Question
In: Chemistry
(a) What is the pH of 0.89 M potassium formate, HCOOK? (The Ka of formic acid...
(a) What is the pH of 0.89 M potassium formate, HCOOK?
(The Ka of formic acid is
1.8 ✕ 10−4.)
(b) What is the pH of 0.65 M NH4Br? (The
Kb of ammonia is
1.76 ✕ 10−5.)
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
12. Calculate the pH of a 0.10 M solution of potassium formate, KHCOO. Ka of formic...
12. Calculate the pH of a 0.10 M solution of potassium formate,
KHCOO. Ka of formic acid (HCOOH) = 1.8 x 10^-4. Write the
dissociation equation and label each ion as acidic, basic, or
neutral. Also write the hydrolysis equation.
Dissociation equation: _____________________________________
cation: __________ anion: __________
Hydrolysis equation:
_________________________________________________________________________
What is the pH of a 0.01 M solution of formic acid ? The ka of...
What is the pH of a 0.01 M solution of formic acid ? The ka of
formic acid is 1.77 x 10-4
a) Calculate the pH of a 0.250 M solution of formic acid, HCO2H? Ka, HCO2H =...
a) Calculate the pH of a 0.250 M solution of formic acid,
HCO2H?
Ka,
HCO2H = 1.8 x
10-4. HCO2H(aq) ⇌HCO2-(aq)
+ H+(aq)
b) What is the concentration of HCO2H at
equilibrium?
Formic acid (HCOOH) has Ka= 1.8x10-4. What is the pH of a 0.01 M solution of...
Formic acid (HCOOH) has Ka= 1.8x10-4. What is the pH of a 0.01 M
solution of formic acid ?
PLEASE HELP I HAVE EXAM
Determine the pH during the titration of 24.3 mL of 0.310 M formic acid (Ka =...
Determine the pH during the titration of 24.3 mL of 0.310 M
formic acid (Ka = 1.8×10-4) by 0.442 M NaOH at the following
points. (a) Before the addition of any NaOH (b) After the addition
of 4.20 mL of NaOH (c) At the half-equivalence point (the titration
midpoint) (d) At the equivalence point (e) After the addition of
25.6 mL of NaOH
Determine the pH during the titration of 24.3 mL of 0.310 M formic acid (Ka =...
Determine the pH during the titration of 24.3
mL of 0.310 M formic acid
(Ka = 1.8×10-4) by
0.442 M NaOH at the following
points.
(a) Before the addition of any NaOH
(b) After the addition of 4.20 mL of
NaOH
(c) At the half-equivalence point (the titration midpoint)
(d) At the equivalence point
(e) After the addition of 25.6 mL of
NaOH
What is the pH of a 1.0 M solution of potassium formate, KHCO2? (No equilibrium constant...
What is the pH of a 1.0 M solution of potassium formate,
KHCO2? (No equilibrium constant given).
Calculate the pH of a 0.500M formic acid (HCOOH) solution. Ka for formic acid is 1.8×10-4.
Calculate the pH of a 0.500M formic acid (HCOOH)
solution. Ka for formic acid is
1.8×10-4.
What is the pH of 10.00 mLs of a 0.100 Molar formic acid solution (ka =...
What is the pH of 10.00 mLs of a 0.100 Molar formic acid
solution (ka = 1.9 x 10^-4) after the following additions: A. 0.00
mLs of 0.100 M lithium hydroxide, B. 5.00 mLs of 0.100 M lithium
hydroxide, C. 10.00 mLs of 0.100 M lithium hydroxide, D. 15.00 mLs
of 0.100 M lithium hydroxide
The Ka for Formic acid (HCO2H) is 1.8 x 10^-4. What is the pH of a...
The
Ka for Formic acid (HCO2H) is 1.8 x 10^-4. What is the pH of a 0.20
M aqueous solution of sodium formate (NaHCO2)? Show all the
work.
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