An MnO2(s) /Mn2+(aq) electrode in which the pH is 10.18 is prepared. Part A Find the...

An MnO2(s) /Mn2+(aq) electrode in which the pH is 10.18 is prepared. Part A Find the [Mn2+] necessary to lower the potential of the half-cell to 0.00 V (at 25 ∘C). Express your answer using two significant figures. [Mn2+] =

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queen_honey_blossom answered 2 years ago

Balance the following reaction, which occurs in basic solution. MnO4-(aq) + Br-(aq) --> MnO2(s) + BrO3-(aq)...

Balance the following reaction, which occurs in basic solution. MnO4-(aq) + Br-(aq) --> MnO2(s) + BrO3-(aq) Please show your work.

Balance the following question in basic medium: MnO4^- (aq) +BrO3^-(aq) > MnO2 (s) + BrO4^- (aq)

HClO(aq) = Cl2 (aq) Eo = + 1.611V MnO4-1(aq) = MnO2(s) Eo = + 1.679V In...

HClO(aq) = Cl2 (aq) Eo = + 1.611V MnO4-1(aq) = MnO2(s) Eo = + 1.679V In a particular cell, Ecell is measured to be +0.038v when the pH in both half-cells is 4.00 and [Cl2] = 0.20 M, [HClO] = 0.10 M. What is [MnO4-1] in the solution?

Write unbalanced half-reactions for the following net ionic equations. Part A MnO4−(aq)+IO3−(aq)→MnO2(s)+IO4−(aq) Express your answers as...

Write unbalanced half-reactions for the following net ionic equations. Part A MnO4−(aq)+IO3−(aq)→MnO2(s)+IO4−(aq) Express your answers as chemical expressions separated by a comma. Enter the reduction half-reaction first. Identify all of the phases in your answer. Part B NO3−(aq)+SO2(aq)→SO42−(aq)+NO2(g) Express your answers as chemical expressions separated by a comma. Enter the reduction half-reaction first. Identify all of the phases in your answer.

Consider a glass electrode or [pH electrode (combination electrode). a. Identify the reference part. b. Identify...

Consider a glass electrode or [pH electrode (combination electrode). a. Identify the reference part. b. Identify the indicator part. c. Explain how the potential of the electrode is determined. d. Describe a two-point calibration of the electrode. e. State any five of the eight possible errors that might occur in pH measurements with the electrode.

Balance the following redox equation in basic conditions: Ag(s) + MnO4⁻(aq) ⟶ MnO2(s) + Ag+(aq) What...

Balance the following redox equation in basic conditions: Ag(s) + MnO4⁻(aq) ⟶ MnO2(s) + Ag+(aq) What is the stochiometric coefficient for H2O in the balanced equation?

Consider the following reactions. reaction MnO4−(aq) + Cl−(aq) → MnO2(s) + ClO3−(aq) in basic solution Balance...

Consider the following reactions. reaction MnO4−(aq) + Cl−(aq) → MnO2(s) + ClO3−(aq) in basic solution Balance each equation under the specified conditions

Write balanced net ionic equations for the following reactions in acidic solution: Part A MnO−4(aq)+IO−3(aq)⟶MnO2(s)+IO−4(aq) Express...

Write balanced net ionic equations for the following reactions in acidic solution: Part A MnO−4(aq)+IO−3(aq)⟶MnO2(s)+IO−4(aq) Express your answer as a balanced net ionic equation. Identify all of the phases in your answer. Part B Cu(OH)2(s)+N2H4(aq)⟶Cu(s)+N2(g) Express your answer as a balanced net ionic equation. Identify all of the phases in your answer. Part C Fe(OH)2(s)+CrO2−4(aq)⟶Fe(OH)3(s)+Cr(OH)−4(aq) Express your answer as a balanced net ionic equation. Identify all of the phases in your answer. Part D H2O2(aq)+ClO−4(aq)⟶ClO−2(aq)+O2(g) Express your answer as a...

Balance the following redox reaction occurring in basic solution. I−(aq)+MnO−4(aq)→I2(aq)+MnO2(s)

Calculate E∘cell for each of the following balanced redox reactions. Are the reactions spontanous? A) 2Cu(s)+Mn2+(aq)→2Cu+(aq)+Mn(s)...

Calculate E∘cell for each of the following balanced redox reactions. Are the reactions spontanous? A) 2Cu(s)+Mn2+(aq)→2Cu+(aq)+Mn(s) B) MnO2(s)+4H+(aq)+Zn(s)→Mn2+(aq)+2H2O(l)+Zn2+(aq) C) Cl2(g)+2F−(aq)→F2(g)+2Cl−(aq)

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