You need to make a buffer solution with pH of 8.0. You have the following reagents on your shelf:
HC3H5O3 Ka=1.4*10-4 | NaF |
HF Ka=6.6*10-4 | Tris-base |
HC2H3O2 Ka=1.8*10-5 | NH3 |
HClO Ka=2.9*10-8 | NaC2H3O2 |
Tris-HCl Ka=8.3*10-9 | NaClO |
NH4Cl Ka=5.6*10-10 | NaC3H5O3 |
a) Which reagents would you use to make the buffer solution. Briefly explain why you would choose these.
b) In what ration of molar concentrations would you combine them?
a) According to Handerson Hasselbach equation for buffers,.
pH = pKa + log [base] / [acid]
And, buffer would be more effective when pH = pKa
ie when [base] = [acid]
So,
a)
Tris HCl which is having
pKa = - log (Ka) = - log (8.3 x 10^-9) = 8.0 (approx)
and its corresponding base ie Tris base would be best suitable to make the buffer of desired pH.
other reagents would have pKa values that have a higher mismatch with that of pH value ie 8.
b)
since, pH = pKa which means [base] = [acid] . Therefore we would combine them in 1:1 mole ratio.
You need to make a buffer solution with pH of 8.0. You have the following reagents...
In this problem you will predict the pH of a buffer solution and then predict the new pH after you add NaOH or HCl. Write your answers to three decimal places (X.XXX). The Ka of HC2H3O2 is 1.8×10−51.8×10−5. 1) Calculate the pH of a buffer made from mixing 11.011.0 mL of 0.080.08 M NaC2H3O2 and 9.29.2 mL of 0.080.08 M HC2H3O2. 2) Calculate the pH of the buffer when 5.25.2 mL of 0.0090.009 M NaOH is added to the buffer...
How many moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a buffer with a pH of 3.60? (Ka for HF is 6.8 x 10-4)
What is the pH of a buffer solution containing 0.13 M HF and 5.0×10−2 M NaF? What is the pH of a buffer solution containing 1.0×10−2 M HF and 0.16 M NaF? Using the table given below for Ka values, compare the pH of an HF buffer that contains 0.13 MHF and 5.0x10-2 M NaF with another HF buffer that contains 1.0x10-2 MHF and 0.16 M NaF. Ka and K b values for selected weak acids and bases HF Acid...
During this part #3 of the lab, you will make 2 acetic acid buffer solutions (HC2H3O2/NaC2H3O2) of the same pH (pH = 4.0), but with different concentration of the components. Use the Henderson -Hasselbalch equation to perform the following calculations. The Ka of acetic acid is 1.8 x 10-5 M. a. Buffer A: Calculate the mass of the solid sodium acetate (NaC2H3O2) required to mix with 100 ml of 0.1 M acetic acid (HC2H3O2), to prepare a pH 4 buffer....
1. To prepare a buffer solution with a pH of 3.7. Which of the following conjugated pairs would be the best option? A. HSO4- / SO42- Ka = 1.2 x10-2 B. HCN / CN- Ka = 4.0 x 10-10 C. HCHO2 / CHO2- Ka = 1.8 x 10-4 D. H2CO3 / HCO3 Ka = 4.2 x 10-7 E. HClO / ClO- Ka = 2.9 x 10-8
1.) A buffer solution was prepared by mixing 100. mL of 0.500M HF (Ka = 6.6 × 10-4) and 250. mL of 0.250M NaF. You plan to destroy this buffer by addition of KOH. What would be the minimum amount (in grams) of KOH to destroy this buffer? a. 5.94 g b. 3.95 g c. 2.81 g d. 7.27 g e. 4.25 g
4. If you want to make a buffer of 4.5 pH, how many grams of NaF do you need to add to 300 mL of 0.4 M HF solution? (Ka=7.1x10-4) Answer: 114.66 grams Pka -log (7.1 X10-4) = 3.1487411651 234
Calculate the pH of a buffer solution prepared by dissolving 1.79 mol of HF and 2.26 mol of NaF in water to make a total volume of 1.25 L of solution. The Ka of HF is 6.8*10^-4. A) 3.57 B) 3.47 C) 3.27 D) 3.37 E) 3.68 Please let me know what answer is correct and how to work it. Thank You!
You have stock solution of 10M Tris, pH 8.0 and 5 M NaCl. You want to make a one liter buffer of 1M Tris buffer and 50 mM NaCl. How would you do that?
5. You need to make 500.0 mL of a buffer with a pH of 2.20. You have the following substances to work with: 0.100 M NH3 Solid NaN3 Solid NaClO2 0.100 M HClO2 Solid NH4Cl Solid Na2SO3 0.100 M HN3 Solid NaHSO3 Ka for HClO2 = 1.1x10-2 Kb for NH3 = 1.8x10-5 Ka for HN3 = 1.9x10-5 Ka1 for H2SO3 = 1.7x10-2 Ka2 for H2SO3 = 6.4x10-8 (Assume that the addition of solid does not change the volume of the...