Robert Pickett Wildlife Photography

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  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38405RKP.jpg
  • Experiment showing stages of Magnesium strip burning in flame
    38253RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38410RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38408RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38407RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38406RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38404RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38401RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38402RKP.jpg
  • Titration experiment to measure the volume of acid needed to neutralize an alkaline solution. The alkaline solution is in the conical flask (bottom centre) and its alkalinity is indicated by the use of phenolphthalein indicator from the bottle. This indicator turns pink in an alkaline solution and colourless in an acidic solution. The acid is in the burette, the volume-measuring apparatus held over the flask. The tap (lower centre) is used to add acid until a colourless solution forms at the reaction endpoint. This acid volume is compared to the known volume of alkali, giving information on reaction chemistry and chemical concentrations.
    38317RKP.jpg
  • Titration experiment to measure the volume of acid needed to neutralize an alkaline solution. The alkaline solution is in the conical flask (bottom centre) and its alkalinity is indicated by the use of phenolphthalein indicator from the bottle. This indicator turns pink in an alkaline solution and colourless in an acidic solution. The acid is in the burette, the volume-measuring apparatus held over the flask. The tap (lower centre) is used to add acid until a colourless solution forms at the reaction endpoint. This acid volume is compared to the known volume of alkali, giving information on reaction chemistry and chemical concentrations.
    38316RKP.jpg
  • Experiment showing stages of Magnesium strip burning in flame
    38256RKP.jpg
  • Experiment showing stages of Magnesium strip burning in flame
    38255RKP.jpg
  • Experiment showing stages of Magnesium strip burning in flame
    38254RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38411RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38409RKP.jpg
  • Sequence Experiment to demonstrate the extremely violent reaction of thermite when ignited. Thermite is a pyrotechnic composition of a metal powder and a metal oxide, which produces an exothermic reaction known as a thermite reaction. The reaction is not explosive, but can create bursts of extremely high temperatures focused on a very small area for a short period of time. Thermites can have a diverse class of compositions using any of a variety of metals and oxides. The most common is aluminium with iron(III) oxide.
    38403RKP.jpg
  • Titration experiment to measure the volume of acid needed to neutralize an alkaline solution. The alkaline solution is in the conical flask (bottom centre) and its alkalinity is indicated by the use of phenolphthalein indicator from the bottle. This indicator turns pink in an alkaline solution and colourless in an acidic solution. The acid is in the burette, the volume-measuring apparatus held over the flask. The tap (lower centre) is used to add acid until a colourless solution forms at the reaction endpoint. This acid volume is compared to the known volume of alkali, giving information on reaction chemistry and chemical concentrations.
    38315RKP.jpg
  • Titration experiment to measure the volume of acid needed to neutralize an alkaline solution. The alkaline solution is in the conical flask (bottom centre) and its alkalinity is indicated by the use of phenolphthalein indicator from the bottle. This indicator turns pink in an alkaline solution and colourless in an acidic solution. The acid is in the burette, the volume-measuring apparatus held over the flask. The tap (lower centre) is used to add acid until a colourless solution forms at the reaction endpoint. This acid volume is compared to the known volume of alkali, giving information on reaction chemistry and chemical concentrations.
    38314RKP.jpg
  • Reading a burette. A burette is a vertical, cylindrical piece of laboratory glassware, with a volumetric graduation marked along its full length. A precision tap, or stopcock, on the bottom allows highly accurate control over the release of liquid contained within the burette. Burettes are used to dispense known amounts of a liquid in experiments where precise measurements are necessary, such as a titration experiment.
    38319RKP.jpg
  • Reading a burette. A burette is a vertical, cylindrical piece of laboratory glassware, with a volumetric graduation marked along its full length. A precision tap, or stopcock, on the bottom allows highly accurate control over the release of liquid contained within the burette. Burettes are used to dispense known amounts of a liquid in experiments where precise measurements are necessary, such as a titration experiment.
    38318RKP.jpg
  • Experiement items for testing elements in water, Lithium, Sodium & Potassium, with Universal Indicator and colour chart, plus safety goggles and safety screen around bowl of water
    38299RKP.jpg
  • Fat test. Test tube containing a fatty emulsion (suspension of one liquid in another) floating on top of water. This test is used to identify fats in food. A sample of a food stuff is mixed with bromine and added to water. If the emulsion floats on top of the water, fat is present.
    38354RKP.jpg
  • Fat test. Test tube containing a fatty emulsion (suspension of one liquid in another) floating on top of water. This test is used to identify fats in food. A sample of a food stuff is mixed with bromine and added to water. If the emulsion floats on top of the water, fat is present.
    38355RKP.jpg
  • Alkene test - result of testing for an alkene  with bromine water (brown). The positive result (left, clear) is the decolorization of the bromine water by the alkene. No reaction occurs at right, as the alkane  fails to decolorize the bromine water.
    38351RKP.jpg
  • Alkene test - result of testing for an alkene  with bromine water (brown). The positive result (left, clear) is the decolorization of the bromine water by the alkene. No reaction occurs at right, as the alkane  fails to decolorize the bromine water.
    38350RKP.jpg
  • Burning spirits to show different energy consumption
    38313RKP.jpg
  • Showing set up for burning magnesium in bunsen burner flame
    38251RKP.jpg
  • Showing set up for burning magnesium in bunsen burner flame
    38252RKP.jpg
  • Experiement - Lab Technician dropping Lithiumin into water, showing reaction  Lithium (Li) is a highly reactive metallic element. It is light enough to float on water, with which it reacts violently to produce hydrogen (H2) gas and lithium hydroxide (LiOH). Bubbles of H2 can be seen around the piece of metal
    38302RKP.jpg
  • Experiement - Lab Technician dropping Universal Indicator into water with Lithiumin previously added.  Water Turns blue and is compated to chart for reference.  Lithium (Li) is a highly reactive metallic element. It is light enough to float on water, with which it reacts violently to produce hydrogen (H2) gas and lithium hydroxide (LiOH). Bubbles of H2 can be seen around the piece of metal
    38304RKP.jpg
  • Experiement - Lab Technician dropping Universal Indicator into water with Lithiumin previously added.  Water Turns blue and is compated to chart for reference.  Lithium (Li) is a highly reactive metallic element. It is light enough to float on water, with which it reacts violently to produce hydrogen (H2) gas and lithium hydroxide (LiOH). Bubbles of H2 can be seen around the piece of metal
    38303RKP.jpg
  • Experiement - Lab Technician dropping Lithiumin into water, showing reaction  Lithium (Li) is a highly reactive metallic element. It is light enough to float on water, with which it reacts violently to produce hydrogen (H2) gas and lithium hydroxide (LiOH). Bubbles of H2 can be seen around the piece of metal
    38301RKP.jpg
  • Experiement - Lab Technician dropping Lithiumin into water, showing reaction  Lithium (Li) is a highly reactive metallic element. It is light enough to float on water, with which it reacts violently to produce hydrogen (H2) gas and lithium hydroxide (LiOH). Bubbles of H2 can be seen around the piece of metal
    38300RKP.jpg
  • Saponification is an exothermic (gives off heat) chemical reaction that occurs when fats or oils (fatty acids) come into contact with lye (a base.) Saponification literally means turning into soap
    38392RKP.jpg
  • Saponification is an exothermic (gives off heat) chemical reaction that occurs when fats or oils (fatty acids) come into contact with lye (a base.) Saponification literally means turning into soap
    38390RKP.jpg
  • Saponification is an exothermic (gives off heat) chemical reaction that occurs when fats or oils (fatty acids) come into contact with lye (a base.) Saponification literally means turning into soap
    38393RKP.jpg
  • Saponification is an exothermic (gives off heat) chemical reaction that occurs when fats or oils (fatty acids) come into contact with lye (a base.) Saponification literally means turning into soap
    38391RKP.jpg
  • Lab Technician universal indicator to water after previously adding Sodium. Water turns colour and is then checked against chart for reference.
    38307RKP.jpg
  • Lab Technician universal indicator to water after previously adding Sodium. Water turns colour and is then checked against chart for reference.
    38308RKP.jpg
  • Magnetic field. Bar magnet underneath sheet of paper with iron filings aligned around it. The magnetic field induces magnetism in each of the filings, which then line up in the field. Although the field is actually continuous, interactions between the filings cause them to accumulate in thin arcing lines
    38236RKP.jpg
  • Can evacuated by vacuum pump - a can is attached to a vacuum pump. The pump has removed air from the can. The pressure differential between the inside and outside of the can caused it to be crushed.
    38298RKP.jpg
  • Boiling water in a conical flask being heated by a bunsen burner. Pure water boils at a temperature of 100 degrees celsius in the standard atmospheric pressure of 101. 325 kilopascals. The boiling point may be raised by an increased atmospheric pressure or the presence of impurities in the water. The boiling point may be reduced by a low atmospheric pressure.
    38419RKP.jpg
  • Boiling water in a conical flask being heated by a bunsen burner. Pure water boils at a temperature of 100 degrees celsius in the standard atmospheric pressure of 101. 325 kilopascals. The boiling point may be raised by an increased atmospheric pressure or the presence of impurities in the water. The boiling point may be reduced by a low atmospheric pressure.
    38416RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38382RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38381RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38380RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38377RKP.jpg
  • Showing the effect of bubbling carbon dioxide gas through lime water. The lime water is saturated calcium hydroxide solution (Ca(OH)2) which reacts with carbon dioxide (CO2) to precipitate solid calcium carbonate (CaCO3). This turns the lime water cloudy (right) from its initially clear state (left).
    38376RKP.jpg
  • Showing the effect of bubbling carbon dioxide gas through lime water. The lime water is saturated calcium hydroxide solution (Ca(OH)2) which reacts with carbon dioxide (CO2) to precipitate solid calcium carbonate (CaCO3). This turns the lime water cloudy (right) from its initially clear state (left).
    38373RKP.jpg
  • Hydrated Copper Sulphate in left hand tube (blue) and un-hydrated copper sulphate in right hand tube (white) Adding water to de-hydrated copper sulphate. Water being added to a test tube containing de-hydrated (anhydrous) copper (II) sulphate (CuSO4, white). The copper (II) sulphate forms hydration bonds with the water in an exothermic (heat-producing) reaction, resulting in hydrated copper (II) sulphate (blue).
    38368RKP.jpg
  • Hydrated Copper Sulphate in left hand tube (blue) and un-hydrated copper sulphate in right hand tube (white) Adding water to de-hydrated copper sulphate. Water being added to a test tube containing de-hydrated (anhydrous) copper (II) sulphate (CuSO4, white). The copper (II) sulphate forms hydration bonds with the water in an exothermic (heat-producing) reaction, resulting in hydrated copper (II) sulphate (blue).
    38366RKP.jpg
  • Hydrated Copper Sulphate in left hand tube (blue) and un-hydrated copper sulphate in right hand tube (white) Adding water to de-hydrated copper sulphate. Water being added to a test tube containing de-hydrated (anhydrous) copper (II) sulphate (CuSO4, white). The copper (II) sulphate forms hydration bonds with the water in an exothermic (heat-producing) reaction, resulting in hydrated copper (II) sulphate (blue).
    38365RKP.jpg
  • Hydrated Copper Sulphate in left hand tube (blue) and un-hydrated copper sulphate in right hand tube (white) Adding water to de-hydrated copper sulphate. Water being added to a test tube containing de-hydrated (anhydrous) copper (II) sulphate (CuSO4, white). The copper (II) sulphate forms hydration bonds with the water in an exothermic (heat-producing) reaction, resulting in hydrated copper (II) sulphate (blue).
    38364RKP.jpg
  • Paper Chromatography of Ink. Chromatography is an analytical process, which separates a compound into its constituent chemicals. Chromatography paper is dipped vertically in a solvent with the ink painted on it. Capillary action draws the solvent up through the paper and dissolves the ink. As the solvent travels up the paper it takes the various chemicals in the ink with it, separating them into a series of colored bands.
    38357RKP.jpg
  • Iodine test for starch. Test tubes before (left) and right (after) showing a black colour that is the positive result of the test for starch using iodine. The starch  is a long coiled molecule. Iodine combines with the starch and ends up in the coil, which is why the iodine turns from light brown to black.
    38353RKP.jpg
  • Iodine test for starch. Test tubes before (left) and right (after) showing a black colour that is the positive result of the test for starch using iodine. The starch  is a long coiled molecule. Iodine combines with the starch and ends up in the coil, which is why the iodine turns from light brown to black.
    38352RKP.jpg
  • This device is used to measure voltage. Voltage is the potential difference, also called the electromotive force, measured between two points in a flow of electric current. It can be thought of as a measure of the force of the current, and is closely related to the resistance of the circuit and the amount of current. The relative power of batteries is measured in terms of their voltage. This is a digital voltmeter, displaying the voltage as digits on an LCD (liquid crystal display) screen
    38343RKP.jpg
  • Universal indicator paper. This paper is used to measure the strength of an acid or an alkali. When the paper is dipped into a solution, it changes colour depending on the solution's pH. pH is a logarithmic measure of hydrogen ion concentration. Acid solutions have a high concentration of hydrogen ions, while alkali solutions have a low concentration of hydrogen ions.
    38326RKP.jpg
  • pH measurement. Electrometrical measurement of the pH of water. The pH of a solution is a measure of the amount of free hydrogen ions present. This indicates acidity and alkalinity. The more free ions present, the more acidic the solution is said to be. pH is measured on an inverse scale: the smaller the number, the more acidic the solution. Here, the pH meter is showing 5.48, indicating weakly acidic water. The scale runs from 0-14, with pure (distilled and deionised) water considered neutral at pH 7. There are several reasons why water may deviate from pH 7, including the presence of dissolved salts and gases.
    38325RKP.jpg
  • Magnesium metal reacts with oxygen to form magnesium oxide.
    38297RKP.jpg
  • Bromine gas diffusion. Bromine vapour (orange) filling the lower of two gas jar before the seal between them is removed to demonstrate gas diffusion. Because gas molecules can move independently of each other and do so randomly, a gas spreads out from its source in a process called diffusion. The diffusion rate depends mainly on the temperature and the medium through which the diffusion takes place. In this case, the medium is air. The gas colour allows the diffusion to be observed. Sequence 1 of 4
    38292RKP.jpg
  • Sodium reacting with chlorine to form sodium chloride (NaCl, common salt). A burning piece of the alkali metal sodium (Na) has a gas jar containing the halogen gas chlorine (Cl2) placed over it.  The reaction is violent and exothermic (heat-releasing).
    38291RKP.jpg
  • Sodium reacting with chlorine to form sodium chloride (NaCl, common salt). A burning piece of the alkali metal sodium (Na) has a gas jar containing the halogen gas chlorine (Cl2) placed over it.  The reaction is violent and exothermic (heat-releasing).
    38290RKP.jpg
  • Sodium reacting with chlorine to form sodium chloride (NaCl, common salt). A burning piece of the alkali metal sodium (Na) has a gas jar containing the halogen gas chlorine (Cl2) placed over it.  The reaction is violent and exothermic (heat-releasing).
    38286RKP.jpg
  • Magnesium burns in chlorine
    38283RKP.jpg
  • Flame test. Potassium burning in the flame of a bunsen burner producing a lilac flame. The colour of the flame is caused by electrons that have been excited to a higher energy state. When they relax they emit energy in the form of a characteristic wavelength of light. The colour of the flame is different for different elements and can be used to identify unknown substances.
    38270RKP.jpg
  • Lithium burning in the flame of a bunsen burner producing a pink/red flame. The colour of the flame is caused by electrons that have been excited to a higher energy state. When they relax they emit energy in the form of a characteristic wavelength of light. The colour of the flame is different for different elements and can be used to identify unknown substances.
    38269RKP.jpg
  • Bunsen Burner with hot flame - blue
    38264RKP.jpg
  • Flame test for copper. A compound containing the element copper (symbol Cu) produces a characteristic blue-green flame when heated in a bunsen burner. This colour is produced when copper electrons give off extra energy as a specific type of radiation (in this case it is visible light but it can be radio waves or gamma rays). This distinct energy release is known as an emission spectrum. Each element has its own emission spectrum, which allows it to be identified in different materials.
    38267RKP.jpg
  • Flame test. Barium burning in the flame of a bunsen burner producing a green flame. The colour of the flame is caused by electrons that have been excited to a higher energy state. When they relax they emit energy in the form of a characteristic wavelength of light. The colour of the flame is different for different elements and can be used to identify unknown substances.
    38265RKP.jpg
  • Bunsen Burner with Medium flame - yellow to blue
    38262RKP.jpg
  • Bunsen Burner with Medium flame - yellow to blue
    38261RKP.jpg
  • Electromagnet - picking up paper clips.  When electric current is passed through the wire, a magnetic field is produced, attracting steel paper clips
    38238RKP.jpg
  • Boiling water in a conical flask being heated by a bunsen burner. Pure water boils at a temperature of 100 degrees celsius in the standard atmospheric pressure of 101. 325 kilopascals. The boiling point may be raised by an increased atmospheric pressure or the presence of impurities in the water. The boiling point may be reduced by a low atmospheric pressure.
    38420RKP.jpg
  • Boiling water in a conical flask being heated by a bunsen burner. Pure water boils at a temperature of 100 degrees celsius in the standard atmospheric pressure of 101. 325 kilopascals. The boiling point may be raised by an increased atmospheric pressure or the presence of impurities in the water. The boiling point may be reduced by a low atmospheric pressure.
    38418RKP.jpg
  • Boiling water in a conical flask being heated by a bunsen burner. Pure water boils at a temperature of 100 degrees celsius in the standard atmospheric pressure of 101. 325 kilopascals. The boiling point may be raised by an increased atmospheric pressure or the presence of impurities in the water. The boiling point may be reduced by a low atmospheric pressure.
    38417RKP.jpg
  • Benedict's reagent reacting with sugars. It is a blue coloured solution, which is a mixture containing copper sulphate. It is used in biochemistry as a test for the presence of sugars. It reacts with sugars, such as glucose, to form an orange precipitate.
    38415RKP.jpg
  • Benedict's reagent reacting with sugars. It is a blue coloured solution, which is a mixture containing copper sulphate. It is used in biochemistry as a test for the presence of sugars. It reacts with sugars, such as glucose, to form an orange precipitate.
    38414RKP.jpg
  • Benedict's reagent reacting with sugars. It is a blue coloured solution, which is a mixture containing copper sulphate. It is used in biochemistry as a test for the presence of sugars. It reacts with sugars, such as glucose, to form an orange precipitate.
    38413RKP.jpg
  • Benedict's reagent reacting with sugars. It is a blue coloured solution, which is a mixture containing copper sulphate. It is used in biochemistry as a test for the presence of sugars. It reacts with sugars, such as glucose, to form an orange precipitate.
    38412RKP.jpg
  • Parafin oil being poured into a beaker as a demonstration of its viscosity. Viscosity is the internal resistance of a fluid to the flow of that fluid.
    38398RKP.jpg
  • Parafin oil being poured into a beaker as a demonstration of its viscosity. Viscosity is the internal resistance of a fluid to the flow of that fluid.
    38397RKP.jpg
  • Parafin oil being poured into a beaker as a demonstration of its viscosity. Viscosity is the internal resistance of a fluid to the flow of that fluid.
    38396RKP.jpg
  • Parafin oil being poured into a beaker as a demonstration of its viscosity. Viscosity is the internal resistance of a fluid to the flow of that fluid.
    38395RKP.jpg
  • Electrolysis is the use of an electrical current to decompose a chemical, in this case water. Reactions at the two electrodes are powered by an electric current. Oxygen and hydrogen gas bubbles are evolved at the anode and cathode respectively. As water molecules consist of two hydrogen atoms and one oxygen atom, twice as much hydrogen as oxygen is trapped in the test tubes
    38389RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38387RKP.jpg
  • Electrolysis is the use of an electrical current to decompose a chemical, in this case water. Reactions at the two electrodes are powered by an electric current. Oxygen and hydrogen gas bubbles are evolved at the anode and cathode respectively. As water molecules consist of two hydrogen atoms and one oxygen atom, twice as much hydrogen as oxygen is trapped in the test tubes
    38388RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38386RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38385RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38383RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38384RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38379RKP.jpg
  • The precipitates are a result of using silver nitrate to test for halogen ions. The colour of the precipitate depends on the halogen present, chloride is white, bromide pale cream and iodide pale yellow.
    38378RKP.jpg
  • Showing the effect of bubbling carbon dioxide gas through lime water. The lime water is saturated calcium hydroxide solution (Ca(OH)2) which reacts with carbon dioxide (CO2) to precipitate solid calcium carbonate (CaCO3). This turns the lime water cloudy (right) from its initially clear state (left).
    38374RKP.jpg
  • Showing the effect of bubbling carbon dioxide gas through lime water. The lime water is saturated calcium hydroxide solution (Ca(OH)2) which reacts with carbon dioxide (CO2) to precipitate solid calcium carbonate (CaCO3). This turns the lime water cloudy (right) from its initially clear state (left).
    38375RKP.jpg
  • Showing the effect of bubbling carbon dioxide gas through lime water. The lime water is saturated calcium hydroxide solution (Ca(OH)2) which reacts with carbon dioxide (CO2) to precipitate solid calcium carbonate (CaCO3). This turns the lime water cloudy (right) from its initially clear state (left).
    38371RKP.jpg
  • Showing the effect of bubbling carbon dioxide gas through lime water. The lime water is saturated calcium hydroxide solution (Ca(OH)2) which reacts with carbon dioxide (CO2) to precipitate solid calcium carbonate (CaCO3). This turns the lime water cloudy (right) from its initially clear state (left).
    38372RKP.jpg
  • Showing the effect of bubbling carbon dioxide gas through lime water. The lime water is saturated calcium hydroxide solution (Ca(OH)2) which reacts with carbon dioxide (CO2) to precipitate solid calcium carbonate (CaCO3). This turns the lime water cloudy (right) from its initially clear state (left).
    38370RKP.jpg
  • Showing the effect of bubbling carbon dioxide gas through lime water. The lime water is saturated calcium hydroxide solution (Ca(OH)2) which reacts with carbon dioxide (CO2) to precipitate solid calcium carbonate (CaCO3). This turns the lime water cloudy (right) from its initially clear state (left).
    38369RKP.jpg
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