The Ka of Tris is 8.5x10-9 and the pKa of Tris is 8.07. What are the [HA] and [A-] concentrations of this 0.50M buffer at pH 8.75?
Solution-
pH= pKa + log(base/acid)
=>8.75= 8.07 + log(base/acid)
=> log(A-/HA) = 0.68
=> (A-/HA) 10^0.68 = 4 .786301
=> (A-)= 4 .786301*(HA)
=>concentration of buffer = 0.5M
So (A-)+(HA)= 0.5
4 .786301*(A-)+(HA)= 0.5
5.786301*(HA)= 0.5
(HA)= 0.5/5.786301
=0.086411
=(A-)= 4.786301*(HA)
=4.786301*0.086411
=0.413589
(HA)= 0.0864
(A-)=0.414 M
The Ka of Tris is 8.5x10-9 and the pKa of Tris is 8.07. What are the...
3). I need to make a 0.50M Tris buffer with a pH of 8.75. I have access to Tris (a weak acid) and the sodium salt of Tris (think A-). The Ka of Tris is 8.5x10-9 and the pKa of Tris is 8.07. What are the [HA] and [A-] concentrations of this 0.50M buffer at pH 8.75? Part A: [HA] = _____
3). I need to make a 0.50M Tris buffer with a pH of 8.75. I have access to Tris (a weak acid) and the sodium salt of Tris (think A-). The Ka of Tris is 8.5x10-9 and the pKa of Tris is 8.07. What are the [HA] and [A-] concentrations of this 0.50M buffer at pH 8.75? Part B: [A-] = _____
I need to make a 0.50M Tris buffer with a pH of 8.75. I have access to Tris (a weak acid) and the sodium salt of Tris (think A-). The Ka of Tris is 8.5x10-9 and the pKa of Tris is 8.07. What are the [HA] and [A-] concentrations of this 0.50M buffer at pH 8.75? Part B: [A-] = _____
Which of the following compounds would make the best buffer at pH 7.5? Acetic acid, pKa= 4.76 N-tris(hydroxymethyl) methylglycine (Tricine), pKa = 8.15 N-2-hydroxyethylpiperazine-N’-ethansulfonic acid, pKa2= 7.6 Glycine, pKa2= 9.9 Tris(hydroxymethyl)aminomethane (Tris), pKa = 8.3 I believe 3 is the correct answer and therefore I am trying to answer the below question with this information. Using the answer that you selected from question 1 above: a. Explain how you would make the buffer starting with 1M HA and 1M A-...
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. What is the pH of a solution which is 0.025 M in weak base and 0.039M in the conjugate weak acid (Ka = 7.1 × 10-6)? 2. 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] ? 3.A buffer solution is made using a weak acid, HA . If the pH of the...
20. You need to prepare an acetate buffer of pH5.24from-a: 0.810Macetic acid solution and a 2.29MKOHsolution. If you have 880mL of the acetic acid solution, how many milliliters of the KOHsolution do you need to add-to- make a buffer of pH95.24? The pKa of acetic acid is 4.76.1 T mLmLT 21.-1f-a-buffer solution-is-0.450.M-in-a-weak-acid-(Ka=7.3x10^-6)-and-0.110-M-in-its-conjugated base. what-is-the-ph Ph=1 13.A monoprotic weak acid, HAHA, dissociates in water according to the reactionſ HA(aq)---H-(aq)+A-(aq)HA(aq)---H+(aq)+A-(aq) The equilibrium concentrations of the reactants and products are [HAl=0.290M[ [H-]=2.00X10-4M. and...
help with 5 and 6 please 5. Choose the effective pH range of a HF/Naf buffer. For HF, Ka = 3.5 x 10-4 6. If a small amount of a strong acid is added to buffer made up of a weak acid, HA, and the sodium salt of its conjugate base, NaA, the pH of the buffer solution does not change appreciably because a) the Ka of HA is changed. b) the strong acid reacts with Ato give HA, which...
Design a buffer that has a pH of 4.45 using one of the weak base/conjugate acid systems shown below. Weak Base Kb Conjugate Acid Ka pKa CH3NH2 4.2×10-4 CH3NH3+ 2.4×10-11 10.62 C6H15O3N 5.9×10-7 C6H15O3NH+ 1.7×10-8 7.77 C5H5N 1.5×10-9 C5H5NH+ 6.7×10-6 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...
A buffer solution is composed of 0.380 M HA, a weak monoprotic acid, and 0.760 M NaA, the sodium salt of the acid. The solution has a pH of 4.10. What is the Ka of the weak acid, HA? tks!!!!!!!!!!!!!