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- A pH probe/meter uses the following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution Questions: How will measured pH value be affected vs “real” pH if the temperature of the sample is 30C when pH was measured? How will measured pH value be affected vs “real” pH if HCl in pH electrode, became 0.15M instead of 0.1M? How pH value will be affected vs “real” pH if the glass of the pH electrode is not fully hydrated? Please answer all questions and provide a brief explanationa) Define the term pH. Which electrode do you use? Draw a scheme and describe theprinciple of pH measurement. Express the limitations of the electrode used.b) To discuss following each titration of a solution with a strong base and draw each titrationcurvesi) 0.1 M H2SO4 (first acidty is very strong, K2= 1.2 10-2The pH is essentially a voltmeter and the electrical potential across the glass membrane varies with [H+] of the test solution. Thus the Nernst equation, Eglass = Eoglass + 0.0591 log[H+], is applicable to the pH meter. What does Eoglass represent?
- 1. A pH electrode obeys the equation E= constant - 0.0592 pH. If the electrode potiential (E) is -0.105 V at 0.002500 M [H+], what is the electrode constant? 2. Using the electrode constant calculated abobe, determine the pH of a solution that gives the electrode potiential of -0.450V. Sketch the calibration plot for the pH electrode. Label the axes, electrode constant and the value of the slope on the calibration plot. Answer question 1Chemistry Potentiometry Topic Briefly discuss the following: 1.different types of membrane indicator electrode 2.how a pH glass electrode works 3.errors encountered in the use of pH electrode 4.contribution of other variables in the glass indicator potentialA series of solutions was prepared with pH varying from 1 to 13. Each solution contained 2.0mg/L fluoride and had the same ionic strength and temperature. The response of a fluoride ion selective electrode in each solution was recorded relative to a reference electrode. A graph of Ecell versus pH will curve: A.downwards at pH < 4.0 due to H+ interference B.downwards at pH < 4.0 due to OH- interference C.upwards at pH < 4.0 due to H+ interference D.upwards at pH < 4.0 due to OH- interference
- For indicator electrodes, which statements are true?I Indicator electrodes are made from relatively inert metals.II Indicator electrodes work best when the electrode surface is large and clean.III Platinum is a common indicator electrode.IV Platinum electrodes are more inert than gold electrodes. A. I, III, and IV B. I, II, and III C. I, II, III, and IV D. II and III E. I, II, and IV2.1 Calculate the pH of 1.0 M HC2H3O2 solution, using Ka = 1.7 × 10-5 . Begin this calculation by defining the variable x. List the pH answer as “theoretical pH” on the report sheet. Have the instructor check this answer and all subsequent calculations. To test your prediction, obtain about 35 mL 1.0 M HC2H3O2 and add to a clean, dry 50 mL beaker. Measure the pH of this solution. Be sure the electrode is properly submerged and gives a stable reading. Record the pH reading in the “Observed pH” column on the report sheet. The value should be within ± 0.2 pH units of the calculated value. From the experimental pH and beginning concentrations of the solution components, calculate the remainder of the entries across the table to pKa . Save this solution for Sections 2.3 and 2.6. 2.2 Calculate the pH of 0.10 M HC2H3O2 solution. List this answer as “theoretical pH” on the report sheet. Test your prediction by placing 5 mL of 0.10 M HC2H3O2 in a test tube and testing its…If an Ecell of 0.495V was noted when your cell was set-up. What is thesolution pH?
- Why do both Reference and Indicator electrodes need in Potentiometric titration? answer at your own words ans answer to the point not any irrelevant wordsQ.3.(a)List the types of electrodes used for pH measurement. Explain the construction details of one of them. Why is reference electrode required for pH measurementThe selectivity coefficient of the fluoride ion-selective electrode is kF-,OH- = 0.15. How does the electrode potential of 1.4x10-5 M F- ions at pH 5.5 change to pH 11.0? aF- = [F-] dilute solution is considered.