3. For a 0.005 M aqueous solution of SrCl2 at 298 K, the conductivity is 1.242 x 103 S cm-1. What is the molar conductivity of this solution? [248.4]
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- The resistance of a conductivity cell containing a 0.02 M aqueous solution of KCl was fond to be 83 ohms at 298 K. The conductivity of the 0.02 M KCl solution at this temperature is 0.00277 S cm-1. When the cell was filled with a 0.005 M aqueous solution of K2SO4, it exhibited a resistance of 326 ohms at the same temperature. What is the molar conductivity of the potassium sulfate solution? [ answer should be 141 S cm2 mol-1]thank uA 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!In electrochemistry, specific conductance is defined as (1000/N)* k, where N is the normality of the salt solution and k is the specific conductance. Current is carried by both anions and cations to a different degree. Thus, the equivalence of a salt is the sum of the ionic conductances of the cation and anion. If the ionic conductance of Na+ is 50.1 and that of Cl- is 76.6. What is the estimated concentration of NaCl in mg/L. The specific conductance of NaCl is 125x106. A) 49 B) 58 C) 29 D) 38 Note: This is not a graded question. This question is from my reviewer.
- A 0.2653 g of pure potassium dichromate was dissolved in 15 mL of 1.5 M sulfuric acid and transferred to a 250.0 mL volumetric flask and diluted to the mark with distilled water. A 25.0 mL aliquot of this solution was transferred to another 250.0 mL volumetric flask and diluted to the mark with distilled water and this solution has an absorbance 0f 0.387 in a 2.00 cm cell. Calculate the molar absorptivity of potassium dichromate.The E°cell = 0.135 V for the reaction3I2(s) + 5Cr2O72-(aq) + 34H+(aq) → 6IO3-(aq) + 10Cr3+(aq) + 17H2OWhat is Ecell if [Cr2O72-] = 0.014 M, [H+] = 0.21 M, [IO3-] = 0.00018 M, and [Cr3+] = 0.0039 M?Ecell =The electrolytic conductivity of NaCl solution at 18oC is 0.0124 ohm-1cm2 mol-1 and the resistance of the cell containing the solution at the same temperature is 50 ohm. The cell constant will be a. 0.62 b. 0.31 c. 0.124 d. 0.000248
- Calculate the G in kJ for the following cell: Al(s)|Al3+(0.0035M)||Fe3+(0.55M)|Fe(s) Eocell=+1.59 V Al(s)|Al3+(0.0035M)||Fe3+(0.55M)|Fe(s) Group of answer choices -473 -374 -158 -734 -658 Calculate Ecell in volts. Cu(s)|Cu2+(3.00x10-4)||Ag+(0.15M)|Zn(s) Eocell=+0.620 V 0.700 0.544 0.944 0.644 0.800In an unknown sample, the amount of ascorbic acid (C6H8O6) is determined using coulometry. Analysis of a 250.0 mg sample gives an endpoint with starch after reaction with electrogenerated iodine in 384 sec using a current of 30.0 mA. A) What specific type of coulometric method is used? B) What is the % ascorbic acid, (C6H8O6), (FW= 176.12 g/mol) in the sample?ELECTROCHEMISTRY: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous solution containing M2X1 (where X is the anion) with a supplied current of 5.54 A for 11 h, consuming 0.1826 kWh of electrical energy. Assume that the current efficiency is 85%. (Input values only with 2 decimal places. Do not include the unit.)
- 4.In a certain conductivity cell, the resistance of a 0.01 M KCl solution is 150 Ω. Theknown molar conductivity of the solution is 141.27 Ω-1 cm2 mol-1. Calculate the cell constant (Kcell).*(Kcell unit is cm-1) 5. Using the same conductance cell as in Question No. 4, a student measured the resistanceof a 0.10 M NaCl solution to be 19.9Ω. Calculate the experimental value of the molarconductivity of this solution.A piece of an unknown weighing 12.50is placed in 49.7cm of water in a cylinder. The water level increases to 69.0cm3. whats the calculated value for the drnsity of the solid in g ml-1Calculate 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.