If the equilibrium constant for the acid dissociation is KA and pKA (-log Ka) =7.0, what is the ratio of [HPO42-] to [H2PO4−] in this buffer system? Please show your calculation.
The molar ratio is calculated using the Henry Hasselbach equation:
[HPO4-2] / [H2PO4-2] = 10 ^ (pH - pKa) = 10 ^ (7 - 7.2) = 0.63
If you liked the answer, please rate it in a positive way, you would help me a lot, thank you.
If the equilibrium constant for the acid dissociation is KA and pKA (-log Ka) =7.0, what...
The acid dissociation constant ka for an acid is 1x10-6 what is the pka? show the work
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
If a buffer were needed with a pH of 7.0, what would be the best combination of weak acid and conjugate base to formulate the buffer? (please explain why you chose your answer) A) H3PO4 and H2PO4- B) H2PO4- and HPO42- C) HPO42- and PO43- D) acetic acid and acetate E) lactic acid and lactate
The acid dissociation constant, Ka, is 1x10-5 for a monoprotic mystery acid, HMyst. What is the percent dissociation of a 0.10M HMyst? Show all work clearly so I can follow along please.
The acid dissociation constant, Ka, is 1x10-5 for a monoprotic mystery acid, HMyst. What is the percent dissociation of a 0.10M HMyst? Show all work clearly so I can follow along please.
Equations pH=-log[H3O+]; pOH= -log[OH]; pKw=14.00=pH+POH; Ka-[H3O+][A-[HA]; Kb=[BH+][OH-)[B); pKa=-log Ka; Ka. Kb=Kw Constants Ka (HS-)=1x10-19; Ka (HF) 7.2x10-4; Ka ([Al(H20).]+)7.9x10-6; Ka (H3PO4)=7.5x10-2: Ka (HPO42-) =3.6x10-13; Ka (HCI)=Huge; Ka(Na+)=tiny; Ka(Cl-)tiny; Kb(NH3)=1.8x10-5; Kw=1x10-14 1) Calculate the pH of aqueous 0.25M HCl and 0.25M HF solutions. 2) Complete the following tables for aqueous solutions of conjugate acid-base pKa pKb Kb 1.3x10-4 35 3) Complete the following table for aqueous solutions DHL TH+) OH) pOH 1x102 4) Calculate the pH of aqueous 0.15M Ba(OH)2 and...
The equilibrium constant for HBro is Ka=2.3×10^-9 1. What is the pKa for hypobromous acid? 2. What is the pH at half-way to the equivalence point for HBrO? 3. Here 20.00ml of 0.1100M hypobromous acid, HBro, is titrated with 0.1000 M NaOH. what is the initial pH of the solution that will be titrated? 4. What is the pH after 5.50ml of NaOH solution is added?
Base/Acid Ratios in Buffers Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, pKa=?logKa The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: pH=pKa+log[base][acid] Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. Part A Acetic acid has a Ka of 1.8
H2A is a diprotic acid of which pKa values are 3.0 and 7.0. Answer to the following questions. (d) Please explain how to prepare 0.1 M buffer solution with the pH of 7.4. Assume that the equilibrium concentrations of an acid and its conjugate base remain close to their formal concentration and that the buffer solution behaves ideally at room temperature. (10 pt) (d) Please explain how to prepare 0.1 M buffer solution with the pH of 7.4. Assume that...
(a) HA(aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a solution 0.066 M in A-(aq)? The temperature is 25oC. (b) For the reaction A(g) ⇋ B(g) + C(g), the equilibrium constant is 1.80 at 25.0oC and 4.36 at 75.0oC. Assuming ΔH and ΔS do not change with the temperature, calculate the value of the equilibrium constant at 50.0oC and the value of ΔSuniverse at 50.0oC.