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

Answered: Image /qna-images/answer/8b7d1354-c275-4988-a866-49f974259843.jpg

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

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...

See similar textbooks

Similar questions

A student determined the concertration of NaOCI in a commercial bleach sample using the same technique described in section "F" of the Halogens and Their Compounds lab. The student required 18 drops of 0.01M Na25203 to reach the end point. What is the concentration (reported in percentage) of NaOCI in the bleach sample?
Nitesh
Perform the necessary calculations for the preparation of: a) 200 mL of AgNO3 0.50 M from the solid reagent b) 1 L of HCl 0.25 M and N, consider the purity and density of the acid to perform the calculations c) 100 mL of potassium dichromate K2Cr2O7 (294.185 g/mol) 0.2 N
Number 1_ A 0.5707-g sample of a water-soluble fertilizer was dissolved and analysed for nitrogen using the Kjeldahl method. After digestion, the distilled ammonia was collected in 100 mL of 0.1334 M boric acid. This solution required 26.27 mL of 0.202 M HCl for titration to the methyl red end point. Calculate the % N (AW =14 g/mol) in the fertilizer.
A solution of 0.1789 M phosphoric acid is used to standardize an unknown solution of sodium hydroxide according to the following equation: H3PO4 + 3 NaOH → Na3PO4 + 3 H20 After performing a quick titration, the following data was collected: Trial 1 Trial 2 Initial volume H3PO4 (mL) 0.13 8.75 Final volume H3PO4 (mL) 15.73 24.08 Initial volume NaOH (mL) 11.40 0.08 Final volume NaOH (mL) 33.06 21.38 What is the concentration of the sodium hydroxide in trial 1? Enter your numerical answer with a leading zero and appropriate sig figs. Do not enter a unit. What is the concentration of the sodium hydroxide in trial 2? Enter your numerical answer with a leading zero and appropriate sig figs. Do not enter a unit. What is the average concentration of the sodium hydroxide? Enter your numerical answer with a leading zero and appropriate sig figs. Do not enter a unit. What is the unit for all of these concentrations?
How many grams of Pb(10₂)2 (Kap-3.7x10-13) will dissolve in 500. mL of a 0.0042 M PbCl₂ solution? (Ksp -1.7x10-5)
Part C. Determination of Unknown Balanced chemical equation: Hcl+ Na OH -o Nacl t Hg0 Unknown number NA Trial 1 Trial 2 Trial 3 Volume of unknown HCl titrated 10.00mL NA NA Initial burette reading 0.90mL Final burette reading 30.90mL Volume NaOH added 20 00ML 50.00MLXO.144 m=43.2m moles NaOH added 4.335m (Use average molarity from part B and multiply it by the volume you added) 0.4335 M moles HCl 4.335m 04335m 10.00 mL molarity of HCl Actual Molarity (from instructor) 0.3150M percentage error
In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary experimental procedures were performed on it and the titrant consumption was found to be 7.9 mL. What is the KMnO4 concentration? A. 0.040B. 0.044C. 0.021D. 0.027
2 Match the following acid-base titration plots with the correct titrant and sample. Veq = 20.00 mL mea a. b. Hd (1) Titrant: Strong Acid; Sample: Strong Base (2) Titrant: Strong Base; Sample: Strong Acid (3) Titrant: Strong Acid; Sample: Weak Base (4) Titrant: Strong Base; Sample: Weak Acid 3219 11 10 9 8 7 6 5 4 3 2 1 0 14 13 12 11 10 9 8 7 6 5 4 3 2 1 0 0 0 5 5 10 10 15 Volume 15 Volume 20 20 25 25 30 30
Standardization of 1N H2SO4 Titration 1 Titration 2 Titration 3 Titration 4 Mass of flask and Sodium Carbonate 1.5067 g 1.5098 g 1.5076 g 1.5077 Final buret reading (mL) 22 mL 22mL 21.5 mL 22.5 mL Volume of Sulphuric acid used (mL) 30 mL 30 mL 30 mL 30 mL What is the result of my titration?
ry-144 021 / Natural Sciences Chemistry And Polymer Science Chemie - Chemistry - 144 Praktika 2 Verslag Watter komponent van die vo oplossing het tydens Experim tydens die byvoeging van die During Experiment 2, what component of the prepared buffer solution reacted during the addition of the strong base, NAOH? Select one or more: The conjugated base of the weak acid. Die gekonjugeerde basis van die swak suur. The acetic acid molecules. Die asynsuur molekules. No reaction takes place as buffers are able to resist any changes in solution. Geen reaksie vind plaas nie want buffers kan veranderinge weerstaan in oplossing. The acetate ions. Die asetaat ione. The conjugated acid of the weak base. Die gekonjugeerde suur van die swak basis.
Molarity of NaOH Solution 0.15 M NaOH Trial 1 Trial 2 Trial 3 Mass of diprotic acid (H2A) 0.242 g 0.222 g 0.223 g Volume of NaOH soln. titrated 32.50 mL 31.2 mL 30.01 Moles of NaOH 0.004875 0.004875 0.004875 Moles of diprotic acid (H2A) Calculated Molar mass of acid (H2A) Average Molar Mass of diprotic acid (H2A)