HOW DOES THE SOLUBILITY OF POTASSIUM CHLORIDE (KCL) AND POTASSIUM IODIDE (KI) IN WATER VARY WITH TEMPERATURE? AIM To observe solubilities of KCl and KI with water at different temperatures To compare the two solubility curves and discuss what might vary the solubility of different ionic compounds. THE VARIABLES DEPENDENT VARIABLE Temperature INDEPENDENT VARIABLE Amount of solute (KCl‚ KI) CONSTANTS Amount of the solvent (water)‚ pressure APPARATUS 100G OF POTASSIUM CHLORIDE 100G
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I am choosing to study how the PSI (pounds per square inch) of a football is affected by the temperature. I chose to study this because I like football and I always pondered this question. I believe that this is a worthwhile question to study because these studies can help improve the game as the weather gets colder. As air cools‚ it expands‚ so when a football gets colder‚ the air inside it expands. This expansion causes the air pressure to decrease. The air pressure decreases because the molecules
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Title of Experiment 12: The Effect of Ionic Strength on the solubility of an Electrolyte Aim: The purpose of this experiment was to determine the thermodynamics variable of enthalpy‚ ∆H for the dissolution reaction of boric acid in water. The solubility of boric acid was measured over a range of various temperatures by finding out at what temperature crystallization began for solution of different molarities. A graphical relationship between the natural logarithm of molal concentration and the inverse
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Research Question Does the concentration of substrate (H2O2 (hydrogen peroxide)) have an effect on the activity of the enzyme (catalase)? Theory The higher the substrate concentration the more quickly product is produced (rate of reaction increases) until enzyme saturation is reached at which time more substrate has no further effect. Enzymes such as Catalase are protein molecules which are found in living cells. They are used to speed up specific reactions in the cells. They are all
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Date Submitted: August 6‚ 2012 Experiment No. 4 Solubility Equilibrium- Common Ion Effect INTRODUCTION: The common ion effect is another example of Le Châtelier ’s Principle in action.The common ion effect tells us that the solubility of an ionic compound is decreased by the addition to the solution of another ionic compound that contains one of the ions involved in the solution It is also responsible for the reduction in solubility of an ionic precipitate when a soluble compound combining
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The data collected supported the hypothesis and the tablets were significantly more dissolved than the gelcaps and caplets. This experiment could be changed by having a component stir the acetaminophen and the water together. Introduction The solubility of medicine is important because the quicker it dissolves‚ the quicker is can start working. There are many different forms of Acetaminophen on the market. This experiment is an attempt to discover which form of Acetaminophen will dissolve the quickest
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project is to demonstrate how water temperature affects the dissolving of sugar in liquid. Everything in our universe is made up of particles which are in constant motion. In a solid state particles move the slowest while in a liquid state particles move the fastest. Under the right conditions‚ solid particles (the solute) when mixed in liquid (the solvent) can form a solution. This occurrence is called dissolving. I wanted to answer the question; does the temperature of water affect the speed at which
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Title: Study of Solubility Equilibrium Abstract The effect of temperature on the solubility product constant‚ Ksp‚ of potassium hydrogen tartrate in water was investigated in the temperature range of 285K to 318K at normal atmospheric pressure. It was found that the solubility of potassium hydrogen tartrate decreases with a decrease in temperature and consequently a smaller volume of sodium hydroxide is needed to neutralize it. The molar solubility of potassium hydrogen tartrate was calculated
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general‚ solubility rules can be used to predict the outcome of double replacement reactions. I have come to this decision‚ because almost all of the data recorded from the lab‚ with the exception of number 13‚ agreed with the predictions made beforehand. 2. Out of the 15 combinations‚ the observations made for the combination of number 13 (the reaction of lead (II) nitrate and barium chloride)‚ did not agree with what was predicted‚ based on the solubility rules. The solubility rules that
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n this lab experiment factors that affected solubility are temperature‚ liquids‚ concentration‚ pressure‚ polarity‚ and molecule. In this experiment we use temperature‚ centrifuge‚ and concentration solutions to be able to achieve the results that we wanted. Step one of the experiment was to mix HCl‚ to cause a precipitation form‚ after that we had to decant the solution‚ then we used a centrifuged to separate the the precipitate of the supernatant liquid. After the decant was done‚ then the process
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