141480 4. A student needs to prepare a buffer solution with a pH of 5.59. Assuming a pka of 4.54, how many mL of 0.1 M NaOH would need to be added to 24.0 mL of 0.1 M HB to prepare this buffer? Please include a proper (abbreviated) unit. HINT: Use pH = pKa + log ([B-]/[HB]) or, if concentrations are the same, pH = pka + log (Volume of OH-/ (Volume of HB - Volume of OH-) mis

141480 4. A student needs to prepare a buffer solution with a pH of 5.59. Assuming a pka of 4.54, how many mL of 0.1 M NaOH would need to be added to 24.0 mL of 0.1 M HB to prepare this buffer? Please include a proper (abbreviated) unit. HINT: Use pH = pKa + log ([B-]/[HB]) or, if concentrations are the same, pH = pka + log (Volume of OH-/ (Volume of HB - Volume of OH-) mis

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...

See similar textbooks

Similar questions

Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M pyridine with 0.100 M hydrochloric acid (Kb for pyridine is 1.7 109). Do not calculate the points at 24.9 and 25.1 mL.
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
One drop, 0.200 cm3, of 1.00 mol dm-3 of aqueous sodium hydroxide, NaOH, solution is added to 25.0 cm3 of a phosphate buffer that is 0.040 mol dm-3 in KH2PO4(aq) and 0.020 mol dm-3 in K2HPO4(aq). Calculate the resulting pH of the solution given that the second acid dissociation constant, pKa2, for phosphoric acid is 7.21.
A. What is the pH of a 350 mL buffer containing 0.125 mol HCOOH and 0.150 mol HCOONa? Ka=1.70x10-4B. Propionic acid, CH3CH2COOH, has a Ka of 1.3x10-5 M. What mass of CH3CH2COONa would have to beadded to 1.00L of 0.500M propionic acid for a resulting solution of pH=5.00?
When titrating a 25 mL solution of 0.20M CH3COOH with 0.10M KOH, you realize you forgot to add an indicator initially. You've added 10 mL of KOH to the flask of acid. Ka of CH3COOH = 1.8 x 10^-5 1) Calculate the pH at this point 2) What color would your solution be if you add 40 mL KOH more. And a few drops of clorophenol blue indicator at this point. Why?
You make a 200mM potassium phosphate buffer (pKa of 7.20) with monobasic potassium phosphate (molecular weight 136.09 g/mol) and dibasic potassium phosphate (174.20 g/mol). For 100mL of buffer, at a pH of 7.20, how many grams of monobasic potassium phosphate are needed? Please walk through this step-by-step.
A 1.00 L volume of buffer is made with concentrations of 0.350 M sodium formate (NaHCOO) and 0.550 Mformic acid (HCOOH). (Ka of HCOOH is 1.8 x 10^-4)a. Calculate the initial pH of this bufferb. What is the pH after the addition of 0.0050 mol HCl?c. How about after the addition of 0 0050 mol NaOH[For parts b and c, assume that volume doesn t change in the addition process and that neutralization proceeds to completion]
A 1.0L buffer is made at 25°C that consists of 0.80 mol of a weak acid HA and 0.80 mol of its conjugate base A-. The acid ionizarion constant is Ka= 1×10^-4. To this buffer solution 0.80 mol NaOH is added. Assuming that the volume change due to the added NaOH is negligible, calculate pOH in the resulting solution.
Your goal is to make a buffer with a pH of 4.75 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of 1 M sodium acetate added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.
1. How would you prepare 500.0 mI. of 0.050 M phosphate buffer solution, pH 6.7 from 0.20 M solutions of acid and salt? 2. What will be resulting pH of the buffer in Question #1 if the following are added: a. 1.0 mL of 1.0 M HCI b. 1.0 mL of 1M NaOH 3. Compare the results in question # 2 if these reagents were added to 500 mL of distilled water instead? Interpret your results.
Can someone please explain why and how the step 1 was done? What was its purpose? Why was only the pKa2 value was used in the second step 2? I don't understand shortcuts and I would appreciate it if it's explained step by step. This was the solution to my previous question in which I asked: What is the pH of a buffer prepared by mixing 100 mL 0.050 mM NaH2PO4 and 25 mL 0.075 mM Na2HPO4? (pKa1=2.2; pKa2= 7.21; pKa3=12.7)