A chemistry graduate student is given 250. mL of a 0.10M methylamine (CH3NH2) solution. Methylamine is a weak base with K 4.4 x 10CH3NH2Br should the student dissolve in the CH3NH2 solution to turn it into a buffer with pH = 10.21?What mass ofYou may assume that the volume of the solution doesn't change when the CH3NH3Br is dissolved in it. Be sure your answer has a unit symbol, and round it to2 significant digits.0☐ x10XG

The pH of a buffer solution is associated by the Henderson-Hasselbalch Equation (HHE). pKa is the…

Answered: A chemistry graduate student is given…

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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An aqueous solution contains 0.494 M ethylamine (C2H5NH2).How many mL of 0.206 M hydroiodic acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 10.600? mL??
1. Which of the following aqueous solutions are good buffer systems?. 0.35 M ammonia + 0.31 M calcium hydroxide 0.20 M hypochlorous acid + 0.19 M potassium hypochlorite 0.34 M potassium bromide + 0.25 M sodium bromide 0.17 M barium hydroxide + 0.30 M barium bromide 0.28 M hydroiodic acid + 0.18 M sodium iodide 2.A solution contains 0.124 M (CH3)2NH2 and 0.464 M dimethylamine, (CH3)2NH.The pH of this solution is .
An aqueous solution contains 0.18 M ammonium chloride. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) O 0.04 mol Ba(OH)2 O 0.08 mol HCIO4 O 0.18 mol HClO4 O 0.17 mol BaCl2 O 0.17 mol NH3
An analytical chemist is titrating 127.5 mL of a 0.5600 M solution of cyanic acid (HCNO) with a 0.4600 M solution of NaOH. The p K of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 74.40 mL of the NaOH a solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = | ?
Equal volumes of solutions of the given concentrations are mixed together. Which of the resulting aqueous solutions makes a buffer? Group of answer choices 0.1 M HCl + 0.2 M CaCl2 0.1 M HCl + 0.2 M NH3 0.1 M CH3COOH + 0.2 M NaOH 0.1 M CH3COONa + 0.2 M NaOH 0.25 M HCl + 0.2 M NH3
Determine whether or not the mixing of each pair of solutions results in a buffer.a. 100.0 mL of 0.10 M NH3; 100.0 mL of 0.15 M NH4Clb. 50.0 mL of 0.10 M HCl; 35.0 mL of 0.150 M NaOHc. 50.0 mL of 0.15 M HF; 20.0 mL of 0.15 M NaOHd. 175.0 mL of 0.10 M NH3; 150.0 mL of 0.12 M NaOHe. 125.0 mL of 0.15 M NH3; 150.0 mL of 0.20 M NaOH
The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of carbonic acid (H2CO3) to that of the bicarbonate ion (HCO3−). (Ka1 of carbonic acid is 4.2 × 10−7.)
a Calculate the pH of a solution that is 0.20 M HOCI and 0.88 M KOCI. Ka = 3.5x10-8 pH = 8.1 b In order for HOCI/KOCI buffer to have pH = pKa, would you add HCI or NaOH? pKa = 7.46 pH = 8.1 NaOH O HCI What quantity (moles) of HCI would you add to 1.0 L of the original buffer (0.20 M HOCI and 0.88 M KOCI) so that the resulting solution has pH = pKą? pka = 7.46 Quantity = mol Submit
Which of the following buffers has the greatest buffering capacity? Buffer A: Buffer B: Buffer C: 1.0 M NH3 0.98 M NH4+CI 0.30 M NH3 0.35 M NH4+CI 0.50 M NH3 0.50 M NH4+CI Buffer A O Buffer B Buffer C All of these buffers have the same buffer capacity.
What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acid's conjugate base? The acid's ionization constant is Ka=6.7×10^−4 . Use the Henderson-Hasselbach equation Remember to use the rules for significant figures for your answer. For pH values only the digits to the right of the decimal point are considered significant figures. pH =
You need to make a buffer whose pH is 7.0, and you can choose from the weak acids shown. Briefly explain your choice
4. How many moles of NH4C1 must be added to 2.0 L of 0.10 M NH3 to form a buffer whose pH is 9.00? (Kb =1.8x10-5. Assume that the addition of NH4C1 does not change the volume of the solution.)

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