Pushing Electrons
4th Edition
ISBN: 9781133951889
Author: Weeks, Daniel P.
Publisher: Cengage Learning
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The cobalt mu-hydroxide complex cobaltate(III) of potassium is a dinuclear complex. Correct?
The cobalt mi-hydroxide complex cobaltate(III) of potassium is a dinuclear complex. Correct?
3. Arrange the different acids in Exercise B # 2 from the strongest (1) to the weakest acid
(10).
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(strongest)
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- Name Section Score Date EXERCISE B pH, pOH, pка, AND PKD CALCULATIONS 1. Complete the following table. Solution [H+] [OH-] PH РОН Nature of Solution A 2 x 10-8 M B 1 x 10-7 M C D 12.3 6.8 2. The following table contains the names, formulas, ka or pka for some common acids. Fill in the blanks in the table. (17 Points) Acid Name Formula Dissociation reaction Ka pka Phosphoric acid H₂PO₁ H3PO4 H++ H₂PO 7.08 x 10-3 Dihydrogen H₂PO H₂PO H+ HPO 6.31 x 10-6 phosphate Hydrogen HPO₁ 12.4 phosphate Carbonic acid H2CO3 Hydrogen HCO 6.35 10.3 carbonate or bicarbonate Acetic acid CH,COOH 4.76 Lactic acid CH₂CHOH- COOH 1.38 x 10 Ammonium NH 5.63 x 10-10 Phenol CH₂OH 1 x 10-10 Protonated form CH3NH3* 3.16 x 10-11 of methylaminearrow_forwardIndicate whether it is true that Co(III) complexes are very stable.arrow_forwardMnO2 acts as an oxidant in the chlorine synthesis reaction.arrow_forward
- In Potassium mu-dihydroxydicobaltate (III) tetraoxalate K4[Co2(C2O4)4(OH)2], indicate whether the OH ligand type is bidentate.arrow_forwardImagine an electrochemical cell based on these two half reactions with electrolyte concentrations as given below: Oxidation: Pb(s) → Pb2+(aq, 0.10 M) + 2 e– Reduction: MnO4–(aq, 1.50 M) + 4 H+(aq, 2.0 M) + 3 e– → MnO2(s) + 2 H2O(l) Calculate Ecell (assuming temperature is standard 25 °C).arrow_forward: ☐ + Draw the Fischer projection of the most common naturally-occurring form of aspartate, with the acid group at the top and the side chain at the bottom. Important: be sure your structure shows the molecule as it would exist at physiological pH. Click and drag to start drawing a structure. ✓arrow_forward
- For a silver-silver chloride electrode, the following potentials are observed: E°cell = 0.222 V and E(saturated KCl) = 0.197 V Use this information to find the [Cl–] (technically it’s the activity of Cl– that’s relevant here, but we’ll just call it “concentration” for simplicity) in saturated KCl.arrow_forwardA concentration cell consists of two Sn/Sn2+ half-cells. The cell has a potential of 0.10 V at 25 °C. What is the ratio of [Sn2+] (i.e., [Sn2+left-half] / [Sn2+right-half])?arrow_forwardElectrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. What is Κ for the following balanced reaction if E˚ = +0.0218 V? 3 Zn(s) + 2 Cr3+(aq) → 3 Zn2+(aq) + Cr(s) E˚ = +0.0218 Varrow_forward
- Consider the following half-reactions: Hg2+(aq) + 2e– → Hg(l) E°red = +0.854 V Cu2+(aq) + 2e– → Cu(s)E°red = +0.337 V Ni2+(aq) + 2e– → Ni(s) E°red = -0.250 V Fe2+(aq) + 2e– → Fe(s) E°red = -0.440 V Zn2+(aq) + 2e– → Zn(s) E°red = -0.763 V What is the best oxidizing agent shown above (i.e., the substance that is most likely to be reduced)?arrow_forwardCalculate the equilibrium constant, K, for MnO2(s) + 4 H+(aq) + Zn(s) → Mn2+(aq) + 2 H2O(l) + Zn2+(aq)arrow_forwardIn the drawing area below, draw the condensed structures of formic acid and ethyl formate. You can draw the two molecules in any arrangement you like, so long as they don't touch. Click anywhere to draw the first atom of your structure. A C narrow_forward
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