Introduction: Solubility equilibrium refers to the dissolution of a compound in water. Specifically‚ the degree to which a compound is soluble (Tro‚ 739). This can be measured using the expression Ksp = [Mb+]a[Xa-]b‚ in which Ksp represents the solubility product constant (Thorne‚ 90). This constant is important because it does not change at a given temperature‚ regardless of the solution a compound is in; a smaller constant would indicate lower overall solubility. It is important to note that
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07.05 Le Chatelier ’s Principle Research Project Fritz Haber was born in December of 1868‚ in Prussia to a German chemical merchant. He went into the field of organic chemistry at the University of Jena. He was appointed as director of the Kaiser Wilhelm Institute for Physical Chemistry in Berlin in 1911. He was in charge of forming a center for cross-disciplinary research and gave his country the knowledge of ammonia and other significant fertilizers. He left Germany in 1933 after their loss
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Instead‚ by increasing the concentration of the cathode‚ the voltage of the galvanic cell will decrease due to the equilibrium shift to the left. The highest concentration (1.5 mol dm-3 ) was the lowest out of the 3 trials at 1.68 volts‚ thus proving that the higher concentration the lower the voltage. When the concentration of the product decreases‚ it will drive the equilibrium to the right to minimize the impact. Although‚ the lowest calculation (0.5 mol dm-3) is not necessarily the highest out
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Restoring Balance LeChâtelier’s Principle and Equilibrium Introduction Chemical equilibrium is a true balancing act. What happens when the balance is disturbed? The purpose of this lab is to observe the effects of concentration and temperature on equilibrium and to visualize how balance can be restored based on LeChâtelier’s Principle. Background Not all chemical reactions proceed to completion‚ that is‚ to give 100% yield of products. In fact‚ most chemical reactions are reversible
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Experiment 11 Date: 28-3-2011 Title: Interpretation of reaction by the Le Chatelier’s principle Objective: To determine the factors that affecting the equilibrium position Introduction: Le Chatelier’s principle states that if a system in equilibrium is subjected to a change‚ the equilibrium position of the system will shift in a direction to minimize the effect of the change. Iron(III) ions and thiocyanate ions (NCS-) react in solution to produce thiocyanatoiron(III) (FeNCS2+)‚ a
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Title:Interpretation of reaction by the Le Chatelier’s principle Objective:To determine the factors that affecting the equilibrium position Introduction Iron(III) ions and thiocyanate ions (NCS-) react in solution to produce thiocyanatoiron(III) (FeNCS2+)‚ a complex ion‚ according to the equation : Fe3+(aq) + NCS-(aq) [pic] FeNCS2+(aq) yellow colourless blood red The colour produced by the complex ion indicates the position of equilibrium. In this experiment‚ iron(III)
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Torque and Equilibrium Purpose: Apply principle of static equilibrium to determine a coefficient of friction. Research Question: What is the coefficient of friction between a meter stick and wall? Hypothesis: Tying a piece of string on to the end of a meter stick‚ put the other end of the meter stick against the wall so that the meter stick is horizontal and does not slide down the wall. Hang a weight on the meter stick sliding it to a point where the meter stick is about to come off from
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Chemical Equilibrium: Le Chatelier Principle By Sarah Ramos and Kristina Todorovic Chemistry 203 DEN Dr. Mohamed El-Maazawi Part A. Acid-Base Indicators Purpose In this part of the experiment‚ we will find a reagent that will shift the acid-base equilibrium reaction described by Equation (2) in one direction and then a second reagent that will cause the equilibrium position to shift back in the opposite direction. Introduction An acid–base indicator
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Chemical equilibrium is a state of balance within a system of chemical reactions. Equilibrium in chemistry is achieved when substances are produced and broken down at the same rate and thus‚ the number of molecules of each substances becomes constant. Thermodynamics is a branch of physical science that involves the relationship between heat and other forms of energy (Energy‚ Enthalpy‚ and the First Law of Thermodynamics). There is a more specific area of thermodynamics that explicitly pertains to
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(a) Define the term equilibrium potential and use the Nernst equation (see Appendix) to show how the equilibrium potentials for both sodium and potassium are calculated. Equilibrium potential is the potential of the membrane when there is no net flow of ions from one gradient to the other gradient. The ions are equal and are opposite of each other but not moving from one side to the other. Sodium: Ena=2.303((8.31 J m-1 K-1)(310K))/((1(= 9.65 x 104 c m-1))(log(150/15))= 61.54 mV Ek=2.303((8
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