electrolyte Brønsted-Lowry theory Acid is a proton donor Base is a proton acceptor H2O + HNO2 H3O+ + NO2- The conjugate base of the acid HNO2 is nitrite ion. The conjugate acid of water is the hydrated proton written as H3O+ Amphiprotic solvent – solvent that can act either as an acid or as a base‚ a classic example is water. The weakest acid forms the strongest conjugate base The tendency of a solvent to accept or donate protons determines the strength of a solute acid or base dissolved in it. Conjugate
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ionization of a weak acid or a weak base hence this is known as the common ion effect. Simply put‚ the effect of the common ion is to decrease the solubility of the salt. Reactions involving weak conjugate acid-pairs can resist massive change when small amounts of strong acids and bases are added to it. Buffer solutions are also related with the common ion effect. A buffer is an aqueous solution composed of a weak acid and its conjugate base or a weak base with a conjugate acid that will have a minimal
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Laboratory report Shae Aquino Chemistry 161L February 25‚ 2014 Conductivity of Solutions of Ionic and Covalent Compounds Purpose The purpose of this experiment was to use electrical conductivity on ionic‚ molecular acids‚ and covalent compounds in order to determine the properties of each compound. Introduction In chemistry‚ the term of an aqueous solution is defined as a substance that is soluble in water. For example‚ sodium chloride (NaCl) dissolves in water‚ or other
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4 Titration Curve of an Amino Acid pH Simple amino acid Acidic amino acid Basic amino acid 7 OH- equivalents Objectives: A) To determine the titration curve for an amino acid and B) to use this curve to estimate the pKa values of the ionizable groups of the amino acid and the amino acid’s pI. Introduction: A titration curve of an amino acid is a plot of the pH of a weak acid against the degree of neutralization of the acid by standard (strong) base. Consider the ionization
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with each other and with the walls of the container. Due to these collisions the speeds and the kinetic energies of the individual molecules keep on changing. However at a given temperature‚ the average kinetic energy of the gas molecules remains constant. If at a given temperature‚ n1 molecules have speed v1‚ n2 molecules have speed v2‚ n3 molecules have speed v3‚ and so on. Then‚ the total kinetic energy (EK) of the gas at this temperature is given by where m is the mass of the molecule.
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levels and Preparation of Acetate Buffer. Introduction A buffer is a solution having the capacity to resist changes in pH levels. Mostly a buffer consists of a weak acid and a salt of strong base or a weak base and a conjugate salt of strong acid e.g. acetate buffer is the most common buffer in which equimolar mixture of acetic acid and sodium acetate solution is used. CH3COOH CH3 COO - + H+ CH3COONa CH3COO - + Na+ Buffers are divided into 2 parts on the basis of their nature. Acidic Buffer
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2.5 10-5 M 4.9 10-5 M 7.0 10-3 M 3.7 10-2 M 5. What is the pH of the buffer that results when 12.5 g of NaH2PO4 and 22.0 g Na2HPO4 are mixed and diluted with water to 0.500 L? (The acid dissociation constants for phosphoric acid are Ka1 = 7.5 10-3‚ Ka2 = 6.2 10-8‚ and Ka3 = 3.6 10-13) (Points : 10) 2.30 7.04 7.38 12.27 12.62 6. Which of the following combinations would be the best to buffer an aqueous
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acetic acid‚ Gylcine and Tris were investigated. Overall the pKa values obtained experimentally were similar to the published pKa values and the range of the buffer systems were roughly ± 1 pH unit from the pKa values. Introduction A buffer solution works to minimise the change in pH on addition of acid or alkali. Different buffer systems are effective over different pH ranges. The aim of this experiment is to investigate the ranges at which three different buffer systems: Acetic acid/NaOH
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Menbere Wendimu Che101 Laboratory Report Acid Base Laboratory Objective: Introduction: Experimental: 2.04 g of KHP‚ 100ml volumetric flask‚ distilled H2O‚ approximately 0.1 M of NaOH‚ Vinegar‚ Phenolphthalein‚ 250ml Erlenmeyer flask‚ weighing balance‚ Graduating Cylinder‚ burette and pH meter were used in our experiment. In our first part of our experiment to prepare a primary standard‚ 0.1 M solution of KHP‚ we carefully weighed out 2.04g of KHP in a weigh paper using the weighing balance
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prepared a standard solution of magnesium sulfate. The student first weighed out 0.5178 g of magnesium sulfate heptahydrate. The student transferred the solution quantitatively into a 100-mL volumetric flask. The student then added 5 mL of sulfuric acid together with 10 mL of distilled water into the
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