A buffer system is set up with [HA]=2.0[A^-]. if Pka = 4.8, what is the pH of the buffer?
HA = 2.0 A-
pH = pka + log ( A- / HA) [ handerson hasselbalch equation]
= 4.8 + log ( A- / 2 A-)
= 4.49897
If you have any questions please comment
If you satisfied with the solution please rate it thanks
A buffer system is set up with [HA]=2.0[A^-]. if Pka = 4.8, what is the pH...
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...
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
A buffer solution is made using a weak acid, HA, with a pKa of 4.20. If the ratio of AT to HA is 1.0 x10?, what is the pH of the buffer? Number pH-
A buffer solution is made using a weak acid, HA, with a pKa of 8. If the ratio of A– to HA is 0.1, what is the pH of the buffer?
A) If the weak acid in a buffer system has pKa 10.5, in what pH range is the system a most effective buffer? B) In the phosphate buffer system containing K2HPO4 and KH2PO4, what is the weak acid? What is its conjugate base?
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
The pH of a buffer is calculated by using the Henderson-Hasselbalch equation: pH=pKa +log[Base]/[Acid] Part A: What is the pH of a buffer prepared by adding 0.809mol of the weak acid HA to 0.406mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66
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...
What are the predominant forms of acetic acid (pKa is 4.8) at a pH of 2 and a pH of 7?