The equilibrium constant for the conjugate acid/base pair is8.0 x10-5HIn + H₂OH3O+ + In. From additional information:SpeciesAbsorptionMolar absorptivityMaximum, nm430 nm600 nmHIn4308.04×10³1.23x10³In6000.775×1036.96x103(a) Calculate the absorbance at 430 nm and 600 nm for thfollowing indicator concentrations: 3.0 x10-4 M, 2.0 × 10-4 M.and 1.0 ×10-4 M, 0.5 ×10-4 M and 0.25 ×10-4 M.(b) Plot absorbance as a function of indicatorconcentration.(c) Discuss the linearity of the graph of the two absorbancefunctions.

Lambert- Beer's law states that when a monochromatic light passes through a medium, its absorbance…

(a) Calculate the absorbance at 430 nm and 600 nm for th following indicator concentrations: 3.0 x10-4 M, 2.0 ×10-4 M. and 1.0 x10-4 M, 0.5 x10-4 M and 0.25 ×10-4 M. (b) Plot absorbance as a function of indicator concentration. (c) Discuss the linearity of the graph of the two absorbance functions.

(a) Calculate the absorbance at 430 nm and 600 nm for th following indicator concentrations: 3.0 x10-4 M, 2.0 ×10-4 M. and 1.0 x10-4 M, 0.5 x10-4 M and 0.25 ×10-4 M. (b) Plot absorbance as a function of indicator concentration. (c) Discuss the linearity of the graph of the two absorbance functions.

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

A sufficient quantity of each of the following aqueous solutions has been made available to you: (i) 0.2M NaH2PO4; (ii) 0.1M Na2HPO4 (a) How many ml of each of these two solutions would you require to mix together in order to prepare one litre of a 0.01M phosphate buffer pH 7.2? [For H3PO4: pKa1 = 2.15; pKa2 = 6.82; pKa3 = 12.38]. (Ans. = 14.7 ml 0.2M NaH2PO4; and 70.6 ml Na2HPO4). (b) Having calculated these volumes (of 0.2 M NaH2PO4 and 0.1M Na2HPO4) required, what further steps would you take to prepare the 0.01M phosphate buffer solution of pH 7.2?
Which type of indicator is used in permanganatometry titrant plays role of indicator by itself; irreversible Red/Ox indicator; reversible Red/Ox indicator; metallochrome indicator;
A 250-mL buffer solution contains 0.0510 mole of KH2PO4 and 0.0875 mole of K2HPO4. (a) Calculate the molar concentrations of H2PO4–and HPO42–, respectively, in thesolution. (b) What is the pH of the solution? (H2PO4– has Ka = 6.2 x 10–8) (c) Write a net ionic equation for the buffering reaction against a strong acid by this buffer. (d) If 0.012 mole of hydrochloric acid (HCl) is added to the solution, create a reaction table to show the buffering reaction and calculate the molar concentration of H2PO4–and HPO42–, respectively, in the resulting solution after the buffering reaction. (e) What is the pH of the resulting solution?
Sketch a plot of species fraction vs. pH for a base which has pkb 1 = 5.0 and pkb2 = 10.0.
The indicator phenolphthalein may be regarded as a weak monobasic acid. Explain briefly why the indicator is coloured pink when the solution in which it is present has excess of alkali.
Considering 0.1 M acqueous solutions of each of the following, which solution hasthe lowest pH?(A) Na2CO3 (B) Na3PO4 (C) Na2S (D) NaCl(E) CH3COONa
The first acid ionization constant of the oxoacid H;PO, is 8 x 10-2. What molecular structure do you predict for H;PO,? Will this acid be monoprotic, diprotic, or triprotic in aqueous solution?
Name: Date: Section: Report Sheet: pH: Measurement and Application. A: Determination of pH Using Acid-Base Indicators: Indicator Color NaH,PO, HC,H,O, ZNSO, Methyl Violet Thymol Blue Methyl Yellow Congo Red Bromocresol Green pH Range B: Measurement of the pH of Solutions Record the measured pH and the color observed using bromocresol green for each 0.1 M solution NaH,PO, HC,H,O, ZNSO, C: Determination of K, for a Weak Acid Volume Used(Liters) Moles [HC,H,O,] M HC,H;O, () HC,H,O, |NaC,H;O,] M NaC,H,O, (L) NaC,H,O; Buffer pH pK, HC,H,O, K, HC,H,O, 115
Calculate the concentration of nitrate ion in a solution of 0.10M barium nitrate solution following the epectroneutrality principle (ENP).
Write the equation for the reaction of each of the following bases in water and its corresponding Kb expression: (a) ammonia Kb (b) benzoate ion Kb (c) acetate ion Kb (d) monohydrogen citrate ion Kb (e) pyradine (C5H5N). Kb