in water‚ the ions separate and become surrounded by water molecules. The focus of this experiment is on precipitates. The goal of this experiment is to study the nature of ionic reactions‚ write balanced equations‚ and to write net ionic equations for precipitation reactions. A detailed view of the results can be found in the table below. Cations used: Barium‚ Copper‚ Iron‚ Sodium‚ Cobalt‚ Nickel Anions used: Nitrate‚ Carbonate‚ Chloride‚ Hydroxide‚ Sulfate‚ Bicarbonate‚ Iodide‚ Phosphate
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rule‚ reactivity increases as you move down a group in the periodic table. This means in regards to solubility that the more you farther you move down the group the more insoluble the element is when combined with hydroxides‚ chlorides‚ bromides‚ iodides‚ sulfates‚ carbonates‚ and oxalates. My results were consistent with this theory in that the mixtures went from no reaction to forming a precipitate or from forming a light precipitate to a heavy one as the elements moved down the periodic
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Chemical equilibrium is said to be dynamic because‚ at equilibrium‚ there are reactions continually occurring. The rate of the forward reaction equals the rate of the reverse reaction. Equilibrium Constants At equilibrium as much hydrogen iodide is being decomposed as is formed and so the concentrations of all three substances remains constant. Kc is the equilibrium constant in terms of molar concentration. This is known as the Equilibrium Law. The equilibrium constant shows the position
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light (put in a dark place) will not decompose. Theory: Equipment: * 4 x petri dishes * 1 x glass stirring rod * 0.1 mol/L silver nitrate in a dropper bottle * 0.1 mol/L Sodium chloride in a dropper bottle * 0.1 mol/L Sodium iodide in a dropper bottle Method: 1. Ensure you are wearing safety glasses 2. Take the petri dishes and label then 1‚ 2‚ 3‚ and 4. 3. Add 20 drops of silver nitrate solution to each petri dish. 4. Add 20 drops of sodium chloride to petri
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which of the two will reacted with potassium iodide inside the breaker‚ as the latter passed from the beaker into the tube‚ the glucose/starch solution’s change of color showed that the potassium iodide was small enough that it able to pass through from the solution and into the bag. After the Benedict test‚ glucose from the bag was also founded small enough that it can exit from the bag and into and solution. In the end‚ glucose and potassium iodide was the only two that is capable to move freely
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CHAPTER 4 REACTIONS IN AQUEOUS SOLUTION MULTIPLE CHOICE QUESTIONS 4.1 Which of the following compounds is a strong electrolyte? E A. H2O B. O2 C. H2SO4 D. C6H12O6 (glucose) E. CH3COOH (acetic acid) Answer: C 4.2 Which of the following compounds is a strong electrolyte? E A. H2O B. N2 C. KOH D. C2H6O (ethanol) E. CH3COOH (acetic acid) Answer: C 4.3 Which of the following compounds is a weak electrolyte? E A. HCl B. CH3COOH (acetic acid)
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Exp.11) Identification of unknown ketones. Introduction: Given five samples of a known ketone derivative‚ the purpose of this experiment is to identify which unknown ketone derivative corresponds to the five known samples. In other words‚ using specific methods of compound detection‚ it is possible to match an unknown compound with a known compound because similar compounds will display similar characteristics. In this experiment‚ identification of the unknown ketone is accomplished through thin
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List: Sodium carbonate solution Copper sulphate solution (Safety: High toxicity) Sodium hydroxide solution (Safety: Irritant) Ammonia solution (Safety: Toxic by inhalation) Potassium iodide solution (Safety: Mild irritant) Lead nitrate solution (Safety: Toxic) Sulphuric acid (Safety: Corrosive) Copper carbonate Silver Nitrate (Safety:
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Natalia Nelson 6661318 Environmental Studies Section: Friday @ 2:00 with Jason Linn Fracking: The Invention of the Century or Destructive New Technology? Introduction: Possible quote – someone who supports the processs. Possible story: some analogy of something that was a good‚ necessary idea but just put off the inevitable and had a negative affect than fix it. Need for energy‚ how new ideas are necessary But is fracking really the best option? Public eye‚ people here about fracking
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Worked solutions to student book questions Chapter 2 Analysis by mass Q1. a b Why was the soup sample in Worked Example 2.1 heated to 110°C? Why was it necessary to weigh the sample four times? A1. a b The soup was heated above 100°C to evaporate water from the sample. By repeatedly heating the sample until the mass remained unchanged‚ the analyst could be sure that all the water had been removed. Q2. Some laboratories use microwave ovens in place of conventional ovens to
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