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 comparing the Ksp values of two or more compounds can only be done if the compounds share the same dissociation
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Introduction: Chemical equilibrium is when the concentrations of the reactants and products have reached a state where reactions occurring in one direction are at the same rate of reactions occurring in the opposite direction. This process‚ called dynamic equilibrium‚ is the main subject of Le Chatelier’s Principle. Le Chatelier pointed out that if a system at equilibrium is subjected to a stress that momentarily causes the system to be not in equilibrium‚ a spontaneous change will occur to
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AP Chemistry Background The solubility product constant‚ Ksp‚ is a particular type of equilibrium constant. The equilibrium is formed when an ionic solid dissolves in water to form a saturated solution. The equilibrium exists between the aqueous ions and the undissolved solid. A saturated solution contains the maximum concentration of ions of the substance that can dissolve at the solutions temperature. A knowledge of the Ksp of a salt is useful‚ since it allows us to determine the concentration
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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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Experiment 5: Shifting Equilibrium A solution is in equilibrium when the rate of forward reaction and the rate of reverse reaction are equal. This equilibrium may be disturbed when the concentration of the reactants‚ the concentration of the products or the temperature is changed. If the process involves gases‚ a change in pressure can also affect the position of equilibrium. The concept behind this is Le Chatelier ’s Principle which states that when a system is disturbed through application
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found by moles divided by liters which declined with every titration because less and less solution was needed. After the molarity of the Cl- is found the molarity of Pb2+ is half the molarity of Cl- since there is 2 Cl- ions for each Pb2+ ion. Then Ksp can be calculated from equation (3). Then a graph can be created to find free energy of the reaction by lnKsp vs.
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main objective is to test the solubility and the strength of the ionic compounds that are formed during titration. Solubility is a measure of the degree at which a compound is able to dissolve. Titration is used in this experiment to determine the Ksp of the saturated solution of Mg(OH)2 Ca(OH)2 SR(OH)2. Procedure and Observations Saturated solutions of Mg(OH)2‚ Ca(OH)2‚ and Sr(OH)2 are all prepared in which they need to be diluted with distilled water after phenothelain is added to the saturated
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Chemistry 12 Unit 3 - Solubility of Ionic Substances Chemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances 1. Identify each of the following as ionic or molecular substances: a) NaCl(aq) ........................................................___________________________________ b) CH 3COOH(aq) ..........................................___________________________________ c) CCl4(l) ...................................................___________________________________ d) HNO3(aq)
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Worksheet 5. Aqueous Equilibrium Problems; Simple Equilibria 1. Identify the acid/base and their conjugate base/acid‚ and which definition you use to determine(Bronsted‚ Arrhenius or Lewis): a. HCO3- + H+ ↔ H2CO3 Base conj acid: Bronsted b. HCO3- ↔ CO32- + H+ Acid conj base : Arrhenius c. CH3NH2 + H2O ↔ CH3NH3+ + OHBase acid conj acid conj base : Lewis d. C6H5OH + H2O ↔ C6H5O- + H3O+ Acid base conj base conj acid : Lewis‚ Arrhenius‚ Bronsted e. H2O + H2O ↔ H3O + + OHAcid base
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sparingly soluble salt is used. The dissociation reaction is KHC4H4O6 (s) ⇌ K+ (aq) + HC4H4O6- (aq) and the solubility product constant‚ Ksp‚ expression can be written as Ksp = [K+][HC4H4O6-] As KHC4H4O6 dissociates‚ it gives the same amount of HC4H4O6- and K+ ions‚ so the Ksp expression may be rewritten as the square of [HC4H4O6-]‚ i.e. Ksp = [HC4H4O6-]2 The hydrogen tartrate ion‚ HC4H4O6-‚ acts as a weak monoprotic acid. The concentration of HC4H4O6- can be determined by titrating
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