List several sources of uncertainty in pH measurements with a glass/calomel electrode system. (Select all that apply.) O the error that arises when the ionic strength of the calibration standards differs from that of the analyte solution OHg(OH)2 precipitation from the calomel in basic solutions O the hydrogen bonding error in polar solutions O dehydration of the working surface O the alkaline error in strongly basic solutions O the pH of the standard buffers 0 non-reproducible junction potentials with solutions of low ionic strength O the acid error in highly acidic solutions

List several sources of uncertainty in pH measurements with a glass/calomel electrode system. (Select all that apply.) O the error that arises when the ionic strength of the calibration standards differs from that of the analyte solution OHg(OH)2 precipitation from the calomel in basic solutions O the hydrogen bonding error in polar solutions O dehydration of the working surface O the alkaline error in strongly basic solutions O the pH of the standard buffers 0 non-reproducible junction potentials with solutions of low ionic strength O the acid error in highly acidic solutions

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

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 -27.1
Marked out of 3.00 Choose the best answer Ecell for Pt|H2 (p-1 atm)lH*(m)||Cl|H92C2IH9|Pt is 0.398 V at 1.0 atm and 306.4 K. Eo for the normal calomel electrode is 0.28V. Calculate the pH of solution (without activity) a. 3.88087 b. 1.94096 C. -1.63185 d. 2.02350 e. 0.95627
lons that react with Ag like SCN can be determined electrogravimetrically by deposition on a silver working anode: (c) Ag(s) + SCN AGSCN(s) + e A silver anode with initial mass of 12.4730 g was used to electrolyse 85.00 mL of a solution of 0.0245 M KSCN. At the end of the experiment, the anode weighed 12.5767 g. How long did the experiment take, if a current of 100 mA was used?
5
2
Answer the ecell value only
The potentiometric titration data of 2,422 mmol chloride ion with 0.1000 M AgNO3 are as follows. What should the x and y axis values be to find the turning point using the first derivative curve? AgNO3 volume (mL) Potential (Volts) 5.0 0.062 15.0 0.085 20.0 0.107 22.0 0.123 23.0 0.138 23.50 0.146 23.80 0.161 24.00 0.174 24.10 0.183 24.20 0.194 24.30 0.233
General Chemistry (Quesion -8) =====================
Calculate the H* from the following data obtained by the moving boundary method using cadmium chloride as the indicator electrolyte: • Concentration of HCI = 0.100 M • Movement of boundary = 7.50 cm %3D Cross -section Area = 1.24 cm2 Current =2 A • Time • Molar conductivity of solution 350.6 S cm2 mol = 90 s !3! 389.6 S cm² mol- B. 174.8 S cm2 mol-1 180.8 S cm? mol-1 150. A S cm 2 mol-
A 50.00 ml. sample of phenol cleaning solution was analyzed by reaction of phenol with Brg 0 The Bry ) was produced by anodic oxidation of Br by application of a 88.934 mA constant current for 10o.36 minutes. Express your answer in mng phenol/ml. sample. Report your answer to 3 sig figs OH OH Br + 3H + 3Br Br 3Br, + Br
A solution prepared by mixing 60.0 mL of 0.360 M AGNO, and 60.0 mL of 0.360 M TINO, was titrated with 0.720 M NaBr in a cell containing a silver indicator electrode and a reference electrode with a constant potential of 0.175 V. The reference electrode is attached to the positive terminal of the potentiometer, and the silver electrode is attached to the negative terminal. The solubility constant of TIBr is Kp = 3.6 × 10-6 and the solubility constant of AgBr is = 5.0 x 10-13. Ksp Which precipitate forms first? O TIBI O AgBr Which of the expressions shows how the cell potential, E, depends on [Ag*]? E = 0.175 V – [0.799 V – 0.05916log ([Ag+])] 1 E = |0.799 V – 0.05916log - 0.175 V [Ag*) E = [0.799 V – 0.05916log ([Ag*]D] – 0.175 V E = 0.175 V - |0.799 V – 0.05916log [Ag* * (ল) Calculate the first and second equivalence points of the titration. first equivalence point: mL second equivalence point: mL What is the cell potential after each of the given volumes of 0.720 M NaBr have been…
b Calculate PSCN if a cell consisting of a saturated calomel reference electrode ( E = 0.244 V) and a silver indicator electrode has a potential of 0.131 V ( E %3D Ag"/Ag = 0.799 V, ESCN/Ag = 0.091 V, Kp(A9SCN) = 1.1 x 10-12). PSCN = %3D