5. Phosphate buffer is commonly used in biochemical work due to its second pka of 7.2. The two forms of phosphate used in buffers are known as monobasic (H₂PO4¹) and dibasic (HPO4²). Molar mass of KH₂PO₂ = 136.1 g/mol and Molar mass of K₂HPO4 = 174.2 g/mol a. Write an exact recipe for creating 1L stock of 0.5M potassium phosphate buffer, pH 7.0 out of solid mono- and dibasic potassium phosphate. Show your calculations.

5. Phosphate buffer is commonly used in biochemical work due to its second pka of 7.2. The two forms of phosphate used in buffers are known as monobasic (H₂PO4¹) and dibasic (HPO4²). Molar mass of KH₂PO₂ = 136.1 g/mol and Molar mass of K₂HPO4 = 174.2 g/mol a. Write an exact recipe for creating 1L stock of 0.5M potassium phosphate buffer, pH 7.0 out of solid mono- and dibasic potassium phosphate. Show your calculations.

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...

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Hh.84.
3 NEXT > < PREV 1 2 Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = = 6.3 × 10-5 RESET [0] [21.5] [37.7] [0.176] [0.261] [0.880] [1.31] [0.178] [0.888] [x] [2x] [21.5-x] [37.7+x] [0.176-x] [0.261 + x] [0.880 - x] [1.31 + x] [0.178 + x] [0.888 + x] < PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Ka (Part 2), determine the pH of the buffer solution. pH = RESET 0 4.2 x 10-5 6.23 4.37 2.4 × 10-11 7.77 9.63 0.880
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Q3
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