The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 6.05 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 23.7 mL of a 0.145 M aqueous solution of KBrO, (aq). The unbalanced equation for the reaction is BrO, (aq) + Sb³+(aq) Br (aq) + Sb3+ (aq) (unbalanced) Calculate the amount of antimony in the sample and its percentage in the ore. mass of antimony: percentage of antimony:

The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 6.05 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 23.7 mL of a 0.145 M aqueous solution of KBrO, (aq). The unbalanced equation for the reaction is BrO, (aq) + Sb³+(aq) Br (aq) + Sb3+ (aq) (unbalanced) Calculate the amount of antimony in the sample and its percentage in the ore. mass of antimony: percentage of antimony:

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

Complete and balance the following redox equations using the smallest whole-number coefficients. The reaction takes place in a BASIC solution. CrO42–(aq) + Cu (s) → Cr(OH)3 (s) + Cu(OH)2 (s) In the balanced equation, 3 molecules of water are present on the product side. In the balanced equation, 3 molecules of water are present on the reagent side. In the balanced equation, 4 OH- are present on the reagent side. In the balanced equation, 4 OH- are present on the product side. In the balanced equation, 5 molecules of water are present on the product side. In the balanced equation, 5 molecules of water are present on the reagent side.
Determine if the following reaction is a redox reaction. Use evidence from the equation to explain your reasoning. Cu(s)+NO3(aq) yields NO(g)+Cu+2(aq)
The quantity of antimony in an ore can be determined by an oxidation-reduction titration with an oxidizing agent. The ore is dissolved in hot, concentrated acid and passed over a reducing agent so that all of the antimony is in the form of Sb³+(aq). The Sb3+ (aq) is completely oxidized by an aqueous solution of BrO, (aq). Complete and balance the equation for this reaction in acidic solution. equation: Question Source: McQuarrie, Rock, And Gallogly 4e-General Chemsitry| Publisher: University Science Search or type URL
AaBbCcDc AaBbCcDc AAB6CC AaBbCcD AaB 三 . 1 Normal 1 No Spac.. Heading 1 Heading 2 Title Paragraph Styles 2) Four metals (A, B, C, and D) were studied for activity, and the following information was collected on the reactions between the metals and their salts: I) 2 A (s) + C(NO3)2 (ag) → No Reaction II) C (s) + 2 BCI (ag) → CC12 (ag) + 2 B (s) III) D (s) + B2S04 (ag) → DSO4 (ag) + 2 B (s) IV) 2 B (s) + 2 HCI (ag) → BC12 (ag) + H2 (g) V) D (s) + 2 AÑO3 (ag) → No Reaction a) Based on the above results, indicate the more reactive metal for each reaction: Most reactive> least reactive b) Would you expect A to react with sulfuric acid? Explain. 3)
Balance the following oxidation-reduction reaction that occurs in an acidic solution using the half-reaction method. I(aq) + Clo-(ag) → I3¯(aq) + CI-(aq) HOW DO WE GET THERE? For the reduction half-reaction, which half-reaction correctly balances the elements on both sides? ClO (aq) + H2O(1) → CI-(aq) + 2 H*(aq) clo-(aq) → Cl-(aq) 2 H+(aq) + ClO-(aq) → Cl-(aq) + H20(I) Clo-(aq) → CI-(aq) + H20(1) Clo-(aq) → Cl(aq) + H20(1) + 2 H*(aq) Check Next (4 of 6)
Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H 2C 2O 4 and H 2O in the balanced reaction? MnO 4⁻( aq) + H 2C 2O 4( aq) → Mn 2+( aq) + CO 2( g) H2C2O4 = 5, H2O = 8 H2C2O4 = 1, H2O = 4 H2C2O4 = 5, H2O = 1 H2C2O4 = 1, H2O = 1 H2C2O4 = 3, H2O = 2
Balance the following reaction in acidic solution. Cr2O, (ag) + HNO,(aq) → Cr* (aq) + NO, (aq) 3 Fill in the coefficients for the balanced overall equation. HNO, + -- v H* + -v Cr.O,* → -- ♥ NO, +- Cr3+ + Cr,O, - H.O --V
Use the relative strengths of nonmetals and metals as oxidizing and reducing agents, as indicated in the following unbalanced equations, to construct a table of half‐reactions. Ag (s) + Br2 (l) → AgBr (s) Ag (s) + I2 (s) → no evidence of reaction Cu2+ (aq) + I‐ (aq) → no redox reaction Br2 (l) + Cl‐ (aq) → no evidence of reaction
6. The following reaction forms a white precipitate. Is this a redox reaction? AgNO3(aq) + HCl(aq) → HNO3(aq) + AgCl(s)
Balance the following redox reaction in the gas phase. Note that this reaction cannot be balanced with the half-reaction method and must be done by inspection. In the gas phase, H2 O (1) is used to balance oxygen atoms and H3 O+ and OH are not available for balancing purposes. ONLY integers should be used in your answer. NH3 (aq) + O2 (g) –→ NO2 (g) Enter your chemical notation here
Balance the following redox reaction in BASIC conditions. Once you complete the balancing use your workings to answer four questions on this quiz. Mn2+ (aq) + BiO3 → Biš+ (aq) + MnO4 (aq) (aq) In the final balanced BASIC reaction, which statement is true? There is no water in the final balanced reaction There are 7 water molecules on the reactant side There are 7 water molecules on the product side There are 14 water molecules on the reactant side There are 14 water molecules on the reactant side and 7 water molecules on the product side
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?