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18 Cards in this Set
- Front
- Back
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Describe: neutral
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Neither acidic nor alkaline; neutral solutions have a pH of 7
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Describe: acidic
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Has a pH less than 7; an acidic solution contains hydrogen ions
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Describe: Alkaline
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Has a pH above 7; alkaline solutions contain hydroxide ions
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Classify: Oxides
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...as either acidic or basic, realted to metallic and non-metallic character of the other element.
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Describe: The characteristic between acids and metals, bases (including alkalis) and carbonates
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-When an acid reacts with a metal, hydrogen is displaced, leaving a salt in solution
-When an acid and an alkali react, salt and water are formed -When an acid and a metal oxide react, a salt and water are formed -When an acid and a metal carbonate react, salt, water and carbon dioxide are formed -An acid and a metal react in order to form a metal salt and hydrogen -An acid and a metal oxide or hydroxide form a metal salt and water -An acid and a metal carbonate form a metal salt, water and carbon dioxide |
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Describe: The importance of controlling acidity in the environment (air,water and soil)
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-Plants prefer a neutral pH of 7 to grow in. Therefore, if the soil, is too acidic many plants will not grow. Soil acidity is contolled by treating the soil with a base, such as limestone, quick lime or slaked lime.
-Liquid factory waste also often contains acid, which can harm the environment as it flows into rivers etc. Therefore, the factory waste is often treated with slaked lime -As fossil fuels are burned to generate energy, waste gases are released into the atmosphere, such as sulphur dioxide and oxides of nitrogen. These waste gases combine with water and the air in order to form acids and therefore acid rain. Acid rain can erode buildings and other infastructure and damages the soil, plants and lakes etc. as well. |
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Classify: Oxides as either acidic or basic, related to metallic and non-metallic character of the other element.
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-In general,metals react with oxygen in order to form basic oxides
-In general, non-metals react with oxygen in order to form acidic oxides |
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Test for: Ammonium
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-Add a little dilute sodium hydroxide solution and heat gently
-If ammonia gas is given off, ammonium ions were present in the solution (Ammonia gas turns red litmus blue and has a sharp smell) |
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Test for: Copper (II), Iron (II), Iron (III) and Zinc
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-Add a few drops of dilute sodium hydroxide solution
-Pale blue precipitate indicates Copper (II) -Green precipitate indicates Iron (II) -Red-brown precipitate indicates Iron (III) -Add more sodium hydroxide and ammonium hydroxide solution -If the precipitate dissolves, zinc is present |
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Test for: Carbonate ions
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-Add a little dilute hydrochloric acid
-If the mixture bubbles and gives off a gas, that turns lime water milky, carbonate ions were present |
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Test for: Chloride ions
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-Add an equal volume of dilute nitric acid
-Add silver nitrate solution -White precipitate indicates Chloride ions |
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Test for: Nitrate
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-Add a little sodium hydroxide solution
-Add some aluminium foil. Heat gently. -If ammonia gas is given off, the unknown substance contained nitrate ions. |
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Test for: Sulfate
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- Add an equal volume of dilute hydrochloric acid
- Then add barium nitrate solution - Barium sulfate is insoluble. So if sulphate ions are present a white precipitate will form |
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Test for: ammonia (gas)
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Ammonia gas has a strong sharp smell and turns red litmus blue
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Test for: carbon dioxide
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turns limewater milky
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Test for: Chlorine
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turns indicator paper white
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Test for: Hydrogen
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- collect the gas in a tube and hold a lighted splint to it
- the gas burns with a squeaky pop |
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Test for: Oxygen
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- collect the gas in a tube and hold a glowing splint to it
- the splint immediately bursts into flame |
