4. In lake water at a pH of 5 and a redox potential of +0.30 volt, what concentration of Cu could exist in contact with metallic copper? 5. What redox potential must 2+ ond
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- Gases in a Salt Marsh: You measure appreciable CH 4(g) andCO 2(g) partial pressures in the sediment pore fluid and you want toknow if there is equilibrium between these redox couples. The measuredpartial pressure of CO 2 (g) is 1x10 -5 atm and the measured partialpressure of CH 4 (g) is 5x10 -3 atm in the pore fluid.You measure a redox potential (E h) of pore-fluid water of Eh = -0.1 V atpH=8.3 using a platinum electrode and suitable reference electrode. Calculate a value of E h from the ratio of the measured gas partialpressuresIron in an NaCl solution, pH=1, shows a potential of +0.2 volts vs. SHE. What are the possible anodic and cathodic reactions, assuming that the Pourbaix diagram of Figure 2.4 is applicable? 2-8. A student suggests that two possible reactions for Problem 2.7 are Cl2 + 2e = 2CI and Na = Na* + e". = Do you agree with either or both? If so, what assumptions must you make?a) Define the term pH. Which electrode do you use? Draw a scheme and describe theprinciple of pH measurement. Express the limitations of the electrode used.b) To discuss following each titration of a solution with a strong base and draw each titrationcurvesi) 0.1 M H2SO4 (first acidty is very strong, K2= 1.2 10-2
- At 25C, you conduct a titration of 20.00 mL of a 0.0400 M AgNO3 solution with a 0.050 M NaI solution within the following cell: Saturated Calomel Electrode | Titration solution | Ag(s) for the cell as writted, what is the voltage after the addition of 10.00 mL of the NaI sooution? The reduction potential for the saturated calomel electrode is E=0.241 V. The standard reduction potential for the reaction: Ag++e- ® Ag(s) E0= 0.79993V. The solubility constant of AgI is Ksp=8.3x10-17 Note: the cell potential could be negative since the condditions are non-standard ones. a)0.169 b)0.354 c)0.235 d)2.360 e)0.441When a fluoride selective electrode was immersed in a solution that is 1.0 x 10-4 M in F-, the potential that developed (versus SCE) was 41.5 mV. What will be the potential that will develop if the same electrode is immersed in a solution that is 5.0 x 10-5 M in fluoride? -51 mV -47 mV -59 mV -32 mVA potentiometric titration was done using a solution containing 200 mL of water, 20 mL of 3 M sulfuric acid, 5 mL of concentrated phosphoric acid and 10.00 mL of 0.5964 N K2Cr2O7. The amount of titrant added was 19.24 mL of 0.3355 N Fe2+ solution. [H+] = 1.41 x 10-3 M during the titration. Find the concentrations of all species relevant to the redox chemistry present in solution at this point in the titration.
- true or false 9 __ The equilibrium constant of a redox reaction can be calculated from the standard reduction potentials of involved redox couples at given temperature. __ The charge balance for mixture 0.5 M K2HPO4 + 0.1 M H3PO4 is : [ H +] = [ H2PO4 -] + [ HPO4 2-] + [ PO4 3-] + [ OH-] __ The reduction reaction always occurs at a cathode. __ In EDTA titration, the media pH can impact the conditional formation constant Kf ’ . __ Adding table salt into a sugar solution will result in the increasing activity of coefficient of sugar molecules.A bare silver wire electrode is dipped into a solution 0.05M in KNO3 (supporting electrolyte) and saturated in AgBr (Ksp = 5.0 x 10-13), and connected to the back of an mV/pH meter along with a saturated calomel reference electrode. Calculate the potential of the silver indicator electrode. Calculate the cell potential.6) Chromium can be electroplated from aqueous potassium dichromate, with thereduction shown below. If a current of 6.0A and a voltage of 4.5V are used:Cr2O7+(aq) + 14H+(aq) + 12e- -> 2Cr(s)+7H2Oa) How many hours would it take to completely convert215mL of 1.25M K2Cr2O7 to elemental chromium?b) How many kilowatt-hours of electrical energy arerequired to plate 1.00 g of chromium?
- 1. Convert -0.916 V (on SCE. 1.0 N) to the SHE scale. 2. What is the potential on SHE scale, for an electrode which is at a potential of —0.920 V relative to a Ag/AgCl reference in 0.01 N KC1 at 25° C.A pH meter is calibrated using a pH 4.00 buffer with 174.48 mV, pH 7.00 with 0 mV and pH 10.0 buffer with (-)174.48 mV. Calculate the Molar concentration of a Ba(OH)2 solution with electrode potential of (-)337.19 mV.A pH meter is calibrated using a pH 4.00 buffer with 174.48 mV, pH 7.00 with 0 mV and pH 10.0 buffer with (-)174.48 mV. Calculate the Molar concentration of a HCl solution with electrode potential of 396.31 mV.