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Experiment 1: Equilibrium and Thermodynamic Study of Borax

by: Brenna Roti

Experiment 1: Equilibrium and Thermodynamic Study of Borax 43430

Marketplace > Western Michigan University > Chemistry > 43430 > Experiment 1 Equilibrium and Thermodynamic Study of Borax
Brenna Roti
GPA 3.82
General Chemistry Lab II
Ekkehard Sinn

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About this Document

Book: Chemistry 1130 General Chemistry Lab II Fourth Edition Hayden McNeil Acknowledgement: This experiment was adapted from Purdue University Chemistry Department CHM 116 Lab Manual, 1999.
General Chemistry Lab II
Ekkehard Sinn
Study Guide
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This 5 page Study Guide was uploaded by Brenna Roti on Monday October 5, 2015. The Study Guide belongs to 43430 at Western Michigan University taught by Ekkehard Sinn in Summer 2015. Since its upload, it has received 363 views. For similar materials see General Chemistry Lab II in Chemistry at Western Michigan University.


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Date Created: 10/05/15
Experiment 1 Brenna M Roti Equilibrium and Thermodynamic Study of Borax CHEM 1130 TA Jorden Kegeler Tuesday 800 am Room 1871 Colin Sytsma Purpose of Experiment The purpose of this experiment is to determine the concentration of B4O5OH4239 in several saturated borax solutions at different temperatures With this data one can calculate the solubility constant of Borax as a function of temperature and use the KSID to calculate AG AH and AS Procedures Obtain a 50 mL burette ring stand 10 mL graduated cylinder test tubes Erlenmeyer flask thermometer indicator and 0125 M HCI Using an eyedropper take the Na2B40710H20 solution from the 45 C bath and add it to a 10 mL graduated cylinder until you have 5mL of Borax Immediately transfer the solution into a test tube labeled with the correct temperature corresponding with the bath and take the temperature of the solution Add the contents of the test tube to an Erlenmeyer flask and rinse the test tube with deionized water into the flask to make sure all of the Borax and any precipitate is transferred before starting the titration Two drops of indicator will then be added to the solution and the Borax will be titrated with standardized 0125 M HCI The end point is determined when the color changes from blue to yellow This process will be repeated for another test tube at 45 C The process will be repeated again twice for each temperature of 35 C 25 C 15 C and 5 C for a total of ten titrations Observations Results and Data Sheets Table 11 Titration Data Titration Burettei mL Burettef mL 1 169 61 2 497 389 3 389 265 4 265 138 5 397 335 6 335 280 7 446 357 8 497 397 9 357 255 10 255 169 AmL 108 108 124 127 62 55 89 100 102 86 Test Temp Vol 10 Exp C 342 341 30J5 29 222 222 1815 191 12f7 14f7 HCI L 0108 0108 0124 0127 0062 0055 0089 0100 0102 0086 Table 12 Titration Calculations 34050H42 39 M 135 135 155 159 078 069 111 125 128 108 Kw 984x1 03 984X1 03 L49X1 2 L61 X104 L90 x103 L31 X103 5A7 x103 39L81 X103 839 x103 5103 X103 In Ksp T C 45 45 35 35 25 25 15 15 T K 307 1 307 303 302 295 295 291 292 285 287 1T K 32 6 x1039 3 32 6 X1039 3 32 9 x1039 3 133 O X10 3 33 9 x1039 3 I33 9 X1039 3 3A 3 x1039 3 3A 2 X1039 3 35 0 x1039 3 3A 8 X1039 3 AGP fro Sp 1180 1180 1060 1040 1540 1630 1260 1170 1140 1270 0 AHP 3181 3181 3181 3181 3181 3181 3181 3181 3181 3181 3 AS 1179 1180 1203 1207 1258 1257 1280 1278 1319 1306 Example Calculations Graph Equation y38265x7841 Graph 11 ansp vs 1T 0 0 0 0 0 0 0 0 0 1 2 3 In Ksp 4 5 6 7 1T K DiscussionConclusions Based on Le Chatelier s principle it one added more solid borax to a saturated solution of borax at equilibrium the additional solid borax would not dissolve A saturated aqueous solution means that the maximum amount of solid which can be dissolved in a given amount of water is present If one added more B4O5OH4239 ions to the saturated solution of borax the common ion decreases solubility and cause the equilibrium to shift towards the reactants causing precipitation Dissolving borax in water is an endothermic reaction because the sign of AH is positive which means the reaction is absorbing heat from the surroundings not releasing it The equilibrium constant increases as temperature increases and decreases as temperature decreases This happens because heat is a reactant When temperature increases the equilibrium shifts towards the products or speeds up When temperature decreases the equilibrium shifts towards the reactants or slows down The accepted value of Ksp at 25 C for the dissolution of borax is 176x102 Compared to the average value calculated in this lab at 25 C the percent error equals 909 With a 909 error some sources of error in this lab could be the accuracy of the temperature of borax solution and mL of HCI used to titrate Although the temperature of the borax solution was taken immediately after being removed from its bath this lab section had to retrieve the solution from a different lab room and bring it back before titrating which allowed time for the temperature to fluctuate before adding HCI The amount of mL of 125 M HCI could also be off because it is difficult for one to stop the burette at the exact moment the indicator changes from blue to yellow The wrong amount of mL recorded could have affected the concentration of B4O5OH4239 which is turn would affect the KSID leading to the high percent error calculated This experiment taught the lab how a titration can be used to find the concentration of ions in a solution With that concentration one can calculate the solubility constant to find the change in free energy entropy and enthalpy


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