A conductivity cell filled with 0.1 M KCI at 25°C has a measured resistance of 24.36 2. The conductivity of KCI at this concentration is = 116.39 cm²/2-mol. When the cell was filled with 0.01 M acetic acid, the cell resistance was found to be 1982 at 25°C. Calculate the molar conductance of the acetic acid in 2-¹ cm² mol-¹.
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- 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!(c) 0.04 molar solution of NaCl is filled in a conductance cell at 25°C that showed a resistance of 175 ohms. The specific conductance of the NaCl solution used is 2.77 x 102 mho cm. The same cell containing 0.02 molar KCl solution gave an electrical resistance of 424 ohms. What will be the specific and equivalent conductance of the KCI solution?At 25 °C, 0.05 M of MgCl2 electrolyte solution showed molar conductivity of 194.2 S cm? mol-. A cell with electrodes that 1.50 cm² in surface area and 0.50 cm apart is filled with the above electrolyte. Determine the resistance of the solution.
- 116.In a conductivity cell of a cell constant 0.003 cm³¹ concentration of 0.01 M solution of acetic acid, the resistance against ionic mobility is 20 ohm at 25 °C. the degree of dissociation of the acid is (where the molar conductance at infinite dilution = 390 x 104 2¹¹ m² mol¹ at 25° C) a) 0.015 b) 0.027 c) 0.038 d) 0.047The conductivity of a 0.0312 M solution of a weak base is 1.53 x 104 Scm'. If the sum of the limiting ionic conductances for BH* and OH-' is 237.0 Scm²mol·' what is the value of the base constant K6? 4.5 x 10s mol.dm (i) 2.3 x 103 mol.dm (iii) 2.89 x 10 mol.dm3 (ii) 1.37 x 10-5 mol.dm3 (iv) (v) 4.78 x 103 mol.dm3The described electrochemical cell (concentration cell) was set up: Cu|CuSO4 (c1) // CuSO4 (c2)|Cu Determine which electrode is the positive terminal (+) of the cell and calculate the cell potential E (electromotive force, EMF) for the given concentrations of the electrolyte CuSO4 in the cell (25oC): c1 = 0.01 mol dm-3, c2 = 1×10-4 mol dm-3
- At 25°C, a cell filled with 0.01 demal KCI solution gave a resistance of 484.02. The following data for NaCl solutions were then taken in the same cell at 25°C: Normality 0.0005 0.0010 0.0020 0.0050 Resistance ( SI) 10910 5494 2772 1129 Evaluate the equivalent conductance (in cm² 2-¹ mol-¹) of NaCl at the limit of infinite dilution. The specific conductance of a 0.01 demal KCI solution is 0.00140877 $2¹cm-¹. Express your answer in four significant figures.A solution containing 0.402 49 g of CoCl2 ? xH2O (a solid with an unknown number of waters of hydration) was exhaustively electrolyzed to deposit 0.099 37 g of metallic cobalt on a platinum cathode by the reaction Co21 1 2e2¡Co1s2. Calculate the number of moles of water per mole of cobalt in thereagent. A good approach is to find moles of Co, moles of CoCl2, mass of CoCl2, and, by difference, mass of H2O in the sample.Please assist with the following sub questions of question 1. a) The conductivity of a 0.05M solution of acetic acid at 18⁰C is 4.4×10-4 (ohms)-1cm-1. Limiting molar conductivity of acetic acid at the same temperature is 387 (Ohms)-1cm². Calculate the dissociation constant (Ka) of acetic acid? b) The resistivity of aluminum is 2.824×10-8 ohms.m. Calculate the potential drop across a piece of aluminum wire that is 2.0 mm in diameter and 1.00 m long. Assume current is 1.25 A. C) Calculate the conductance and conductivity of a metal if the resistivity of the metal is 2.824×10-8 ohms.m, with resistance of 9.0×10-3 ohms when current is 1.25 A.
- 12. The described electrochemical cell (concentration cell) was set up:Cu | CuSO4 (c1) || CuSO4 (c2) | CuFrom the previous cell reaction:Determine which electrode is the positive terminal (+) of the cell and calculate the cell potential E (electromotive force, EMF) for the given concentrations of the electrolyte CuSO4 in the cell (25C):b) c1 = 1×10-4 mol dm-3, c2 = 0.01 mol dm-3 EMF=0.2808 V, left hand cathode EMF=-0.2808 V, right hand cathode EMF=-0.0592 V, left hand cathode EMF 0.0592 V, right hand cathodeA solution containing 25.0 mL of H2C2O4 required 13.78 mL of 0.04162 N KMnO4 for titration forming Mn2+ and CO2 as products. Calculate the normality and molarity of the H2C2O4..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?