––> SALT + HYDROGEN Hydrochloric acid + Magnesium Magnesium Chloride + Hydrogen 2HCl(aq) + 2Mg(s) 2MgCl(aq) + H2(g) Sulphuric acid + Zinc Zinc Sulphate + Hydrogen H2SO4(aq) + Zn(s) ZnSO4(aq) + H2(g) Nitric acid + Aluminium Aluminium Nitrate + Hydrogen 2HNO3(aq) + 2Al(s) 2AlNO3(aq) + H2(g) 2. ACID + BASE –––––––> SALT + WATER Hydrochloric acid + Copper
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typical properties of bases. Materials: * * Goggles * Well plate * 2 strips of magnesium ribbon * Sodium hydrogen carbonate (baking soda)‚ NAHCO3 * Red litmus paper * Blue litmus paper * Conductivity tester * Beakers of: * Tap water * Dilute bromothymol blue indicator * Dilute hydrochloric acid * Dilute sodium hydroxide * Eye droppers * Unknown acids and bases * Phenolphthalein Procedure: 1. A data table was
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the neutralization reaction of an acid and a base. They are composed of related numbers of cations (positively charged ions) and anions (negative ions) so that the product is electrically neutral (without a net charge). Salts can appear to be clear and transparent (sodium chloride)‚ opaque‚ and even metallic and lustrous (iron disulfide). In many cases the apparent opacity or transparency are only related to the difference in size of the individual monocrystals. Now examples of using salts in our daily life with some
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Acetate formula | CH3COO- | 5 | Ammonia formula | NH3 | 6 | Nitric acid formula | HNO3 | 7 | Phosphoric acid formula | H3PO4 | 8 | Sodium phosphate formula | Na3PO4 | 9 | Calcium carbonate formula | CaCO3 | 10 | Ammonium sulfate formula | (NH4)2SO4 | 11 | Carbonic acid formula | H2CO3 | 12 | Sodium bicarbonate formula | NaHCO3 | 13 | Sodium hydroxide formula | NaOH | 14 | Calcium hydroxide formula | Ca(OH)2 | 15 | Ethanol formula | C2H5OH | 16 | Hydrobromic acid formula |
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damage will cause further damage and evolve noxious fumes. When there is solution or concentrated acid has been accidentally spilled on the bench or floor‚ the spill area may need to be isolated and can be neutralized with commonly used Sodium Bicarbonate. Sodium bicarbonate is good to minimize acid/base spills due to its amphiprotic nature and There are many advantages of using neutralization reactions including the ability to change can be used in laboratories to clean up after acids
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1. Identify the natural sources of sulphur dioxide and oxides of nitrogen. SO2‚ natural: - Geothermal hot springs and volcanic activity are natural sources of SO2. - In the process of decaying of organic matter some bacteria will produces hydrogen sulphide as a waste product which will oxidise‚ forming so2. - Phytoplankton release dimethyl sulphide (DMS) into the atmosphere‚ when this is oxidised it forms sulphuric acid. NOx‚ natural: - Lightning activity generates high temperatures to allow
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KMnO4 Potassium Manganate (VII) 10 Cu(OH)2 Copper (II) Hydroxide 11 FeSO4 Iron (II) Sulfate 12 NH4Cl Ammonium Chloride 13 ZnCO3 Zinc Carbonate 14 SnF2 Tin (II)Fluoride 15 MgSO4 Magnesium Sulfate 16 MnO2 Manganese (IV) Oxide 17 Ca3(PO4)2 Tricalcium Phosphate 18 NaOH Sodium Hydroxide 19 HCl Hydrogen Cloride 20 Ba(HSO3)2 Barium Bisulfite 21 HNO3 Hydrogen Nitrate 22 FeSO3 Iron (II) Sulfite 23 Al2S3 Aluminum Sulfide 24 KNO3 Potassium Nitrate Part B Write the formulas for the following
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fossil fuels are said to be this as we are using them up faster than they can be made Finite- these will run out if we continue using them Crude oil This fossil fuel is made up of a mixture of hydrocarbons. Hydrocarbons are compounds that contain hydrogen and oxygen atoms only a) b) In the exam you may be asked to identify hydrocarbons from their structure. You can see that a) is not a hydrocarbon as it contains oxygen as well Crude oil on its own is not useful but the hydrocarbons
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Problems‚ Chapters 1–3 Chapter 1 – Chemistry: The Study of Change 1. Element‚ compound‚ homogeneous mixture (solution)‚ or heterogeneous mixture: a) orange juice b) brass c) 0.9% saline (NaCl) solution d) garden soil e) room air f) methane gas g) sodium metal h) N2 gas i) Cu(NO3)2 crystals (freshly-squeezed) 2. Define (some of these terms are found in Chapters 2 and 3): a) c) e) g) i) k) m) o) 3. b) d) f) h) j) l) n) compound physical change law of conservation of mass extensive properties
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