## mass of iron ore is 3842 g and volume of kmno4 is 7 ml

#### Iron weight to volume conversion - Aqua-Calc

About Iron; 7 873 kilograms [kg] of Iron fit into 1 cubic meter; 491.49533 pounds [lbs] of Iron fit into 1 cubic foot; Iron weighs 7.873 gram per cubic centimeter or 7 873 kilogram per cubic meter, i.e. density of iron is equal to 7 873 kg/m³; at 20°C (68°F or 293.15K) at standard atmospheric pressure.In Imperial or US customary measurement system, the density is equal to 491.4953 pound per ...

#### Oxidation – Reduction Titration: Determination of Iron ...

Introduction: In this experiment, oxidation/reduction (or redox) will be used in the titration analysis of an iron compound. We will use potassium permanganate, KMnO4, as the titrant in the analysis of an unknown sample containing iron to determine the percent iron by mass in the sample.

#### Pearson Education

Table 1 Analysis of an Unknown Iron-Containing Ore. Initial Volume of KMnO4 48.65 mL Final Volume of KMnO4 23.35 mL Volume of MnO4– Moles MnO4– Moles Iron(II), Fe2+ Mass of Iron % of Iron in Ore 1. Match each component from the following list with the correct number shown in Figure 1. The same number may be used more than once.

#### (DOC) COURSE CODE : CHM 138 EXPERIMENT 6 REDOX

c) APPARATUSSince the colour of the KMnO4 solution is quite intense, you may be required to give a good estimate of the burette volume. 3. On an analytical balance, 8 g FeSO4 weighed accurately using weighing paper. The mass of FeSO4 recorded. 4. With the aid of a filter funnel, the FeSO4 transferred carefully to a 250 mL volumetric flask.

#### I need Chemistry Help? Yahoo Answers

Oct 26, 2008 A 1.362 g sample of an iron ore that contained Fe3O4 was dissolved in acid and all the iron was reduced to Fe2+. The solution was then acidified with H2SO4 and titrated with 39.42 mL of 0.0281 M KMnO4, which oxidized the iron to Fe3+. The net ionic equation for the reaction is 5Fe2+ + MnO4- + 8H+ 5Fe3+ + Mn2+ + 4H2O. What was the percentage by mass of iron in the ore?

#### Determination of Iron in Ore by Redox Titration

Dilute the solution to volume. Transfer four 25 mL aliquots of the solution to four 200 mL Erlenmeyer flasks. Warm the solution gently and perform the pre‐reduction of the iron as described above. Once the samples have been pre‐reduced, you may proceed with the titration of the iron ore samples with Ce4+ as described above.

#### The iron content of iron ore can be determined by ...

The iron content of iron ore can be determined by titration with a standard KMnO 4 solution. The iron ore is dissolved in HC1, and all the iron is reduced to Fe 2+ ions. This solution is then titrated with KMn0 4 solution, producing Fe 3+ and Mn 2+ ions in acidic solution. If it required 38.37 mL of 0.0198 M KMnO 4 to titrate a solution made from 0.6128 g of iron ore, what is the mass

#### Experiment 16 Help!!! - uml.edu

By determining the exact mass of the FAS samples taken, and from the volume of KMnO 4 solution required to titrate those samples, the exact molarity of the KMnO 4 solutions could be calculate.. In the second week of the experiment, you titrated samples of an "unknown" iron(II) salt with the same KMnO 4 solution, in order to determine what % by mass of Fe it contained.

#### Solved: A sample of iron ore weighing 0.2792 g was ...

A sample of iron ore weighing 0.2792 g was dissolved in an excess of a dilute acid solution. All the iron was first converted to Fe(II) ions. The solution then required 23.30 mL of 0.0194 M KMnO 4 for oxidation to Fe(III) ions. Calculate the percent by mass of iron in the ore.

#### Iron (Fe) - Atomic Mass Number, Melting Point, Chemical ...

Iron is represented as Fe and has an atomic number of 26. Iron atomic mass is 55.845 u. Know the physical and chemical properties, density, boiling and melting point, along with the uses of Iron on BYJU'S.

#### Pearson Education

Table 1 Analysis of an Unknown Iron-Containing Ore. Initial Volume of KMnO4 48.65 mL Final Volume of KMnO4 23.35 mL Volume of MnO4– Moles MnO4– Moles Iron(II), Fe2+ Mass of Iron % of Iron in Ore 1. Match each component from the following list with the correct number shown in Figure 1. The same number may be used more than once.

#### (DOC) COURSE CODE : CHM 138 EXPERIMENT 6 REDOX

c) APPARATUSSince the colour of the KMnO4 solution is quite intense, you may be required to give a good estimate of the burette volume. 3. On an analytical balance, 8 g FeSO4 weighed accurately using weighing paper. The mass of FeSO4 recorded. 4. With the aid of a filter funnel, the FeSO4 transferred carefully to a 250 mL volumetric flask.

#### ChemTeam: Redox Titration

Problem #2: Potassium dichromate is used to titrate a sample containing an unknown percentage of iron. The sample is dissolved in H 3 PO 4 /H 2 SO 4 mixture to reduce all of the iron to Fe 2+ ions. The solution is then titrated with 0.01625 M K 2 Cr 2 O 7, producing Fe 3+ and Cr 3+ ions in acidic solution. The titration requires 32.26 mL of K 2 Cr 2 O 7 for 1.2765 g of the sample.

#### Experimental - Redox titrations - analysis of iron(II)

Data processing. Moles of manganate(VII) = 0.01 x 0.01 = 0.0001 mol. Therefore, from the reaction stoichiometry, moles of iron(II) = 5 x 0.0001 = 5.00 x 10-4 mol. This is in 27.90 ml, therefore in 250 ml there is (250/27.9) x 5.00 x 10-4 = 8.96 x 5 x 10-4 moles of iron = 4.48 x 10-3 mol. Therefore mass of iron in 250 ml = 56 x 4.48 x 10-3 g = 0.25 g. Hence, mass of iron

#### Chemistry Chapter 6 You'll Remember Quizlet

A 1.45 g sample of an iron ore is dissolved in acid and the iron obtained is Fe2+(aq). To titrate the solution, 21.6 mL of 0.102 M KMnO4(aq) is required. What is the percent of iron in the ore?

#### The mass percent of iron in an iron ore can be determined ...

Sep 27, 2011 The mass percent of iron in an iron ore can be determined by converting Fe to Fe2+ in acid solution, and then titrating the dissolved sample with KMnO4 solution. A 2.51 g ore sample dissolved in acid required 28.62 mL of 0.0821 M KMnO4 to react the equivalence point.

#### CHEMISTRY LAB REPORT NAME NUR FARAHIN BINTI AGOS ...

2 . Analysis of ore Trial 1 Trial 2 Trial 3 Weight of iron ore (g) 0.2017 0.2017 0.2017 Final burette reading (mL) 23 21.20 21.00 Initial burette reading (mL) 0.00 0.00 0.00 Volume of KMnO4 (mL) 21.20 21.20 21.00 Questions : 1 .

#### EXPERIMENT 7 REDOX REACTION.docx - NAME OF PROGRAMME ...

Analysis of ore Trial 1 Trial 2 Weight of the iron ore (g) 1.010 g 1.003 g Final buret reading (mL) 19.1 mL 26.8 mL Initial buret reading (mL) 11.3 mL 14.1 mL Volume of KMnO4 (mL) 7.8 mL 7.7 mL ABSTRACT The aim of this experiment was to standardize the potassium permanganate solution and to determine the composition of metal by titration method.

#### Titrimetric Redox of Iron in an Ore Using Dichomate

Weigh out three samples of about 0.5 g into 500 mL conical flasks. Add 25 mL of 6 M HCl to each flask; cover with a watch glass and, in the fume hood, heat below boiling until the iron ore dissolves (about 20 minutes). The solution will turn yellow as the iron dissolves and Fe(III) is complexed with chloride ion.

#### Determination of Iron in Ore by Redox Titration

Dilute the solution to volume. Transfer four 25 mL aliquots of the solution to four 200 mL Erlenmeyer flasks. Warm the solution gently and perform the pre‐reduction of the iron as described above. Once the samples have been pre‐reduced, you may proceed with the titration of the iron ore samples with Ce4+ as described above.

#### Pearson Education

Table 1 Analysis of an Unknown Iron-Containing Ore. Initial Volume of KMnO4 48.65 mL Final Volume of KMnO4 23.35 mL Volume of MnO4– Moles MnO4– Moles Iron(II), Fe2+ Mass of Iron % of Iron in Ore 1. Match each component from the following list with the correct number shown in Figure 1. The same number may be used more than once.

#### ap07 chemistry q5 - College Board

(ii) The mass of iron in the sample, in grams mass Fe = 5 × M × V × 55.85 g mol−1 OR mass Fe = mol Fe2+ × 55.85 g mol−1 One point is earned for the answer in part (d)(i) multiplied by 55.85. (iii) The mass percent of iron in the compound mass % Fe = 5 55.85×××MV g × 100 OR mass % Fe = mass Fe g × 100 One point is earned for the ...

#### (DOC) COURSE CODE : CHM 138 EXPERIMENT 6 REDOX

c) APPARATUSSince the colour of the KMnO4 solution is quite intense, you may be required to give a good estimate of the burette volume. 3. On an analytical balance, 8 g FeSO4 weighed accurately using weighing paper. The mass of FeSO4 recorded. 4. With the aid of a filter funnel, the FeSO4 transferred carefully to a 250 mL volumetric flask.

#### The iron content in ores can be determined by titrati...

The ore is first dissolved in hydrochloric acid, forming iron (II) ions, which react with permanganate ions according to the following net-ionic reaction: MnO4- (aq) + 5 Fe 2+ + 8H + (aq) → Mn 2+ (aq) + 5 Fe 3+ (aq) + 4 H 2O (l) A sample of ore of mass 0.202g was dissolved in hydrochloric acid, and the resulting solution needed 16.7 mL of 0 ...

#### Determination of iron (II) by permanganate titration

For 0.02 M titrant and assuming 50 mL burette, aliquot taken for titration should contain about 0.2-0.25 g of iron (3.5-4.5 millimoles). end point detection As usual in the case of permanganate titrations, pink color of excess permanganate is strong enough so that there is

#### Chapter 4 Flashcards by Dorothée Viau Brainscape

(0.0195 mol KMnO4 / 1L) X 0.02435= 0.000475 mol KMnO4 Step 3: use the stoichiometric factor to calculate the amount of iron (ii) ion 0.000475 mol KMnO4 X (5 mol Fe / 1 mol KMnO4) = 0.00237 mol Fe Step 4: calculate the mass of iron 0.00237 mol Fe X (55.85g Fe / 1 mol Fe) = 0.133g Fe Step 5: determine the mass percent 0.133g Fe / 1.026 g sample ...

#### Determination Of Iron By Redox Titration Answers

Therefore mass of iron in 250 ml = 56 x 4.48 x 10-3 g = 0.25 g. Hence, mass of iron per tablet = 250 mg Experimental - Redox titrations - analysis of iron(II) The mass percent of iron (8.29 or 6.85 in data) in each sample was calculated from the mass of iron present in each unknown sample (0.0849g and

#### The mass percent of iron in an iron ore can be determined ...

Sep 27, 2011 The mass percent of iron in an iron ore can be determined by converting Fe to Fe2+ in acid solution, and then titrating the dissolved sample with KMnO4 solution. A 2.51 g ore sample dissolved in acid required 28.62 mL of 0.0821 M KMnO4 to react the equivalence point.

#### 0.804 g sample of iron ore was dissolved in acid. Iron was ...

Click here👆to get an answer to your question ️ 0.804 g sample of iron ore was dissolved in acid. Iron was reduced to + 2 state and it required 47.2 mL of 0.112 N KMnO4 solution for titration. Calculate the percentage of iron of Fe3O4 in the ore.

#### Chapter 4 Test Flashcards by Irina Soloshenko Brainscape

A sample of iron ore has a mass of 2.47 g. The sample is dissolved in an acidic solution, and the iron is titrated with 35.3 mL of a 0.120 M solution of K2Cr2O7. What is the percent by mass of iron in the ore? (Assume that all of the iron from the sample exists as Fe2+ in solution. The net ionic equation of the redox reaction is shown below.)

#### Titration Questions and Answers Study

The iron content of iron ore can be determined by titration with a standard KMnO4 solution. The iron ore is dissolved in HCl, and all the iron is reduced to Fe^2+ ions. ... A volume of 96.47 mL of ...

#### Convert moles Iron to grams - Conversion of Measurement Units

7 moles Iron to grams = 390.915 grams. ... Finding molar mass starts with units of grams per mole (g/mol). When calculating molecular weight of a chemical compound, it tells us how many grams are in one mole of that substance. The formula weight is simply the weight in atomic mass units of all the atoms in a given formula.

#### Permanganate Titrations - Buffalo State College

2. Knowing the molarity of your Fe(II) solution then allows you to calculate the number of moles of iron (as Fe 2+) in your unknown sample and the mass of Fe in g: mass(Fe) = (moles Fe) ´ (55.85 g Fe/mole Fe) m(Fe)=55.85 x (total volume) x molarity(Fe(II)) Take into account that your total volume is 100 mL and atomic weight of Fe is 55.85. 5.