Solve for the average molarity of sodium thiosulfate titrant if 0.1532 g, 0.1573 g, 0.1551 g KIO3 (MW: 214.001 g/mol) consumed 3.60 mL, 3.56 mL, and 3.45 mL, respectively from three 10 mL aliquots of KIO3 solution. Assume that the procedure for BOD determination experiment done here is same to our class experiment. A 0.1232 M B 0.1215 M с 0.1250 M D 0.1221 M

Solve for the average molarity of sodium thiosulfate titrant if 0.1532 g, 0.1573 g, 0.1551 g KIO3 (MW: 214.001 g/mol) consumed 3.60 mL, 3.56 mL, and 3.45 mL, respectively from three 10 mL aliquots of KIO3 solution. Assume that the procedure for BOD determination experiment done here is same to our class experiment. A 0.1232 M B 0.1215 M с 0.1250 M D 0.1221 M

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 10P

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Solve for the average molarity of sodium thiosulfate titrant if 0.1532 g, 0.1573 g, 0.1551 g KIO3 (MW: 214.001 g/mol) consumed 3.60 mL, 3.56 mL, and 3.45 mL, respectively from three 10 mL aliquots of KIO3 solution. Assume that the procedure for BOD determination experiment done here is same to our class experiment. 0.1215 M 0.1232 M 0.1221 M 0.1250 M
2,5 ml volume has taken from an “hypothetic” solution which includes (3+) Sb and (3+) Fe and at the titration with 0.1004 N KMnO4, the wasted amount has found as 16,4 mL. The other 2,5 mL that has taken, has reduced with Zn after that, this 2,5 mL solution has titrates with the same KMnO4 solution solution and the wasted amount is 26,5mL. With these datas find the %concentrations of the ions at the solution.
Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3
Which of the following statements is advantageous? A). The main differences between potentiometric and conductometric titrations are that potentiometric titrations exemplify the analyte sample-by-sample while conductometric titrations show the potential of the analyte B). A conductivity is analyl from the people of the charge. C.) Conductivity increases rapidly as close as equivalence, as a strong acid and a strong base will decrease D). The conductor remains constant according to the viscosity of the pixel, the decomposer and its size, which consists of design modelling.
A 0.5131-g sample that contains KBr (MM: 119.0023) is dissolved in 50 mL of distilled water. Titrating with 0.04614 M AgNO3 requires 25.13 mL to reach the Mohr end point. A blank titration requires 0.65 mL to reach the same end point. Report the %w/w KBr in the sample.
Calculate the alkaline strength of pearl ash (impure potassium carbonate) in terms of percent K2O from the following data: Sample = 0.3500 g; HCl used = 48.03 mL; NaOH used for back titration = 2.02 mL; 1.000 mL HCl = 0.005300 g Na2CO3; 1.000 mL NaOH = 0.02192 g KHC2O4.H2O. (Note: Use the least significant digits in your answer.)
A 370.00 mL solution of 0.00185 M A3B4 is added to a 390.00 mL solution of 0.00100 M C3D4. What is pQsp for A3D4?
answer the following: Let us assume that there is a 0.020 M EDTA titrant solution. Calculate the mass of pure dry CaCO3 standard to use such that the volume of titrant needed to reach the endpoint will be about 35mL if one mole of calcium carbonate reacts with one mole EDTA. Given choices: 0.050 g 0.060 g 0.070 g 0.080 g
Give typed full explanation not a single word hand written otherwise leave it An experiment requires a pH 6.5 buffer. Solid sodium acetate and glacial acetic acid available. Glacial acetic acid is 99% acetic acid by mass and has a density of 1.05 g/mL. If the buffer is to be 0.20 M in acetic acid, how many grams of NaC2H3O2 and how many milliliters of glacial acetic acid must be used?
Tony is showing a bacterium having high pH requirement for its growth. He then has to prepare a minimal medium at pH 9. Adding 0.5 ml of the pH indicator to 10 ml of the medium, the solution remained colorless. The pH of the medium was adjusted using 2.25 ml of the 0.05 N titrant. a. What was the pH indicator utilized? b. What is the amount of 1 N titrant needed to adjust 150 ml of minimal medium to pH 9? c.What was the titrant he used?
4. The molar absorptivities of the indicator weak acid HIn (K_{a} = 1.42 * 10 ^ - 5) and its conjugate base In at 570 were determined as epsilon(HIn) = 7120 and ε(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 ^ - 5 (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 and pH = 6.5 .
please stop rejecting. we pay for this service, so we deserve getting our answer! I do not want to have to put a claim in and report Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10