otentiometry 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
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Chemistry
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 potential
Step by step
Solved in 2 steps
- a) 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 solution is 0.20 M MgSO4 and 0.70 M NaCl. Solid Na2SO4 is added to the solution so that the total ionic strength of the solution is 3.3. What is the Na2SO4 concentration of the solution then. The change in solution volume is not taken into account when adding reagents.(3) Calculate the solubility (K) of CO₂ in seawater using the AG values given below for each, and the relation between AGr and K H₂CO3(aq) -623.2 AGf CO₂ (g) + H₂O → -394.37 -237.18
- How do you choose the most suitable precipitate for gravimetric purposes if given many choices?4. The molar absorptivities of the indicator weak acid HIn (K₁ = 1.42 x 105) and its conjugate base In at 570 were determined as ε(HIn) = 7120 and ɛ(In) = 961. The optical length b = 1.00 cm. (a) What is the absorbance of an unbuffered indicator solution having total indicator concentration 8.0 × 10%. (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 x 105 and pH = 6.5.An alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled at 15 deg C, treated with 2 drops of phenolphthalein indicator and titrated with 1.058 N H2SO4 requiring 6.8 mL to render the solution colorless. Upon adding 2 drops of methyl orange and continuing the titration 16.5 mL more of the acid was needed to complete analysis. What is the quantitative composition of the sample?
- Calculate the activity coefficient, Y. of Ni2+ when the ionic strength of the solution, u, is 0.085 M by linear interpolation Ionic Activity strength coefficient of the data in the table. (H, M) 0.001 0.870 0.005 0.749 YN? 0.01 0.675 0.05 0.485 0.1 0.405 Calculate the activity coefficient, y, of Ni2+ when the ionic strength of the solution, u, is 0.085 M by using the extended Debye-Hückel equation at 25 °C, where the ion size is 600 pm. YN =.Water sample from different river water was subjected to a qualitative alkaline analysis by titrating against 0.1250 MHC1 and using phenolphthalein and bromocresol green end point. The table below shows the volumes of acid needed to titrate 25.00-mL portions of each sample and their corresponding end point, separately. Use this information to deduce the composition of the solutions. Calculate the molar concentration of each solute. Volume (mL) Phenolphthalein end Bromocresol green Solute identity concentration end point Volume (mL) Molar Sample point 22.40 of solute/s 1 22.41 2 0.00 33.40 3 15.67 42.13 4 29.64 36.42(b) In the pH metric titration, calomel and glass electrodes are used for measuring. What are the other electrodes that can be used for measuring the pH of a solution? Explain the advantages and disadvantages along with the full cell diagram. (c) To study the kinetics of iodination of acetone, why starch is used as an indicator just before the endpoint? What will happen if starch is used as an indicator at the beginning of the titration?
- Consider the titration of 25.0 mL of 0.010 0 M Sn21 by 0.050 0 M Tl31 in 1 M HCl, using Pt and saturated calomel electrodes. (a) Write a balanced titration reaction. (b) Write two half-reactions for the indicator electrode. (c) Write two Nernst equations for the cell voltage. (d) Calculate E at the following volumes of Tl31: 1.00, 2.50, 4.90, 5.00, 5.10, and 10.0 mL. Sketch the titration curve.A 40.00-mL aliquot of 0.05000 M HNO2 is diluted to 75.00 mL and titrated with 0.0800 M Ce4+. The pH of the solution is maintained at 1.00 throughout the titration; the formal potential of the cerium system is 1.44 V. Calculate the potential of the indicator electrode with respect to a saturated calomel reference electrode after the addition of 5.00, 10.00, 15.00, 25.00, 40.00, 49.00, 49.50, 49.60, 49.70, 49.80, 49.90, 49.95, 49.99, 50.00, 50.01, 50.05, 50.10, 50.20, 50.30, 50.40, 50.50, 51.00, 60.00, 75.00, and 90.00 mL of cerium(IV). Generate a titration curve for these data. Upload your excel file showing the titration curve and manual computations. Upload Choose a fileHow many grams of oxalic acid (A), potassium oxalate (B), and dipotassium oxalate (C) will need to be added to 1 L of water to obtain a solution with a pH of 4.7 and a total solute concentration of 50 mM? The volume of 1 L will remain constant during the procedure.