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Compute for the volume of concentrated HCl needed to prepare 500 mL of 0.1000 M HCI solution.

Compute for the volume of concentrated HCl needed to prepare 500 mL of 0.1000 M HCI solution.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A. Compute for the volume of concentrated HCl needed to prepare 500 mL of 0.1000 M HCI solution.

EXPERIMENT 3 Determination of Carbonates in a Mixture: Double Indicator Titration In this experiment, a solution of hydrochloric acid is prepared and is standardized against N22CO3. This will then be used to determine the constituents present in a mixture, and the concentration present for each constituent. The carbonate in aqueous solution acts as a base; thus, it accepts a proton to form the bicarbonate ion according to the equation: pH 8.3; K1 = 3.5 x 10-7 рH 3.8; Кг %3D 5.11 х 10-11 CO32- + H* = HCO3 %3D HCO32- + H* = H2CO3 Two endpoints can be observed in titration of Na2CO3. The first endpoint corresponds to the conversion of carbonate to hydrogen carbonate that occurs at around pH 8.3. The second endpoint involves the formation of carbonic acid and carbon dioxide at pH 3.8. The latter endpoint is always used for standardization because the change in pH is greater than that of the first. From the volumes of titrant used for both endpoints, the constituents of the mixture and its corresponding concentration can be computed (Figure 1). pH 14- From NazCO, cos cm From NaHCO, HCO HCO cm b cm CO2 Volume of HCI added Figure 2: Guide for determination and computation of the constituents involving carbonate mixtures.
Transcribed Image Text:EXPERIMENT 3 Determination of Carbonates in a Mixture: Double Indicator Titration In this experiment, a solution of hydrochloric acid is prepared and is standardized against N22CO3. This will then be used to determine the constituents present in a mixture, and the concentration present for each constituent. The carbonate in aqueous solution acts as a base; thus, it accepts a proton to form the bicarbonate ion according to the equation: pH 8.3; K1 = 3.5 x 10-7 рH 3.8; Кг %3D 5.11 х 10-11 CO32- + H* = HCO3 %3D HCO32- + H* = H2CO3 Two endpoints can be observed in titration of Na2CO3. The first endpoint corresponds to the conversion of carbonate to hydrogen carbonate that occurs at around pH 8.3. The second endpoint involves the formation of carbonic acid and carbon dioxide at pH 3.8. The latter endpoint is always used for standardization because the change in pH is greater than that of the first. From the volumes of titrant used for both endpoints, the constituents of the mixture and its corresponding concentration can be computed (Figure 1). pH 14- From NazCO, cos cm From NaHCO, HCO HCO cm b cm CO2 Volume of HCI added Figure 2: Guide for determination and computation of the constituents involving carbonate mixtures.
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