28. Answer the following questions to find the mass (g) of dipotassium phthalate must be added to 250 mL of 0.0250 M phthalic acid to give a buffer of pH 5.75? MW K2P = 242.32 g/mol Ka2 = [H30^+] [P^-] / [HP^-] = 3.91 x 10^-6 %3D %3D %3D What is the amount of P^2- needed in the buffer?

28. Answer the following questions to find the mass (g) of dipotassium phthalate must be added to 250 mL of 0.0250 M phthalic acid to give a buffer of pH 5.75? MW K2P = 242.32 g/mol Ka2 = [H30^+] [P^-] / [HP^-] = 3.91 x 10^-6 %3D %3D %3D What is the amount of P^2- needed in the buffer?

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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Calculate the pH of solution after the addition of 0.010 mol NaOH to 1.00L of a 0.100 M acetic acid / 0.100 M sodium acetate buffer solution. (Ka = 1.8 x 10*) What is the neutralization reaction that happens? Is the system still a buffer after neutralization?
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1. How do you prepare a 100mL of 0.1 M phosphate buffer?To make 100 mL of 0.1 M phosphate buffer: Calculate the amount of sodium phosphate needed. moles of sodium phosphate = (0.1 mol/L) x (0.1 L) = 0.01 moles mass of sodium phosphate = moles x molar mass = 0.01 moles x 142 g/mol = 1.42 g Dissolve 1.42 g of sodium phosphate in distilled water in a 100 mL volumetric flask. Adjust the pH of the solution to the desired value (usually around 7.4) using a strong acid or strong base. Bring the solution to the final volume (100 mL) with distilled water. 2. From the anterior buffer, how do you make 100mL of 0.05 M? To make 100 mL of 0.05 M phosphate buffer from the 0.1 M stock solution: Calculate the amount of the 0.1 M phosphate buffer needed. moles of phosphate buffer = (0.05 mol/L) x (0.1 L) = 0.005 moles Calculate the volume of the 0.1 M phosphate buffer needed. moles = concentration x volume (in liters) volume = moles / concentration = 0.005 moles / 0.1 mol/L = 0.05 L or 50 mL Measure…
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