HEPES is a commonly used biochemical buffer with a pKa 7.5 at 25 °C. Please answer the questions below on the use of HEPES as a buffer. Use the Henderson-Hasselbalch equation.
a) What is the pH of a solution prepared by combining 100.0 mL of 0.50 M protonated HEPES with 50.0 mL of 0.20 M HEPES base and diluting to a final volume of 1.00 L?
b) You add 20 mL of 1.0 M NaOH to the solution prepared in Part a. What is the final pH and concentration of all relevant HEPES species in the resultant solution?
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HEPES is a commonly used biochemical buffer with a pKa 7.5 at 25 °C. Please answer...
HEPES is a commonly used biochemical buffer with a pKa 7.5 at 25 °C. Please answer the questions below on the use of HEPES as a buffer. Use the Henderson-Hasselbalch equation. a) What is the pH of a solution prepared by combining 100.0 mL of 0.50 M protonated HEPES with 50.0 mL of 0.20 M HEPES base and diluting to a final volume of 1.00 L? b) You add 20 mL of 1.0 M NaOH to the solution prepared in...
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.5? Note that the concentration and/or pH value may differ from that in the first question. STRATEGY 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid Step 1: Rearrange the Henderson Hasselbalch...
Hello, I will try this again I am trying to prepare a buffer from a solution of a weak acid. This is for part D. of Experiment 25 - Ph Measurements - buffers and their properties I am to be give an 0.50 M solution of weak acid with a given pKa, and I will preparre a buffer of a desired pH measurement (choose any pH) I must first dilute the acid solution to 0.10 M by adding 10 ml...
An unknown weak acid, HA, is used to create a buffer solution. When the concentrations are {HA} = 0.500 M and {A–} = 1.048 M, the pH of the buffer solution is 5.49. Use the Henderson-Hasselbalch equation to find the pKa of the weak acid. Henderson-Hasselbalch equation: pH = pKa + log({A–}/{HA})
4. (12 pts) A buffer is created by mixing 50.0 mL of 0.50 M C6H5N and 40.0 mL of 1.0M HC.HSNCI. What is the final pH of the solution if 20.0 mL of 0.50 M KOH is added to the buffer at 25 °C? K(C6H5N) - 1.4 x 10-9 To receive full credit, all work must be explicitly shown, including the relevant neutralization and hydrolysis chemical reactions that are occurring, and do not use the Henderson-Hasselbalch equation.
Phosphate buffered saline (PBS) is a buffer solution commonly used in biological research. The buffer helps to maintain a constant pH. The osmolality and ion concentrations of the solution usually match those of the human body. A) You need to prepare a stock solution at pH 7.00 with KH2PO4 and Na2HPO4 (pKa =7.21). What would be the respective concentration of these substances if you wish to obtain the final phosphate concentration [HPO4 −2 ] + [H2PO4 − ] = 0.3...
A 50 mL sample of 0.20 M propionic acid buffer (pKa 4.87 according to Google) has an initial pH of 4.77. After an unknown amount of 0.25 M HCl is added to the buffer, its pH has been lowered to 4.47. Using the Henderson-Hasselbalch equation, determine what volume of HCl was added to the buffer to cause the pH change, as well as the mass of Pr- necessary to return the buffer to its original pH.
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate acid and the ratio of the concentrations of the conjugate base and acid. The equation is important in laboratory work that makes use of buffered solutions, in industrial processes where pH needs to be controlled, and in medicine, where understanding the Henderson-Hasselbalch equation is critical for the control of blood pH. Part A As a technician in a large pharmaceutical research firm, you need...
pH
of 9.2
using ammonium nitrate: pKa= 9.24
2 Introduiction The Henderson-Hasselbalch equation, or A-1 HAl relates the pH of a buffer with the pKo of the acid and the concentration of the conjugate base A- and the monoprotic acid HA. In cq. (1), pH-_ log[H+], pK, =-log Ka, and [J]i and [JIe are the initial and equilibrium molar concentration of the Jth species, respectively. The buffering capacity of the buffer is given by [1] Ka H+ where K,e-1.0 ×...
4. The unknown x is in units of Molar. Given the volume from the beginning, how many moles of NaOH would this be? 5. Calculate how many mL of a 1 M NaOH solution you would need for the number of moles calculated in the previous question. When making a buffer using two solutions conjugate base - the calculations are very similar. one of the conjugate acid, one of the You are to make 100.0 mL of a 0.50 M...