Calculate the potential of the copper electrode immersed in a 0.0750 M NaCl solution saturated with CuCl2 (EOCU + / Cu = 0.521 V; Kç CuC12 = 1.9 x 10-7)
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- The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.Calculate the potential of an alloy (Ni) electrode immersed in Ni(OH)2, pH = 9.00, Ksp = 6.5 × 10-18An exhausted zeolite softener was regenerated by passing 100 litres, of NaCl. Solution containing 150 gm per lit. of NaCl. How many lit. of a sample of H2O of hardness 300 ppm can be softened by this softener? (Given at wts. for C = 12, O = 16, Na = 23, CI = 35.5, Ca = 40).
- Explain why ionic attractions are weaker in media with high dielectric constants, e. g.,water and aqueous buffers.A conductivity cell filled with a 0.01 M KCl solution was found to have a resistance of 189 ohms at 25oC. When filled with 0.01 M HCl solution, the cell gave a resistance of 64.8 ohms at the same temperature. At 25oC, the conductivity of 0.01 M KCl solution was 1.4088 x 10-3 S cm-1. Calculate (a) the cell constant and (b) the conductivity of the HCl solution. answer is [0.266; 4.105 x 10-3] please explain. thank you!By employing a given conductivity cell with 0.1N potassium chloride at 18pC, an observed conductance of 0.025 mho was obtained. What is the cell constant if the specific conductance of KCL at 18°C is 0.0112 mho.
- In a polarographic experiment of a 60 mL of 0.08 M Cu2+solution, a limitingcurrent was left on for 15 minutes. If the average current during the time of theexperiment is 6.0 μA, what fraction of the copper is removed from the solution? TheFaraday constant is 96485 C/mol of electron.Calculate the potential of a platinum electrode immersed in a solution that is (a) 0.0613 M in K4Fe(CN)6 and 0.00669 M inK3Fe(CN)6. E0=0.36 (b) 0.0400 M in FeSO4 and 0.00915 M in Fe2(SO4)3. E0=0.771 (c) buffered to a pH of 5.55 and saturated with H2 at 1.00 atm. (d) 0.1015 M in V(OH)4+, 0.0799 M in VO2+, and 0.0800 M in HClO4. E0=1 (e) prepared by mixing 50.00 mL of 0.0607 M Ce(SO4)2 with an equal volume of 0.100 M FeCl2 (assume solutions were 1.00 M in H2SO4 and use formal potentials).E0=0.68 (f ) prepared by mixing 25.00 mL of 0.0832 M V2(SO4)3 with 50.00 mL of 0.00628 M V(OH)4+ and has a pH of 1.00.The following cell was found to have a potential of 0.2897 V:SCEIIMg2+(a = 3.32 * 10^-3M)membrane electrode for Mg^2+(a) When the solution of known magnesium activity was replaced with an unknown solution, the potentialwas found to be 0.2041 V. What was the pMg of this unknown solution?(b) Assuming an uncertainty of 60.002 V in the junction potential, what is the range of Mg21 activitieswithin which the true value might be expected?(c) What is the relative error in [Mg^2+] associated with the uncertainty in Ej?
- 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.Given: You weigh out exactly 0.200 g of Fe(NH4)2(SO4)2·6H2O and dissolve it in the 100.00 mL volumetric flask. You then pipette 2.00 mL of this solution into the 50.00 mL volumetric flask to prepare the stock standard tris-bipyridyl-iron(II) solution. a. Calculate the molar concentration of iron(II) in this solution in the 50.00 mL volumetric flask. (The MW of Fe(NH4)2(SO4)2·6H2O is 392.14 g/mol) (answer a given the information above)A 0.075 M solution of [Co (C2O4) 3] -3 it has an absorbance of 1.1 at 660 nm in a 1 cm cell. Calculate: a) The molar absorptivity coefficient, b) The value of I / I0, c) The absorbance for a 0.035 M solution in the same cell.