Given the following dataDissolved Oxygen Titration DataTrial 1Preparation of titrant0.4455 g NazS203•5H20 in 50.0 mL waterMass of water sample used (g)5.21 gInitial mass of Na2S203 soln andBeral pipet(g)12.40 gFinal mass of Na2S203 soln and Beralpipet(g)12.20 gMW of Na2S203•5H2O248.11 g/molMW of NazS203158.11 g/molMW of O232 g/molCalculate the following:a) Concentration of Na2S203•5H20 in mol/gc) DO of sample (ppm)Final answer: 3 significant figures

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Given the following data Dissolved Oxygen Titration Data Trial 1 Preparation of titrant 0.4455 g Na2S203 5H20 in 50.0 mL water Mass of water sample used (g) 5.21 g Initial mass of NazS203 soln and Beral pipet(g) 12.40 g Final mass of Na2S203 soln and Beral 12.20 g pipet(g) MW of Na2S203•5H2O 248.11 g/mol MW of Na2S203 158.11 g/mol MW of O2 32 g/mol Calculate the following: a) Concentration of Na2S203•5H20 in mol/g c) DO of sample (ppm)

Given the following data Dissolved Oxygen Titration Data Trial 1 Preparation of titrant 0.4455 g Na2S203 5H20 in 50.0 mL water Mass of water sample used (g) 5.21 g Initial mass of NazS203 soln and Beral pipet(g) 12.40 g Final mass of Na2S203 soln and Beral 12.20 g pipet(g) MW of Na2S203•5H2O 248.11 g/mol MW of Na2S203 158.11 g/mol MW of O2 32 g/mol Calculate the following: a) Concentration of Na2S203•5H20 in mol/g c) DO of sample (ppm)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 93QRT: When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence...

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When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Potassium hydrogen phthalate, known as KHP (molar mass = 204.22 g/mol), can be obtained in high purity and is used to determine the concentration of solutions of strong bases by the reaction HP(aq)+OH(aq)H2O(l)+P2(aq) If a typical titration experiment begins with approximately 0.5 g KHP and has a final volume of about 100 mL, what is an appropriate indicator to use? The pKa for HP is 5.51.
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?
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