Use the following data to calculate the mass percent of oxalate in the sample:
Mass of sample: 0.200 grams
Starting buret volume: 12.48 mL
Final buret volume: 37.50 mL

Use the following data to calculate the mass percent of oxalate in the sample: Mass of...
Use the data below to determine the mmoles of sodium oxalate to 2 decimal places. (MM sodium oxalate = 134 g/mol) mass of sodium oxalate (g) 0.096 initial buret reading (mL) 0 final buret reading (mL) 16.37
Given the following data, determine the % by mass of oxalate (C2O42-) in a sample of an iron oxalate complex with the general formula Kz[Fex(C2O4)y].wH2O. The reaction between oxalate and permanganate is as follows : 6H+ + 5(COOH)2 + 2MnO4- → 10CO2 + 2Mn2+ + 8H2O m(iron oxalate complex) used for titration = 0.100 g C(KMnO4) standard solution = 0.0200 M M(C2O42-) = 88.02 g mol-1 Titre volume = 11.91 mL Enter your answer to 3 significant figures. Do not...
1. Calculations Given the following data, determine the % by mass of oxalate (C2O42-) in a sample of an iron oxalate complex with the general formula Kz[Fex(C2O4)y].wH2O. The reaction between oxalate and permanganate is as follows: 6H+ + 5(COOH)2 + 2MnO4- → 10CO2 + 2Mn2+ + 8H2O m(iron oxalate complex) used for titration = 0.100 g C(KMnO4) standard solution = 0.0200 M M(C2O42-) = 88.02 g mol-1 Titre volume = 10.18 mL Enter your answer to 3 significant figures. 2....
What is the percent by mass of oxalate ion in a 0.291 g sample of the iron salt that took 20.91 mL of 0.02073 M potassium permanganate to titrate to a light pink endpoint?
What is the percent by mass of oxalate ion in a 0.218 g sample of the iron salt that took 17.62 mL of 0.02006 M potassium permanganate to titrate to a light pink endpoint.
Question 13 Calculate the amount of dissolved oxygen (ppm 02) using the following data: • Sample volume (mL) = 224.893 • Buret Reading, initial (mL) = 3.581 • Buret Reading, final (mL) = 18.25 • Volume of Na2S203 dispensed (mL) = • Average molar concentration of Na2S203 (mol/L) = 0.0219 • Moles of Na2S203 dispensed (mol) = • Moles of 13° reduced by S2032-(mol) = • Moles of O2 (mol) = • Mass of O2 (mg) • Dissolved oxygen, ppm...
KMnO4 Molarity is .02107M
.02107
Oxidation-Reduction Titrations I: Determination of Oxalate Č. Analysis of Oxalate Complex or Unknown Mass of sample Trial Trial 2 Trial 3 Weighing bottle initial mass Weighing bottle final Mass of sample Titration Final reading Initial reading O,1121 Volume of KMnO4 Millimoles of oxalate, C,0,2- Mass of oxalate, C2042 Percent oxalate, C,042 Average percent oxalate If you analyzed your oxalate complex from your experiments, complete the following: Standard devia eoretical percent oxalate in your complex (show...
Calculate the moles of I3-reduced by S2O32- using the following data: Sample volume (mL) = 200.0 Buret Reading, initial (mL) = 3.85 Buret Reading, final (mL) = 18.25 Volume of Na2S2O3 dispensed (mL) = 14.4 mL Average molar concentration of Na2S2O3 (mol/L) = 0.02077 Moles of Na2S2O3 dispensed (mol) = __________ Moles of I3- reduced by S2O32- (mol) = __________ Hint: Compute for moles of Na2S2O3 first then use Equation 31.3 of your lab manual to convert it to moles...
QUESTION 5 What is the percent by mass of oxalate ion in a 0.175 g sample of the iron salt that took 16.37 mL of 0.02004 M potassium permanganate to titrate to a light pink endpoint.
In this experiment you will use an oxidation - reduction titration to determine the percent of oxalate ion, CO2 in an unknown sample containing oxalate ion. Potassium permanganate (KMnO.) will be titrated against the oxalic acid (C2H:08) as shown by the following oxidation-reduction reaction: +3 +7 5C,044 2MnO4 + 16H* → 10CO, 8H0 + 2Mn2 +4 + + Mno. Mn? is the reduction process C2042 → CO2 is the oxidation process The underlying principle behind a titration is that an...