The quantity of antimony in an ore can be determined by an oxidation-reduction titration with an...
Question:
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 the antimony is in the form {eq}\rm Sb^{3+} {/eq} (aq). The {eq}\rm Sb^{3+} {/eq} (aq) is completely oxidized by an aqueous solution of {eq}\rm BrO_3^- {/eq} (aq). Write Complete and balance the equation for this reaction in acidic solution.
Redox Reactions:
A redox reaction is characterized by the simultaneous loss and gain of electrons in a chemical reaction. Oxidation involves the loss of electrons while reduction involves the gain of electrons.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerWrite Complete and balance the equation for this reaction in acidic solution.
The oxidation half-reaction is given below.
{eq}\rm...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Redox (Oxidation-Reduction) Reactions: Definitions and Examples
from
Chapter 2 / Lesson 12
288K
What is a redox reaction (oxidation reduction reaction)? Learn about redox reaction examples, balancing redox reactions, and the redox reaction definition.
Related to this Question
- 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 tha
- The quantity of antimony in 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 a
- The quantity of antimony in an ore can be determined by oxidation-reduction titration with an oxidizing agent. The ore is dissolved in hot, concentrated acid and passed over a reducing agent so that a
- The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 7.99-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
- The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 9.51 g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated H C l ( a q ) and passed over a reducing agent so that
- The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 8.29-g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated H
- The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 5.75-g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated H
- The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 9.57-g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated H
- The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 6.35 g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated H
- A quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 9.62 gram sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl (aq) and passed over a reducing agent so that all t
- The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 9.59-g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl solution and passed over a reducing agent so that al
- The quality of antimony in an ore can be determined by an oxidation-reduction titration with an oxidizing agent. The Ore dissolved in hot, concentrate acid and passed over a reducing agent so that all
- A 9.11-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 35.7 mL of a 0.145 M aqueous solution of K
- The amount of Fe in a 2.0008 g sample of iron ore was determined by a redox titration with K 2 Cr 2 O 7 . The sample was dissolved in HCl and the iron brought to a +2 oxidation state. Titration requir
- Manganese in an ore can be determined by treating the ore with a measured, excess quantity of sodium oxalate ( N a 2 C 2 O 4 ) to reduce M n O 2 ( s ) to M n C l 2 ( a q ) followed by determination of the unreacted sodium oxalate by titration with pot
- 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 Fe2+ ions. This solution is then titrated with KMnO4 solution, producing Fe3+ and Mn2+ ions in
- A sample of iron ore weighing 916 mg was dissolved in acid and pretreated to oxidize all of the iron to F e 3 + . After removing any remaining oxidizing agent, an excess of K I was added to the solution. The liberated iodine required 22.9 mL of 0.0934
- Heating an ore of antimony (Sb_2S_3) in the presence of iron gives the element antimony and iron(II) sulfide. Sb2S3(s) + 3Fe(s) ---> 2Sb(s) + 3FeS(s) When 15.0 g Sb_2S_3 reacts with an excess of Fe, ...
- 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. This solution is then titrated with a KMnO4 solution, producing Fe^3+ and Mn^2+ ions i
- Antimony is obtained by heating pulverized stibnite (Sb 2 S 3 ) with scrap iron and drawing off the molten antimony from the bottom of the reaction vessel. Sb 2 S 3 + 3Fe 2Sb + 3FeS Suppose that 0.600
- A 6.39-g sample of an ant-control preparation was decomposed by wet ashing with H2SO4 and HNO3. The arsenic in the residue was reduced to the trivalent state with hydrazine. After the excess reducing agent had been removed, the arsenic(III) was oxidized
- A 0.446-gram sample of iron ore is dissolved in HCl and the iron (Fe solid) is reduced to Fe2+. The solution is then titrated by 38.6 mL of 0.105 N KMn4. Calculate the percentage of Fe in the iron ore
- Assume that the iron in iron ore (a mixture of iron and other substances) is in the form of Fe3+. The iron content of iron ore can be determined by dissolving the iron ore in HCl. The dissolved Fe3+ (aq) from the iron ore is then reduced to Fe2+. e- + Fe3
- The iron content of ores can be determined by titrating a sample with a solution of KMnO_4. The ore is dissolved in HCl forming iron (II) ions, which react with MnO_4^-: 5Fe^{2+} (aq) + MnO_4^-(aq) + 8H^+(aq) \rightarrow 5Fe^{3+}(aq) + Mn^{2+} (aq) + 4H_
- A 2.0 g sample of silver alloy was dissolved in nitric acid and then precipitated as AgBr. After drying, the sample of silver bromide weighed 2.0 g. Calculate the percentage of silver in the alloy.
- Twenty dietary iron tablets with a total mass of 21.232 g were ground and mixed thoroughly. Then 2.898 g of the powder were dissolved in HNO_3 and heated to convert all iron into Fe^{3+}. Additional of NH_3 precipitated Fe_2O_3. xH_2O which was ignited to
- An iron ore sample weighting 0.5453 g is dissolved in HCl(aq), treated with a reducing agent to convert all the iron in sample to Fe2+(aq), and then titrated with exactly 32.77 mL of 0.02726 M K2Cr2O7
- Magnetite is a mineral having the formula Fe3O4 or FeOFe2O3. A 1.1324-g sample of a magnetite ore was dissolved in concentrated HCl to give a solution that contained a mixture of Fe^{2+} and Fe^{3+}. Nitric acid was added and the solution was boiled for a
- A taconite ore consisted of 35.43% Fe_3O_4 and the balance of siliceous impurities. How many tons of the ore must be processed in order to recover 1 ton of metallic iron?
- Thermite is a composition of metal powder and metal oxide. In this reaction, iron oxide solids, Fe_2O_3, and aluminum powder, Al, react exothermically to release a large large amount of heat. Aluminum
- A sample of 0.6805 g iron ore was dissolved in concentrated HCl. After the reduction of all Fee to Fe^{3+} with SnCl_2, the solution needed 45.50 ml of 0.515 M K_2 Cr_2O_7 to reach the endpoint. What is the % Fe in the ore? 6Fe^{2+} + Cr_2O_7^{2+} + 14H
- An 8.00 g sample of an iron ore was dissolved in an acid solution and the iron converted to the +2 oxidation state. The resulting solution took 75.0 mL of 0.200 M KMnO_4 solution to titrate to a light pink color.
- Stainless steel is an alloy of iron, chromium, and nickel, having approximately 15.5% chromium. In an assay to discover how much chromium is present, the steel is oxidize in acid to form chromate ion. The resulting solution is treated with excess lead(II)
- A solution of potassium permanganate is standardized with iron metal, a primary standard. The iron is dissolved in acid, reduced to Fe(II), and titrated with permanganate. 5Fe^2+(aq) + MnO_4^-(aq) + 8H^+(aq) to 5 Fe^3+(aq) + Mn^2+ + 4H_2O(l) 33.17 mL of p
- A sample of a tin ore weighing 0.3550 g was dissolved in an acid solution and all the tin in the sample was changed to tin(II). In a titration, 7.90 mL of 0.0401 M KMnO_4 solution was required to oxidize the tin(II) to tin(IV). (a) What is the balanced
- 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
- Extraction of metal from the ore cassiterite involves: (A) carbon reduction of an oxide ore. (B) self-reduction of a sulphide ore. (C) removal of copper impurity. (D) removal of iron impurity.
- The amount of iron in ore can be quantitatively determined by titrating a solution of the unknown with a standard solution of dichromate. The net ionic equation is as follows. 6Fe2+(aq) + Cr2O72-(aq) + 14H+(aq) arrow 6Fe3+(aq) + 2Cr3+(aq) + 7H2O(aq) The t
- A 0.855 g sample of ore of iron is dissolved in acid and converted to Fe(II). The sample is oxidized by 36.50 mL of 0.161 M ceric sulfate, Ce(SO4)2, solution; the cerium(IV) ion, Ce4+, is reduced to Ce3+ ion. What is the percent of iron in the ore?
- Liquid elemental iron is produced in the thermite reaction because enough heat is generated to melt the iron : 2 Al (s) + Fe_2O_3 (s) rightarrow Al_2O_3 (s) + 2 Fe (l). (a) What mass of aluminum
- Solder is an alloy, or mixture, of the metals tin and lead. A 1.50 g sample of solder is dissolved in acid and all of the Sn is oxidized to Sn^{2+}. The Sn^{2+} is reacted with a 0.0525 M solution of sodium dichromate according to the following net ionic
- State whether a physical process or a chemical reaction is involved in the separation of: Iron is produced from an iron ore that contains the substance iron(III) oxide.
- A sample of 0.6805 g iron ore was dissolved in concentrated HCl. After reduction of all Fe^(3+) to Fe^(2+) with SnCl2, the solution needed 45.50 ml of 0.515 M K2Cr2O7 to reach the end point. What is the % Fe in the ore? 6Fe^(2+) + Cr2O_(7)^(2-) + 14H^(+)
- A 0.8552g sample of copper alloy is treated with 8 molars nitric acid and filtered and the precipitate is ignited giving a residue of 0.0632g of SnO_2. The zinc is determined in one half of the filtra
- An iron ore was analyzed by dissolving a 1.1324 g sample in concentrated HCl. The resulting solution was diluted with water, and the iron (lI) was precipitated as the hydrous Fe_2O_3-xH_2O by the addition of NH_3.
- A 0.5962g sample of iron ore is dissolved in acid-producing Fe^{3+}. Through a series of reactions, the iron precipitates as the Fe(OH)_3. The precipitates is heated, forming solid Fe_2O_3. What is th
- The concentration of manganese in steel can be determined spectrophotometrically by dissolving the steel in acid and oxidizing Mn to MnO_4?. The resulting solution is purple and the absorbance at 525
- Estimate the temperature at which Fe_2O_3 can be reduced to iron, using hydrogen gas as a reducing agent (assume H_2O(g) is the other product).
- The mass fraction of eutectoid cementite in an iron-carbon alloy is 0.109. On the basis of this information, is it possible to determine the composition of the alloy? If so, what is its composition? If this is not possible, explain why.
- A 0.5962 g sample of iron ore is dissolved in acid, producing Fe3+. Through a series of reactions, the iron precipitates as the Fe(OH)3. The precipitate is heated, forming solid Fe2O3. What is the mas
- Iron ores have different amounts of iron per kilogram of ore. Calculate the mass percent composition of iron for each iron ore: Fe2O3 (hematite), Fe3O4 (magnetite), FeCO3 (siderite).
- A quantity of ore consist of 90% (by weight) chalcopyrite mineral with a composition of CuFeS_2. The rest is inert quartz, SiO_2. The ore is roasted by heating it in oxygen at 800 degree C. This pr
- O2F2 is a vigorous and potent oxidizing and fluorinating agent. Are oxidation states or formal charges more useful in accounting for these properties of O2F2?
- An important source of silver is its recovery as a byproduct in the metallurgy of lead. The percentage of Ag in the lead is determined as follows. A 1.050 g sample is dissolved in nitric acid producing Pb^{2+} (aq) and Ag^+ (aq). The solution was diluted
- A 0.6505 g sample of ferrite ore is dissolved in nitric acid. All of the iron present is oxidized to iron(III). The solution is filtered and made basic with addition of ammonium hydroxide. The iron precipitates as the iron(III) hydroxide hydrated solid. T
- Magnesium metal is placed in contact with an underground steel storage tank to inhibit the corrosion of the tank because: a. magnesium has a higher reduction potential than iron. b. magnesium has a lower oxidation potential than iron. c. magnesium is chea
- An alloy of iron and carbon was treated with sulfuric acid, in which only iron reacts. 2Fe(s) + 3H_2SO_4(aq) to Fe_2(SO_4)_3(aq) + 3H_2(g) If a sample of alloy weighing 2.358 g gave 0.1067 g of hydrogen, what is the percentage of iron in the alloy?
- An excess amount of chlorine was passed over hot iron fillings. The experiment yielded the following data: weight of crucible: 26.3821 g Weight of crucible plus iron fillings: 26.8511 g Weight of cruc
- A sample weighing 0.0123 g was dissolved in concentrated nitric acid to convert all of the arsenic to arsenate. The solution was diluted 10 times and excess silver added to precipitate silver arsenate (Ag_3 \cdot AsO_4), which was collected, dried, and we
- A total charge of 96.5 kC is passed through an electrolytic cell. Determine the quantity of substance produced in each of the following cases. (a) the mass (in grams) of silver metal from a silver nit
- Gold has always been a highly prized metal, widely used from the beginning of history as a store of value. It doesn't rust like iron and doesn't become tarnished like silver. It is so chemically inert that it won't react even with the strongest concentrat
- Sample of silver metal is suspected to be contaminated with zinc. A 0.2365 g portion of this metal is dissolved in nitric acid and the silver ions precipitated with excess aqueous NaCl. After filterin
- Using the following results, prepare a single table of relative strengths of oxidizing and reducing agents. Reaction 1: Cu (strongest reducing agent) I^- Ag Br^- (weakest reducing agent) Reaction 2: Zn(strongest reducing agent) Pb Cu Ag(weakest ...
- A sample of 1.55 g of iron ore is dissolved in a acid solution in which the iron is converted into Fe^{2+}. The solution formed is then titrated with KMnO_4 which oxidises Fe^{2+} to Fe^{3+} while the
- You are looking to reduce chromate (CrO42-) to Cr(OH)4- in a basic solution (E = -0.14 V). You are trying to decide between the following commonly used reducing agents: zinc metal (E = -0.762 V for Zn2+|Zn), magnesium metal (E = -2.360 V for Mg2+|Mg), a f
- Much lead ore is PbS in rock. The higher the percentage of lead in the rock, the better the ore. Suppose 9.543 grams of ore is heated, allowing the sulfur to burn off and the lead to melt and be separated from the rock, and 5.270 grams of lead is recovere
- A copper ore contains Cu2S and CuS plus 10% inert impurities. When 200 grams of the ore was roasted, it yielded 150.8 grams of 90.0% pure copper and sulfur dioxide gas. What is the percentage of Cu2S in the ore? Cu2S + O2 arrow 2Cu + SO2 CuS + O2 arrow Cu
- An electrolytic cell is used to separate copper from the impurities, that is, zinc, iron, silver, gold, and platinum. Can this process be used to separate the metals left after the copper has been removed?
- To determine the Ksp value of Hg2I2, a chemist obtained a solid sample of Hg2I2 in which some of the iodine is present as radioactive 131I. The count rate of the Hg2I2 sample is 5.0x10^11 counts per minute per mole of I. An excess amount of Hg2I2(s) is p
- For the following reactions, identify the limiting and excess reagents. Give reasons for choices. a) wood burning in a campfire b) subdue in the air with silver flatware to produce tarnish, or silver sulfide
- Zinc is more active chemically than is silver; it can be used to remove ionic silver from solution. The concentration of a silver nitrate solution is determined to be 1.330 mol/L. Pieces of zinc totaling 100.0 g are added to 1.000 L of the solution; 90.0
- Copper(II) oxide, CuO, may be formed when copper metal is gently heated in air or oxygen gas. Copper metal surfaces that have been tarnished by a layer of black CuO can be cleaned by treating the surface with dilute solutions of hydrobromic acid, HBr(aq).
- An iron ore sample is analyzed for iron content by dissolving it in acid, converting the iron to Fe^+2 and then titrating with standard 0.0150M K_2Cr_2 O_7 solution. If 32.05 mL is required to titrate
- a)What mass of chromium is present in 234 grams of an ore of chromium that is 55.0 % iron(II) dichromate, FeCr_2O_7, and 45.0 % impurities by mass? b) If 90.0 % of chromium can be recovered from 400 grams of the ore, what mass of pure chromium is obtained
- To assay silver content in an alloy, a 13.38 g sample of alloy was dissolved in nitric acid. The addition of 0.53 molar sodium chloride resulted in the precipitation of silver chloride. If the alloy w
- The concentration of manganese in steel can be determined spectrophotometrically by dissolving the steel in acid and oxidizing M n to M n O 4 . The resulting solution is purple and the absorbance at 525 nm can be monitored. A standard solution contai
- A mixture of 3.00 g of silver and copper metals was dissolved in excess nitric acid. Resulting salts, silver(I) nitrate and copper(II) nitrate, were isolated and dissolved in enough water to make 0.10
- The production of uranium metal from purified uranium dioxide ore consists of the following steps. UO2(s)+4HF(g) UF4(s)+2H2O(l). Identify the reducing agent.
- The large scale production of iron would involve: a) forming an amalgam. b) just purification as iron occurs freely in nature. c) the electrolysis of molten iron salt. d) reduction of an iron oxide with coke.
- A sample of rutile, an ore of titanium consisting principally of TiO_2(s), was found to be 65.2% TiO_2(s) by mass, with the remainder being sand impurities. What is the minimum number of metric tons of the ore that must be processed to obtain 10.0 metric
- The chief ore of zinc is the sulfide, ZnS. The ore is concentrated by flotation and then heated in air, which converts the ZnS to ZnO. 2ZnS + 3O_2 \to 2ZnO + 2SO_2 The ZnO is then treated with dilute H_2SO_4 to produce an aqueous solution containing the
- For a melting point determination, if the compound is less pure, then the melting point will generally be higher or lower and why? (a) Lower, impurities may react to form gasses which dissipate at room temperature (b) Lower, because defects in a crystal l
- Rank these species by their ability to act as an oxidizing agent. Na^+, I_2, Cr^{3+}, F_2. Put best oxidizing agent first and continue to have best reducing agent last.
- Gold has always been a highly prized metal, widely used from the beginning of history as a store of value. It doesn't rust like iron and doesn't become tarnished like silver. It is so chemically inert
- While trace impurities of iron and chromium in natural corundum form the gemstones ruby and sapphire, they are basically a binary compound of aluminum and oxygen, with 52.9% Al. Find the empirical for
- Tarnished silver is coated with a layer of Ag2S(s). The coating can be removed by boiling the silverware in an aluminum pan, with some baking soda or salt added to make the solution conductive. Explain this from the point of view of electrochemistry.
- Element M is a shiny and highly reactive metal (melting point 63^{\circ}C ), and element X is a highly reactive nonmetal (melting point -7.2^{\circ}C ). They react to form a compound with the empiri
- If iron filings are placed with excess powdered sulfur in a beaker, the iron filings are still attracted by a magnet and could be separated from the sulfur with the magnet. Would this combination of iron and sulfur represent a mixture or a pure substance?
- In a laboratory studying the extraction of iron metal from iron ore, the following reaction was carried out at 1270 K in a reaction vessel of volume 10.0 L: FeO(s) + CO(g) => Fe(s) + CO_2(g), at equilibrium the partial pressure of CO was 4.24 bar and that
- A student dissolved a piece of copper wire, then converted it to CuO, filtered the CuO from solution, and determined the mass of the CuO. The CuO was then dissolved, reduced to copper metal, and recov
- Powdered iron is magnetic, but powdered sulfur is not. What occurs when they form a mixture in a beaker at room temperature? a) The iron retains its magnetic properties. b) The iron loses its metallic properties. c) The sulfur gains magnetic properties. d
- Two experiments were conducted: 2.750 g of copper (II) oxide, CuO2, was reduced by heating at high pressure with excess hydrogen to yield 2.196 g of copper Cu. 1.179 g of copper Cu was dissolved in nitric acid to yield copper(II) nitrate, which was conver
- 1. Cu^2+/Cu, Zn^2+/Zn, Fe2+/Fe, H+/H2, I2/I- a. Arrange the oxidizing agents in order of their oxidizing strength. b. Arrange the reducing agents in order of their reducing strength. c. Compare the tr
- The compound with the formula TlI3 is a black solid. Given the following standard reduction potentials, TI^3++2e^- gives to TI^+ E^0=1.25 V I3^-+2e^- gives to 3I^- E^0=0.55 V would you formulate this compound as thallium(III) iodide or thallium(I) triiodi
- A sample of pressure-treated wood weighing 0.3245 g was dissolved in concentrated nitric acid to convert all of the arsenic to arsenate. The solution was diluted 10 times and excess silver added to precipitate silver arsenate (Ag_3AsO_4), which was colle
- A silver coin has a mass of 2.50 g and is analyzed for silver by dissolving in dilute nitric acid, and precipitating silver as solid AgCl and weighing this. If the precipitate weighs 2.99 g, what perc
- Elemental chlorine is obtained by the electrolysis of molten NaCl (Downs cell). Elemental fluorine is obtained by the electrolysis of KHF_2 in a cell made of Monel metal (a stainless steel alloy). Both of these processes are dangerous. Why?
Explore our homework questions and answers library
Browse
by subject