Quiz. C...According to the activity series, which of the following metals willreact with HCI to produce H2(g)? Select any that apply.MetalOxidation ReactionLi(s)* K(s)Ba(s)Li (aq) + eK*(aq) + eBa2+(aq) + 2eCa2" (aq) + 2eNa*(aq) + eLithiumPotassiumBariumCa(s)Na(s)Mg(s)Al(s)Mn(s)Zn(s)Cr(s)Fe(s)Co(s)Ni(s)Sn(s)Pb(s)H2(g)Cu(s)Ag(s)Hg(!)Pt(s)Calcium>SodiumMg2 (aq) + 2eAl3+ (aq) + 3eMagnesiumAluminumMn2"(ag) + 2eZn2*(aq) + 2eCr (aq) + 3eFe2*(aq) + 2eManganeseZincChromium>IronCobaltCo2* (aq) + 2e>Ni2*(aq) + 2eSn2 (aq) + 2e2*(aq) + 2eNickel>TinLeadPb2+HydrogenCopper2 H (aq) + 2e2+Cu?"(aq) + 2e>Ag*(aq) + e>SilverHg2"(aq) + 2ePt2*(aq) + 2e>MercuryPlatinumGoldAu(s)Au3+(aq) + 3e

In the activity series, on moving from above to below in the activity series, there is a lower…

According to the activity series, which of the following metals will react with HCI to produce H2(g)? Select any that apply. Metal Oxidation Reaction Li*(ag) + e K*(aq) + e → Ba2*(aq) + 2e → Ca2 (aq) + 2e Na*(ag) + e Li(s) * K(s) Ba(s) Ca(s) Na(s) Mg(s) Al(s) Mn(s) Zn(s) Cr(s) Fe(s) Co(s) Ni(s) Sn(s) Pb(s) H2(g) Cu(s) Ag(s) Hg(!) Pt(s) Lithium Potassium Barium Calcium Sodium -> Mg (aq) + 2e 3+ → Als*(aq) + 3e 2+ Magnesium Aluminum - Mn2 (aq) + 2e Zn2+(aq) + 2e Cr (aq) + 3e Manganese - Zinc Chromium > Iron F 2+(aq) +2e Co2* (aq) + 2e Ni2*(aq) + 2e Sn2*(aq) + 2e → Pb2*(ag) + 2e 2 H (aq) + 2e Cu"(aq) + 2e Ag (aq) + e Cobalt > Nickel Tin > 2+ Lead Hydrogen Copper > Silver Hg"(aq) + 2e Pt2*(aq) + 2e > Mercury Platinum Gold Au(s) Au (aq) + 3e

According to the activity series, which of the following metals will react with HCI to produce H2(g)? Select any that apply. Metal Oxidation Reaction Li(ag) + e K(aq) + e → Ba2(aq) + 2e → Ca2 (aq) + 2e Na(ag) + e Li(s) * K(s) Ba(s) Ca(s) Na(s) Mg(s) Al(s) Mn(s) Zn(s) Cr(s) Fe(s) Co(s) Ni(s) Sn(s) Pb(s) H2(g) Cu(s) Ag(s) Hg(!) Pt(s) Lithium Potassium Barium Calcium Sodium -> Mg (aq) + 2e 3+ → Als(aq) + 3e 2+ Magnesium Aluminum - Mn2 (aq) + 2e Zn2+(aq) + 2e Cr (aq) + 3e Manganese - Zinc Chromium > Iron F 2+(aq) +2e Co2 (aq) + 2e Ni2(aq) + 2e Sn2(aq) + 2e → Pb2(ag) + 2e 2 H (aq) + 2e Cu"(aq) + 2e Ag (aq) + e Cobalt > Nickel Tin > 2+ Lead Hydrogen Copper > Silver Hg"(aq) + 2e Pt2(aq) + 2e > Mercury Platinum Gold Au(s) Au (aq) + 3e

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 147CP: The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a...

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The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a pH meter at 25 00C is given by the equation where contains the potential of the reference electrode and all other potentials that arise in the cell that are not related to the hydrogen ion concentration. Assume that = 0.250 V and that a. What is the uncertainty in the values of pH and [H+] if the uncertainty in the measured potential is 1 m V ( 0.001 V)? b. To what precision must the potential be measured for the uncertainty in pH to be 0.02 pH unit?
a. Balance the following redox in acidic media C2O42- (aq) + MnO4- (aq) → CO2(aq) + Mn2+ (aq) b. If you titrated this reaction to determine the moles of C2O42-, the colormetric endpoint is pink due to the Mn2+. How many moles of the oxalate (C2O42-) existed in solution if 12 mL of 0.791M permanganate was needed to hit the endpoint?
Predict the product and balance redox reaction The presence of sulfuric acid , an excess KMnO4 will oxidize a chromic salt to dichromate and manganous ion.
A precipitate of AgCl + AgBr weighs 0.8132 gram. On heating in a current of chlorine, the AgBr is converted into AgCl, the mixture losing 0.1450 gram in weight. What was the percentage of chlorine in the original precipitate?
A precipitate of AgCl + AgBr weighs 0.8132 g. On heating on a current of Cl2, the AgBr is converted to AgCl, the mixture loses 0.1450 g in wt. Find the percentage Cl in the original sample.
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When an aqueous solution of CuSO, is electrolyzed copper metal is deposited. If a constant current was passed for 5.00 h and 404 mg of Cu (63.546) metal was deposited, what was the current?
Write balanced equations for the following reactions: HCOOH + MnO₄⁻ ----> CO₂ + Mn²⁺ in acidic solution
In the redox titration of FeCl2 with KMnO4, exactly what reaction is happening to make the voltage increase?
A redox titration is performed to investigate iron content in an alloy sample. The potential of titration is monitored against a standard hydrogen electrode at 25 °C. All materials needed for redox titration were prepared accordingly. The half reactions involved in his experiment are:Fe3+ + e ̄ → Fe2+ E° = 0.771 V I3 ̄ + 2e ̄ → 3I ̄ E° = 0.535 Va) Construct a balanced titration equation.b) Assess the E° for this redox reaction.c) Depict whether the name of pH indicator that could be used to determine the endpoint of thistitration.d) Given a 25 mL portion of 0.5 M Fe3+ was titrated with 1 M titrant. Calculate the volumeof titrant required to reach equivalence point.e) Evaluate the cell potential at this point if over-titrated by 2.50 mL.
4 If the glass and reference electrode are immersed in a buffer solution pH = 3.56 ,the electrode voltage was = -0.111V. when the two electrodes immersed in unknown solution , it was found that the voltage of the glass electrode = -0.041V. Calculate the pH of the unknown solutionUnknown