Experiment 5 revised Titration of strong acid and strong base newer word version

Experiment 5 revised Titration of strong acid and strong base newer word version

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1 Experiment 5: Titration – Strong Acid and Strong Base PURPOSE A titration is a process used to determine the volume of a solution with a known concentration that is needed to react with a given amount of another substance. In this experiment, your goal is to determine the molar concentration of an unknown acid solution by conducting titrations with a base of known concentration. You will be testing a strong acid, HCl, solution by two methods, 1) using the indicator phenolphthalein and 2) by a pH meter. Both testing methods will be combined during the titration process and you will compare the results obtained by the indicator with the results obtained from a titration curve and a Gran Curve. You will use a standardized sodium hydroxide, NaOH, solution as your strong base of known concentration for the titrations. The reaction equation is shown below in net ionic form. H + (aq) + OH (aq) H 2 O(l) The stoichiometry of the reaction is one mole of hydrogen ion reacts with one mole of hydroxide ion to produce one mole of water. Therefore, you calculations will be straightforward. You will determine the concentration of an unknown strong acid by both methods. The volume of NaOH titrant used at the end point as determined by the indicator and the equivalence point as determined by the titration curves will be used to determine the molarity of an unknown concentration of HCl solution. PRINCIPLES Acid-base reactions are among the most important kinds of reactions that occur in aqueous solutions because of their significance in the metabolism of plants and animals and their plentiful use in industrialized societies. A neutralization reaction is the commonly used expression used to describe the reaction of an acid with a metal hydroxide base that produces a salt and water. The term is derived from the observation that the standard properties of the acids and the bases are neutralized when reacted with each other. The driving force of nearly all neutralization reactions is the combination of the H + (aq) from an aqueous acid solution with the OH - (aq) from an aqueous base solution to form water molecules. All strong acids and bases completely or nearly completely ionize in dilute solution. Strong acid and strong base solutions contain predominately ions rather than acid or base molecules; the equilibrium falls almost entirely to the right in dilute solution. There are only six strong acids and eight strong soluble bases. They are listed below. Strong acids: a) Three binary acids derived from Group VIIA halogens 1) Hydrochloric acid – HCl 2) Hydrobromic acid – HBr 3) Hydroiodic acid – HI
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2 b) Three ternary acids (oxyacids) derived from polyatomic ions 4) Sulfuric acid – H 2 SO 4 5) Nitric acid – HNO 3 6) Perchloric acid – HClO 4 Strong bases: a) Group IA metal hydroxides 1) Lithium hydroxide – LiOH 2) Sodium hydroxide – NaOH 3) Potassium hydroxide – KOH 4) Rubidium hydroxide – RbOH 5) Cesium hydroxide – CsOH b) Heavier Group IIA metal hydroxides
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This note was uploaded on 03/19/2011 for the course CH 204 taught by Professor Leytner during the Spring '08 term at University of Texas at Austin.

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Experiment 5 revised Titration of strong acid and strong base newer word version

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