31. A buffer solution where [A-] is 100 times lower than [HA] has a pH equal...

Question

Question

31. A buffer solution where [A-] is 100 times lower than [HA] has a pH equal to:
a.pKa -100
b. pKa + 100
C. pKa-2
d. pKa +2

Answer 1

Answer #1

ре реле Le Tл) & THA Гнк)- 115 ) TA [sa I Too - гия от - plea -2 CPH _pka_a (Am)

Answer 2

Similar Homework Help Questions

1. (2pts) What is the pH of a buffer solution in which [HA] = [AC]? A....

1. (2pts) What is the pH of a buffer solution in which [HA] = [AC]? A. pH = 1 D. pH = POH B. pH = Ka E. pH=7.0 C. pH = pka
A buffer solution is made using a weak acid, HA HA , that has a p...

A buffer solution is made using a weak acid, HA HA , that has a p K a pKa of 6 6 . If the pH of the buffer is 5 5 , what is the ratio of [ A − ] [A−] to [ HA ] [HA] ?
10. For an aqueous solution labeled "0.10 M potassium bromide," A) the pH is greater than...

10. For an aqueous solution labeled "0.10 M potassium bromide," A) the pH is greater than 7. B) the pH = 13. D) the pH is less than 7. E) the pH = 7. C) the pH = 1. 11. For a 0.10 M solution of a weak acid, HA, with pKa = 6, which of the following is true? A) [HA] =[A-] B) [HA] does not equal [H3O+] C) [HA] =[H3O] D) [HA] = K E) [HA] = 0...

1.A buffer solution is made using a weak acid, HA , that has a pKa of...

1.A buffer solution is made using a weak acid, HA , that has a pKa of 5 . If the pH of the buffer is 8 , what is the ratio of [A−] to [HA] ? 2. A buffered solution containing dissolved aniline, C6H5NH2, and aniline hydrochloride, C6H5NH3Cl, has a pH of 5.40. A. Determine the concentration of C6H5NH3+ in the solution if the concentration of C6H5NH2 is 0.320 M.. The pKb of aniline is 9.13. B. Calculate the change...
1. The pH of a HA/A = 1/10 buffer is (pKa 4.8) (A) 4.8 (B) 5.8...

1. The pH of a HA/A = 1/10 buffer is (pKa 4.8) (A) 4.8 (B) 5.8 (C) 5.85 (D) 5.9 (E) 6.0 2. Which of the following values is closest to the pH of 10 M NaOH (A) 11 (B) 10 (C) 8 (D) 12 (E) 9 3. The pH of a solution containing 0.01 M HCl plus 0,04M KCIO, is: (The activity coefficient of H' in this solution is 0.86) (A) 2.07 (B) 1.97 (C)3.00 (D) 1.00 (E) 2.04...
1) You have 50 mL of a buffer solution that is 0.15 M in HA and...

1) You have 50 mL of a buffer solution that is 0.15 M in HA and 0.25 M in A-. Calculate the pH of the solution after you add 100 mL of 0.01 M HCl to the solution. The pKa of HA is 4.75. 2)You wish to prepare 100 mL of a buffer solution that is 0.025 M in carbonic acid (H2CO3). The pKa of H2CO3 is 6.351. Calculate the amount of H2CO3, in grams, that you will need to...

Consider two buffer solutions. Buffer 1 consists of 0.50 M HA and 0.25 M KA, and...

Consider two buffer solutions. Buffer 1 consists of 0.50 M HA and 0.25 M KA, and Buffer 2 is made from 0.050 M HA and 0.050 M NaA. How do the pHs of these buffer solutions compare? Select one or more: a. The pH of Buffer 1 is twice the pH of Buffer 2. b. The pH of Buffer 1 is half the pH of Buffer 2. c. The pH of Buffer 1 is equal to the pH of Buffer...
A buffer solution is made using a weak acid, HA, with a pKa of 5.88. If...

A buffer solution is made using a weak acid, HA, with a pKa of 5.88. If the ratio of [A-] to [HA] is 0.010, what is the pH of the buffer? pH
An unknown weak acid, HA, is used to create a buffer solution. When the concentrations are...

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})

A student wishes to prepare a buffer solution at pH = 5.60. Which of these weak...

A student wishes to prepare a buffer solution at pH = 5.60. Which of these weak acids (HA, HB and HC) should he/she choose: HA (pKa = 2.57), HB (pKa = 5.36), or HC (pKa = 8.59)? Select one: a. Only HA b. Only HC c. Only HB d. HA or HB e. None of HA, HB or HC