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- A 0.2g sample of toothpaste containing fluoride was treated with 50 cm3 of a suitable buffer solution and diluted to 100 cm3. Using a fluoride ion-selective electrode, a 25.00 cm3 aliquot of this solution gave cell potentials of –155.3 mV before and –176.2 mV after spiking with 0.1 cm3 of a 0.5 mg/cm3 fluoride standard. Calculate the pF– corresponding to each cell potential and the percentage by weight of fluoride in the toothpaste.The standard potentials of Pb2+|Pb and Sn2+|Sn are −126 mV and −136 mV respectively at 25 °C, and the overpotential for their deposition are close to zero. What should the relative concentrations of Pb2+(aq) and Sn2+(aq) be in order to ensure simultaneous deposition from a mixture? You may assume that activities can be approximated by molar concentrations.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.
- Given that ΔrG⦵ = −212.7 kJ mol−1 for the reaction Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) in the Daniell cell at 25 °C, and b (CuSO4) = 1.00 × 10−3 mol kg−1 and b (ZnSO4) = 3.00 × 10−3 mol kg−1, calculate (a) the ionic strengths of the solutions, (b) the mean ionic activity coefficients in the compartments, (c) the reaction quotient, (d) the standard cell potential, and (e) the cell potential. (Take γ+ = γ− = γ± in the respective compartments. Use the Debye–Hückel limiting law.)Create a calibration curve. Electrode potential (mV) vs. log [Ca2+]. (complete with, the equations of the best fit line, and the correlation coefficient) log[Ca 2+] Electrode potential (mV) -5 -105.4 -105.1 -106.5 -6 -120.9 -120.3 -120.6 -4.4 -96.6 -97.2 -96.5 -4 -85.5 -85.8 -85.2 -3 -56.6 -56.2 -56.4 -2 -26.6 -27.1 -27.1What Range of cathode potentials versus the saturated calomel electrode can be used to quantitatively separate Ag+ and Ni2+ by electrolytic deposition? Assume that the sample solution is initially 0.1000M in each ion and the quantitative removal of an ion is realized when only 1 part in 10000 remains undeposited. ESCE = 0.244V E0Red (Ag+) = 0.8V E0Oxid (Ni) = -0.25V
- Use the shorthand notation to describe a cell consisting of a saturated calomel reference electrode and a silver indicator electrode for the measurement of (a) pSCN. (b) pI. (c) pSO3 (d) pPO. Then, generate an equation that relates pAnion to Ecell for each of the cells. (For Ag2SO3 Ksp = 1.5 * 10-14; for Ag3PO4, K,p = 1.3 *10-20 ).When the difference in pH across the membrane of a glass electrode at 25C is 4.63 pH units, how much voltage is generated by the pH gradient? Assume that the constant in Equation 15-6 is 1.00.Is a quantitative separation of Zn2+ and Ag+ by electrolytic deposition feasible in principle? If so what range of cathode potential versus that saturated calomel electrode can be used? Assume that the solution is initially 0.1000M in each ion and that quantitative removal of an ion is realized when only 1 part in 1000 remains undeposited E0reduction of Zn2+ = -0.76V E0oxidation of Ag = -0.8V
- An ion selective electrode is utilised to determine the concentration of Ca2+ in the presence of Mg2+. The selectivity coefficient for the electrode kij is 0.015. If the concentrations of Ca2+ and Mg2+ are 50 and 500 ppm, respectively, calculate the change in potential (in mV) when the temperature of the measurement cell is increased from 20oC to 40oC.Significant evolution or deposition occurs in electrolysis only if the overpotential exceeds about 0.6 V. To illustrate this criterion calculate the effect that increasing the overpotential from 0.40 V to 0.60 V has on the current density in the electrolysis of 1.0 m NaOH(aq), which is 1.0 mA cm−2 at 0.4 V and 25 °C. Take α = 0.5. Hint: Assume that the current is entirely anodic.why the reference electrode can serve as a probe to measure relativereduction potentials or even detect a change in pH of solution