Experiment 9 a volumetric analysis lab report

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i need the pre lab to be solved in an hour with calculations after finishing ill send u the data for the lab and the lab i want it with calculation9 Experiment A Volumetric Analysis A titrimetric analysis requires the careful addition of titrant. • To prepare and standardize a sodium hydroxide solution • To determine the molar concentration of a strong acid Objectives The following techniques are used in the Experimental Procedure: Techniques A chemical analysis that is performed primarily with the aid of volumetric glassware (e.g., pipets, burets, volumetric asks) is called a volumetric analysis. For a volumetric analysis procedure, a known quantity or a carefully measured amount of one substance reacts with a to-be-determined amount of another substance with the reaction occurring in aqueous solution. The volumes of all solutions are carefully measured with volumetric glassware. The known amount of the substance for an analysis is generally measured and available in two ways: Introduction 1. As a primary standard—An accurate mass (and thus, moles) of a solid substance is measured on a balance, dissolved in water, and then reacted with the substance being analyzed. 2. As a standard solution—A measured number of moles of substance is present in a measured volume of solution, generally expressed as the molar concentration (or molarity) of the substance. A measured volume of the standard solution then reacts with the substance being analyzed. Primary standard: a substance that has a known high degree of purity, a relatively large molar mass, is nonhygroscopic, and reacts in a predictable way Standard solution: a solution having a very well known concentration of a solute The reaction of the known substance with the substance to be analyzed, occurring in aqueous solution, is generally conducted by a titration procedure. The titration procedure requires a buret to dispense a liquid, called the titrant, into a ask containing the analyte (Figure 9.1a, page 128). For the acid–base titration studied in Part B of this experiment, the titrant is a standard solution of sodium hydroxide and the analyte is an acid. Experiment 9 127 Figure 9.1 (a) Titrant in the buret is dispensed into the analyte until (b) the indicator changes color at its endpoint. Stoichiometric amounts: amounts corresponding to the mole ratio of the balanced equation Acid–base indicator: a substance having an acidic structure with a different color than its basic structure pH: the negative logarithm of the molar concentration of H3O⫹, pH ⫽ ⫺log[H3O⫹]. Refer to Experiment 6. Standardization of a Sodium Hydroxide Solution Hygroscopic: able to absorb water vapor readily COOH _ COO K+ potassium hydrogen phthlate A reaction is complete when stoichiometric amounts of the reacting substances are combined. In a titration this is the stoichiometric point.1 In this experiment, the stoichiometric point for the acid–base titration is detected using a phenolphthalein indicator. Phenolphthalein is colorless in an acidic solution but pink in a basic solution. The point in the titration at which the phenolphthalein changes color is called the endpoint of the indicator (Figure 9.1b). Indicators are selected so that the stoichiometric point in the titration coincides (at approximately the same pH) with the endpoint of the indicator.