Determining the equilibrium constant from pH values of changing concentrations of ethanoic acid Design Research question: How will altering the concentrations of ethanoic acid affect the pH value‚ and‚ in-turn‚ the equilibrium constant? Background information: When weak acids react‚ the reaction typically does not go to completion. Rather‚ the system goes to an intermediate state in which the rates of the forward and reverse reactions are equal. Such a system is said to be in chemical equilibrium
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dissociation constant (Ka) for the weak acid HX in aqueous solution is 3.01 × 10–5 mol dm–3. (i) Calculate the value of pKa for HX at this temperature. Give your answer to 2 decimal places. ............................................................................................................... ............................................................................................................... (1) (ii) Write an expression for the acid dissociation constant (Ka) for
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Chapter 13 Acids and Bases (Dr Chong Fai Kait) 1) A 7.0 103 M aqueous solution of Ca(OH) 2 at 25.0 °C has a pH of __________. A) 12.15 B) 1.85 C) 1.4 102 D) 7.1 1013 E) 11.85 Answer: A 2) The acid-dissociation constant at 25.0 °C for hypochlorous acid (HClO) is 3.0 108 . At equilibrium‚ the molarity of H 3 O in a 0.010 M solution of HClO is __________. A) 1.7 105 B) 0.010 C) 5.8 1010 D) 4.76 E) 2.00 3) Using the data in the table‚ which of the conjugate acids below is the weakest
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ACIDS AND BASES The reason that acid-base reactions are so important is that many of the things you come into contact with on a daily basis are either acids or bases. Most fruits are acids‚ as are carbonated beverages‚ tea‚ and battery acid. Common household bases include baking soda‚ ammonia‚ soap‚ and antacids. What are acids and bases? There are not one but three common definitions used to describe acids and bases: 1. Arrhenius acids and bases 2. Brønsted-Lowry acids and bases 3. Lewis acids
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POTENTIOMETRIC DETERMINATION OF THE PURITY AND DSSOCIATION CONSTANT OF HYDROGEN PHTHALATE Department of Chemical Engineering‚ College of Engineering University of the Philippines‚ Diliman‚ Quezon City‚ Philippines Date Due: September 20‚ 2013 Date Submitted: September 20‚ 2013 RESULTS AND DISCUSSION An experiment was conducted to determine the purity of Hydrogen Phthalate sample and its dissociation constant. To perform the experiment with the utmost precision‚ equivalence point was
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WRITE YOUR NAME HERE:________________________________________________________ CHM 2046 (Gower sections) Exam 2 (Form Code A) Fall 2014 Instructions: On your scantron sheet enter and bubble in your name‚ UF ID number‚ and Form Code. Check your bubbling carefully – bubbling errors will not be negotiated. Turn in your scantron and retain your exam (with your answers circled). Potentially useful info : Kw = 1 x 10‒14 at 25°C pH = −log [H3O+] pH = pKa + log ([base] / [acid]) R =
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molecules or solute ions. In pure water‚ a small amount of molecules take part in an equilibrium reaction1. 2 H2O (l) H3O+ (aq) + OH- (aq) This self-ionization of water produces a small amount of both hydronium and hydroxide ions. The equilibrium constant expression for this reaction is called Kw (1.0x10-14)‚ or the ion product of water1. From this number‚ if the concentration of hydronium is known the concentration of hydroxide can be found or vice versa. Strong acids are substances that ionize
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activity‚ and that catalase will denature in the pH after pH10. At the start of the reaction‚ there is no product‚ and the concentration is the same as the atmosphere. After a short time‚ oxygen accumulates at a rather constant rate. The slope of the curve at this initial time is constant and is called the initial rate. As the peroxide is destroyed‚ less of it is available to react and the O2 is produced at lower rates. When no more peroxide is left‚ O2 is no longer produced.
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endpoint of this titration. As a result‚ the concentration of the NaOH solution was found to be 0.124 M with a standard deviation of 0.004 M. In the second titration‚ the goal was to use both an acid’s formula weight and acid dissociation equilibrium constant (pKa) value to determine the identity of this unknown acid. Both values were found by preparing the unknown acid solution‚ preparing a buret‚ titrating the acid solution with the strong basic NaOH solution from the previous experiment‚ and determining
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concentration the same in each solution‚ we were able to identify the addition of more C2H3NaO2 as the sole factor causing increased resistance. The results found backup my group’s original hypothesis that predicted that greater amounts of C2H3NaO2 in the constant amount of HC2H3O2 would result in the greatest resistance to pH change by acting as a buffer in the solution. The buffer capacity‚ which is the increased about of acid or base that can be added to a buffer without destroying it’s effectiveness increased
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