a) What is the buffer range for a buffer made with formic acid (HCOOH)? (Ka = 1.8 x 10-4)
b) What is the buffer range for a buffer made with CH3NH2 ? (Kb = 3.7 x 10-4) Be sure to think of the conjugate acid.
a)
use:
pKa = -log Ka
= -log (1.8*10^-4)
= 3.74
pH range of buffer is pKa-1 to pKa+1
SO, here buffer range is 2.74 to 4.74
Answer: 2.74 to 4.74
b)
use:
Ka = Kw/Kb
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
Ka = (1.0*10^-14)/Kb
Ka = (1.0*10^-14)/3.7*10^-4
Ka = 2.703*10^-11
use:
pKa = -log Ka
= -log (2.703*10^-11)
= 10.57
pH range of buffer is pKa-1 to pKa+1
SO, here buffer range is 9.57 to 11.57
Answer: 9.57 to 11.57
a) What is the buffer range for a buffer made with formic acid (HCOOH)? (Ka =...
1. What is the pOH of 2.9 ×
10-7 M KOH?
2. Formic acid (HCOOH) undergoes the following dissociation
reaction:
HCOOH ⟷
H+ + HCOO- Ka = 1.8 ×
10-4
What would be the Kb value of its conjugate base?
A solution of 7.95 M formic acid (HCOOH) is 0.47% ionized. what is the K, value of formic acid? 1.8 x 10-4 3.7 3.7 x 10-2 more data is needed 4.7 x 10-
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A solution buffered at pH 3.90 is needed for a reaction. Would formic acid (HCOOH = HA) and its salt, sodium formate, NaHCO2 = NaA), make a good choice for this buffer? If so, what ratio of moles of A- and HA is needed? Use the Henderson Hasselbalch Equation. Ka formic acid = 1.8 x 10-4
0. A solution of formic acid (HCOOH, Ka 1.8 x 10) has a pH of 2.70. Calculate initial concentration of formic acid in this solution.
Question 4 2 pts If 11 drops of a formic acid (HCOOH) solution are titrated with 10 drops of a 0.12 M NaOH solution, what is the percent ionization of the formic acid solution? (Ka for formic acid 1.78 x 104) 4.0% 1.3% 1.9% @ 2.5% Question 5 2 pts What is the pH of an acetic acid solution if 25 drops are titrated with 44 drops of a 0.45 M KOH solution? (K, for acetic acid 1.8 x 105)...
Given the following information: formic acid HCOOH Ka = 1.8×10-4 triethylamine (C2H5)3N Kb = 5.2×10-4 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.167 Maqueous formic acid and triethylamine are mixed. It is not necessary to include states such as (aq) or (s). Use HCOO- as the formula for the formate ion. -reactant or product favored? -pH is >, <, = to 7?
What is the percent ionization in a 0.300 M solution of formic acid (HCOOH) (Ka 1.78 x 10-4)?
Calculate the pH of a 0.065 M formic acid (HCOOH)
solution.
Formic acid is a weak acid with Ka = 1.8 ×
10–4 at 25°C.
2.48 is WRONG answer!!!!!!
Write your answer to two decimal places. Calculate the pH of a 0.065 M formic acid (HCOOH) solution. Formic acid is a weak acid with 1.8x 10at 25°C. pH 2.48
25.0 mL of 0.10 M formic acid (HCOOH, Ka = 1.8 x 10-4) is mixed with 20.0 mL of 0.10 M potassium hydroxide. What is the pH of the resulting solution? A. 2.37 B. 4.35 C. 13 D. 0.60