A chemical engineer determines the mass percent of iron in an ore sample by converting the Fe to Fe²* in acid and then titrating the Fe²+ with MnO. A 1.2188 g sample was dissolved in acid and then titrated with 33.71 mL of 0.04327 M KMnO4. The balanced equation is SH (aq) + 5Fe (aq) + MnO (ag) → 5Fe³+ (aq) + Mn² (aq) + 4H₂0 (1) Calculate the mass percent of iron in the ore. Be sure your answer has the correct number of significant figures.

A chemical engineer determines the mass percent of iron in an ore sample by converting the Fe to Fe²* in acid and then titrating the Fe²+ with MnO. A 1.2188 g sample was dissolved in acid and then titrated with 33.71 mL of 0.04327 M KMnO4. The balanced equation is SH (aq) + 5Fe (aq) + MnO (ag) → 5Fe³+ (aq) + Mn² (aq) + 4H₂0 (1) Calculate the mass percent of iron in the ore. Be sure your answer has the correct number of significant figures.

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

Calculate the number of milliliters of 0.479 M Ba(OH)2 required to precipitate all of the Cr³+ ions in 156 mL of 0.725 M CrIs solution as Cr(OH)3. The equation for the reaction is: 2Crls (aq) + 3Ba(OH)2 (aq) → 2Cr(OH)s (8) + 3Bal, (aq) ml. Volume= Submit Answer Retry Entire Group 9 more group attempts remaining
Based on the balanced chemical equation shown below, determine the concentration (M) of Fe2+(aq) if 40.00 mL of the Fe2+(aq) solution is required to completely react with 43.47 mL of a 0.125 M bromate, BrO3-(aq), solution. The chemical equation for the reaction is 6 Fe2+(aq) + BrO3-(aq) + 6 H+(aq) → 6 Fe3+(aq) + Br-(aq) + 3 H2O(l) Do not type in units nor write in scientific notation.
The amount of I, (aq) in a solution can be determined by titration with a solution containing a known concentration of S,0 (aq) (thiosulfate ion). The determination is based on the net ionic equation 2 S,03 (aq) + I5(aq) → S,0 (aq) + 31(aq) Given that it requires 30.1 mL of 0.310 M Na, S,O, (aq) to titrate a 15.0 mL sample of I, (aq), calculate the molarity of I, (aq) in the solution. [I]= Question Source: MRG - General Chemistry Publisher: University Science Books
To measure the amount of calcium carbonate (CaCO3) in a seashell, an analytical chemist crushes a 4.20 g sample of the shell to a fine powder and titrates it to the endpoint with 302. mL of 0.210M hydrogen chloride (HCI) solution. The balanced chemical equation for the reaction is: 2HCl(aq) + CO3(aq) → H₂CO3(aq) + 2Cl¯ (aq) 1 What kind of reaction is this? If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of CaCO3 in the sample. Be sure your answer has 3 significant digits. precipitation O acid-base O redox 0 0 0 п% X
Wa 5. In a laboratory activity, Ca(OH)2(s) is completely dissolved in distilled water. This solution is then used to titrate a solution of HClag- Write the equation representing this neutralization reaction. Ca(OH):(aq) + HClI(aq) >
If 785 mL of 0.350 M AgNO₃ is added to 475 mL of 0.250 M CaBr₂, how many moles of AgBr precipitate will be formed? The balanced equation is 2 AgNO₃(aq) + CaBr₂(aq) → 2 AgBr(s) + Ca(NO₃)₂(aq)
The amount of chloride anion in a solution can be determined via titration with AgNO3(aq), according to the following balanced chemical equation: Cl–(aq) + AgNO3(aq) → AgCl(s) + NO3–(aq) What is the molarity of NaCl in a solution if titration of 15.00 mL of the solution with 0.2488 M AgNO3 requires 19.13 mL of the AgNO3 solution to reach the endpoint.
The amount of I−3(aq) in a solution can be determined by titration with a solution containing a known concentration of S2O2−3(aq) (thiosulfate ion). The determination is based on the net ionic equation 2S2O2−3(aq)+I−3(aq)⟶S4O2−6(aq)+3I−(aq) Given that it requires 33.5 mL of 0.430 M Na2S2O3(aq) to titrate a 15.0 mL sample of I−3(aq), calculate the molarity of I−3(aq) in the solution.
The quantity of antimony in a sample can be determined by an oxidation–reduction titration with an oxidizing agent. A 6.19 g6.19 g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl(aq) and passed over a reducing agent so that all the antimony is in the form Sb3+⁢(aq). The Sb3+⁢(aq) is completely oxidized by 30.5 mL of a 0.115 M aqueous solution of KBrO3⁢(aq). The unbalanced equation for the reaction is BrO^− 3(aq) + Sb^3+(aq)⟶Br^−(aq)+Sb^5+(aq)(unbalanced) Calculate the amount of antimony in the sample and its percentage in the ore. mass of antimony in grams: percentage of antimony:
A 25.00 mL sample of boric acid requires 32.57 mL of 0.2514 M NaOH to reach the endpoint of titration. H3BO3 (aq) + 3 NaOH (aq) → Na3BO3 (aq) + 3 H2O (l) Determine the concentration of boric acid in the sample. Write the full and net ionic equation for the reaction.
The amount of I (aq) in a solution can be determined by titration with a solution containing a known concentration of S₂O3(aq) (thiosulfate ion). The determination is based on the net ionic equation 2S₂O3(aq) + 13(aq) · → S₂O²(aq) + 31¯ (aq) Given that it requires 27.4 mL of 0.260 M Na₂S₂O3(aq) to titrate a 10.0 mL sample of 13 (aq), calculate the molarity of I3 (aq) in the solution. [H] = M
A sample of a chloride salt weighing 484.6 mg is titrated with AgNO3 using K2CrO4 as indicator. To reach the end point a 52.3 mL of 0.1475 M of AgNO3 solution is required. The net ionic equation for the reaction of titration is: Ag+ (aq) + Cℓ- (aq) → AgCℓ (s) How many moles of Ag+ (aq) ions are used to reach the end point? How many moles of Cℓ- (aq) have reacted in the titration? How many grams of chloride are present in the sample? What is the mass percent of chloride in the sample?