sure Experiment 13: Electrical Conductivity B. Testing the conductivity of reactions 0.1M KNO3 and 0.1M Na2CO3 a. Substance Observation No, few, or many Species Present Strong, weak or nonelectrolyte ions? KNO3 strong Na, C0 strong Strong light ions Kt, NOs many Na2CO3 strong strong ?] Balaneed equation: 2 KNOacag)+ Nazl0 K2003la6) +2 NaNDzrag) strong light many Na, lc KNO; + Na2CO3 27 Balanced equation: 2 KNO3(09)+ Na2C02 > K2 +2 NaNOzrag Total ionic equation: 2ktan+2N03+ 2Nat + l0, Net ionic equation: tlls + 2Ala 21 No Net lonic No Reaction b. 0,1M HCH:Q2 and 0.1M NH QH

sure Experiment 13: Electrical Conductivity B. Testing the conductivity of reactions 0.1M KNO3 and 0.1M Na2CO3 a. Substance Observation No, few, or many Species Present Strong, weak or nonelectrolyte ions? KNO3 strong Na, C0 strong Strong light ions Kt, NOs many Na2CO3 strong strong ?] Balaneed equation: 2 KNOacag)+ Nazl0 K2003la6) +2 NaNDzrag) strong light many Na, lc KNO; + Na2CO3 27 Balanced equation: 2 KNO3(09)+ Na2C02 > K2 +2 NaNOzrag Total ionic equation: 2ktan+2N03+ 2Nat + l0, Net ionic equation: tlls + 2Ala 21 No Net lonic No Reaction b. 0,1M HCH:Q2 and 0.1M NH QH

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter11: Dynamic Electrochemistry

Section: Chapter Questions

Problem 10P

See similar textbooks

Similar questions

In an experiment to check chemical balance, measurements of electrical conductivity (κ) were made of acid solutions in different concentrations, as shown in the table below. From these data, show that the acetic acid dissociation equilibrium constant is really a constant, that is, it has the same value for any acetic acid solution at a given temperature. The data were collected at 25 oC. The limit molar conductance of the acetic acid solution is Λ0 = 390.71 Ω^-1*cm^2 / mol. Suggestion: calculate the molar conductance (Λm = 1000 κ / c) for each concentration and then use Ostwald's Dilution Law Molarity c (mol / L) Conductivity κ (Ω^-1*cm^-1) 0.010 1.5590 x 10^-4 0.05 3.5939 x 10^-4 0.1 5.0610 x 10^-4 ANSWER: values close to 1.7 x 10^-5 I need the calculations to show how to obtain this value
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-1
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.
Calculate the molarity of the nickel solution. From the following data calculate the normalities of the acid and base solutions: weight of pure Na2CO3 = 0.2448 g; volume of acid = 43.65 mL ; volume of base used in back titration = %3D 0.84 mL ; 1.000 mL of base = 0.982 mL of acid. Reaction: CO, + 2H* → H2CO3
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 u
Allowable recovery from limiting salt calculations Determine the limiting sait and allowable recovery for a brackish water RO system containing the following solutes: calcium 74 mg/L. barium 0.008 mg/L. and sulfate 68 mg/L. Assume 100 percent rejection of all solutes and & polarization factor of 1.15 and ignore activity coeficients (i.e., activity = concentration).
(a) How many coulombs are required to reduce 1 mole Cr2O72- to Cr3+?(b) The conductivity of 0.001 M acetic acid is 4 × 10-5 S/m. Calculate the dissociation constant of acetic acid if [latex]\Lambda_{\mathrm{m}}^{0}[/latex],for acetic acid is 390 S cm2 mol-1.
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.
6. a. Explain the relationship between molar conductivity and ion mobility (both theoretical and existing formulations) b. Explain the relationship between the reaction rate and the size of the ions in a solution (both theoretically and according to the existing formula)
Chemistry The resistance of a saturated solution of PbSO4 (very insoluble salt) at 291K is of 1.7x106 Ω, being the resistivity of pure water 7.1x105 Ωcm. 1. Determine the solubility product of PbSO4 at 291K knowing that Λmº (SO4-2)=136 Ω-1cm2mol-1 and Λmº (Pb+2)=122 Ω-1cm2mol-1 . 2. How many centimeters will the ion move Pb+2 in one second when applying a potential difference of 25V between two electrodes 1 cm apart? Solution: Kso=1.41·10-11
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.
The measurement of pH using a glass electrode obeys the Nernst equation. The typical response of a pH meter at 25 00C is given by the equation where contains the potential of the reference electrode and all other potentials that arise in the cell that are not related to the hydrogen ion concentration. Assume that = 0.250 V and that a. What is the uncertainty in the values of pH and [H+] if the uncertainty in the measured potential is 1 m V ( 0.001 V)? b. To what precision must the potential be measured for the uncertainty in pH to be 0.02 pH unit?