that resists a change in pH when an acid is added. Incorrect D.a solution that contains both a weak acid and its conjugate base. E.All of the above are true. Answer Key: B Question 7 of 12 4.0/ 4.0 Points What is the value of the ion product constant for water (Kw)? A.0.0 B.1.0 x 1014 C.1.0 x 10-7 Correct D.1.0 x 10-14 E.1.0 x 107 Answer Key: D Question 8 of 12 4.0/ 4.0 Points What is the pH of a solution that has a H⁺ concentration equal to 1.7 x 10-5 M? A.0.22 B.5.20 C.10.20
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molecules in a transition-state configuration and the corresponding atoms and molecules in their initial configuration. The activation energy is usually represented by the symbol Ea in mathematical expressions for such quantities as the reaction-rate constant‚ k = Aexp(-Ea/RT).The Arrhenius equation gives the quantitative basis of the relationship between the activation energy and the rate at which a reaction proceeds. This equation suggests that the activation energy is dependent on temperature‚ but
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AbstractWater is important substance for all living organisms. The physical and chemical properties of water play a central role in biological structure and function of the organism. The ionization ability of water to form H+ and OH- ions make it very unique. The hydrogen-ion concentration of biological system is usually preferred as the pH system‚ which determines the pH level of dilute aqueous solutions. In this laboratory‚ the data collected from the experiment will be used to graph the titration
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CHM 116 Lab Investigations of Buffers I. Purpose The purpose of this experiment was to get an understanding as to how to properly prepare chemical buffers. Also part of this experiment was to gauge the effectiveness of the buffers by measuring their pH levels in various titration solutions‚ using a pH meter. II. Procedure To start our experiment we had to prepare Buffer B‚ which was the .060 M Ammonia/Ammonium solution. Using 3.0 M ammonia‚ we had to calculate
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The relationship between Ka and pKa is that Ka is the equilibrium constant for the dissociation of a weak acid and pKa is the half-equivalence point where pH=pKa. In addition to the pH‚ Ka is an indication of an acids strength; pKa = - log Ka. B. The potential sources for errors in this experiment are the inconsistent
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If pH > pI‚ then the protein will have a negative charge and if pH < pI‚ the protein will have a positive charge. Buffer I has a pH >5‚ meaning both proteins carry a negative charge and bind to the DEAE (a positively charged resin). (b) pH = pKa + log10(Base/Acid) [Base = mM of sodium acetate; Acid = mM of acetic acid] = 4.7 + log10 (40/40) = 4.7 In order for the catalase to elute from the column‚ it must have lost its negative charge and stopped binding to the DEAE. Lowering the pH
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______________________________________________________________________________________________________________ INTRODUCTION Monitoring the pH range of a laboratory reaction or a process is very important. It is important to keep the pH almost constant even when addition of acids or bases takes place. One can easily know if a solution is an acid or a base using a visual indicator. Indicators are organic dye added to a solution that changes color base on the concentration of H3O ions in the solution
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Acids‚ Bases‚ and Buffers Introduction: The pH scale is used to determine how acidic or basic a solution is‚ ranging from 1-14. The most acidic of all acids are at a pH level of 1 and the most basic of all bases are at 14. The neutral pH level is 7‚ which is what drinking water is. The pH level is determined by the amount of H+ ions present in a solution‚ and the more H+ ions there are the more acidic it is‚ and the lack of these ions results in more basic solutions. One distinguishing feature
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Phenol‚ also known as carbolic acid‚ is an aromatic organic compound with the molecular formula C6H5OH. It is a white crystalline solid that is volatile. The molecule consists of a phenyl group (-C6H5) bonded to a hydroxyl group (-OH). It is mildly acidic‚ but requires careful handling due to its propensity to cause chemical burns. Phenol was first extracted from coal tar‚ but today is produced on a large scale (about 7 billion kg/year) from petroleum. It is an important industrial commodity as a
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water. References: [1] Mohrig‚ J. R.; Hammond‚ C. N.; Morrill‚ T. C.; Neckers‚ D. C. 1998 Experimental Organic Chemistry‚ New York: Freeman‚ pp. 32-36. [2] www.chemblink.com II. Potentiometric Determination of the Purity and Acid Dissociation Constant of Salicylic Acid Purpose: Part II of the experiment utilizes the concept of potentiometric titration in the determination of the pKa‚ a measure of the relative acidity of an acid‚ of the salicylic acid product in Part I. Potentiometric titration
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