4 Design a buffer that has a pH of 7.34 using one of the weak base/conjugate acid systems shown below.KapkaWeak BaseCH3NH2C6H1503N10.62Kb4.2 x 10-45.9 x 10-71.5 x 10-⁹Conjugate AcidCH3NH3*C6H1503NH*C5H5NH*2.4 x 10-111.7 x 10-86.7 x 10-67.77C5H5N5.17How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?grams chloride salt of conjugate acid =grams weak base =

Given pH of buffer = 7.34select a weak base out of three choicess whose pKb is close to required…

Design a buffer that has a pH of 7.34 using one of the weak base/conjugate acid systems shown below. Ka pKa Weak Base CH3NH2 C6H1503N Kb 4.2 x 10-4 Conjugate Acid CH3NH3* C6H1503NH+ 10.62 5.9 x 10-7 2.4 x 10-11 1.7 x 10-8 6.7 x 10-6 7.77 C5H5N 1.5 x 10-⁹ C5H5NH* 5.17 How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams chloride salt of conjugate acid = grams weak base =

Design a buffer that has a pH of 7.34 using one of the weak base/conjugate acid systems shown below. Ka pKa Weak Base CH3NH2 C6H1503N Kb 4.2 x 10-4 Conjugate Acid CH3NH3* C6H1503NH+ 10.62 5.9 x 10-7 2.4 x 10-11 1.7 x 10-8 6.7 x 10-6 7.77 C5H5N 1.5 x 10-⁹ C5H5NH* 5.17 How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams chloride salt of conjugate acid = grams weak base =

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 2SP: Choose a weak-acid/weak-base conjugate pair from which you could prepare a buffer solution with pH =...

See similar textbooks

Similar questions

Determine the dominant acid-base equilibrium that results when each of the following pairs of solutions is mixed. Indicate the equilibrium by writing 1 for a strong acid, 3 for a weak acid, 4 for an acidic buffer, 7 for a neutral solution, 10 for a basic buffer, 11 for a weak base, and 13 for a strong base. (a) 10.0 mL of 0.15 M NaOH + 15.0 mL of 0.10 M HNO3 (b) 25.0 mL of 0.10 M HCl + 10.0 mL of 0.25 M NH3 (c) 50.0 mL of 0.050 M NaOH + 50.0 mL of 0.10 M NH3 (d) 50.0 mL of 0.10 M NH3 + 50.0 mL of 0.05 M HCl
What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.
Choose a weak-acid/weak-base conjugate pair from which you could prepare a buffer solution with pH = 7.5. Explain how you chose the conjugate pair. Calculate the ratio [weak base]/[weak acid) required to give pH = 7.5.
Calculate the pH of solutions that are 0.25 M formic acid and 0.40 M sodium formate. 0.50 M benzoic acid and 0.15 M sodium benzoate.
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
Enough water is added to the buffer in Question 29 to make the total volume 10.0 L. Calculate (a) the pH of the buffer. (b) the pH of the buffer after the addition of 0.0500 mol of HCl to 0.600 L of diluted buffer. (c) the pH of the buffer after the addition of 0.0500 mol of NaOH to 0.600 L of diluted buffer. (d) Compare your answers to Question 29(a)-(c) with your answers to (a)-(c) in this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity.
8-71 Explain why you do not need to know the chemical formula of a buffer compound to use it.
The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107
A solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein
Which of these combinations is the best to buffer the pH at approximately 9? Explain your choice. CH3COOH/NaCH3COO HCl/NaCl NH3/NH4Cl