Question
In: Chemistry
In the titration of 25.00 mL of 0.100 M acetic acid, what is the pH of...
In the titration of 25.00 mL of 0.100 M acetic acid, what is the pH of the resultant solution after the addition of 15.06 mL of 0.100 M of KOH? Assume that the volumes of the solutions are additive. Ka = 1.8x10-5 for acetic acid, CH3COOH.
Solutions
Expert Solution
no of moles of CH3COOH = molarity * volume in L
= 0.1*0.025 = 0.0025 moles
no of moles of KOH = molarity * volume in L
= 0.1*0.01506 = 0.001506 moles
CH3COOH + KOH -----------------> CH3COOK + H2O
I 0.0025 0.001506 0
C -0.001506 - 0.001506 0.001506
E 0.000994 0 0.001506
PKa = -logKa
= -log1.8*10^-5
= 4.75
PH = PKa + log[CH3COOK]/[CH3COOH]
= 4.75 + log0.001506/0.000994
= 4.75 + 0.1804
= 4.9304 >>>>>>>>>>>>>>answer
queen_honey_blossom answered 2 years agoRelated Solutions
In the titration of 25.00 mL of 0.100 M acetic acid, what is the pH of...
In the titration of 25.00 mL of 0.100 M acetic acid, what is the
pH of the resultant solution after the addition of 25.00 mL of
0.100 M KOH? Assume that the volumes of the solutions are additive.
Ka = 1.8x10-5 for CH3COOH.
What is the pH at the equivalence point for the titration of 25.00 mL 0.100 M...
What is the pH at the equivalence point for the titration of
25.00 mL 0.100 M CH3CH2CH2CO2- with 0.1848 M HCl? Species (K
values) CH3CH2CH2CO2H (Ka = 1.14E-5) CH3CH2CH2CO2- (Kb =
2.63x10-10
Consider the titration of 25.0 mL of 0.100 M acetic acid (HA) with 0.100 M NaOH....
Consider the titration of 25.0 mL of 0.100 M acetic acid (HA)
with 0.100 M NaOH.
1. Write the balanced chemical equation and equilibrium constant
expression (ECE) for all of the reactions that
occur when NaOH is added to the acetic throughout the titration.
Hint: think of what is in the solution (acetic
acid) with water, acetic acid with sodium hydroxide, and acetate
ion with water) as the titration is proceeding.
2. Calculate the volume of NaOH solution needed to...
For the titration of 50.0 mL of 0.150 M acetic acid with 0.100 M sodium hydroxide,...
For the titration of 50.0 mL of 0.150 M acetic acid with 0.100 M
sodium hydroxide, determine the pH when:
(a) 50.0 mL of base has been added.
(b) 75.0 mL of base has been added.
(c) 100.0 mL of base has been added.
titration of 25.00 ml of 0.100M CH3COOH with 0.100 M NaOH (weak acid, strong base) a)...
titration of 25.00 ml of 0.100M CH3COOH with 0.100 M NaOH (weak
acid, strong base)
a) calculate the initial pH ( kb = 1.8 x10 ^-5)
b) why is pH > 7 at the equivalence point?
c) calculate the pH at the equivalence point
25.00 mL of 0.1 M acetic acid are titrated with 0.05 M NaOH. Calculate the pH...
25.00 mL of 0.1 M acetic acid are titrated with 0.05 M NaOH.
Calculate the pH of the solution after addition of 50 mL of NaOH.
Ka(CH3COOH) = 1.8 x 10-5.
Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid , Ka...
Calculate the pH of a titration of 50.00 mL of 0.100 M
Phenylacetic acid , Ka = 4.9 x 10-5, with 0.100 M NaOH at the
following points:
SHOW ALL WORK IN NEAT DETAIL ON A SEPARATE PAGE. (Be sure to
write chemical equations and Ka or Kb expressions when needed.)
a. (4 Pts) Before any NaOH is added.
b. (4 Pts) After 18.7 mL of NaOH are added.
c. (4 Pts) After 25.00 mL of NaOH are added.
d....
25.00 mL 0.100 M CH3NH2 is titrated with 0.100 M HCl. Calculate the pH of this...
25.00 mL 0.100 M CH3NH2 is titrated with 0.100 M HCl. Calculate
the pH of this the titration solution after the addition of a) 12.5
mL and b) 25.00 mL of the titrant has been added. Based on these pH
values, select an appropriate indicator for the titration from
table at the end of lecture notes for Chapter 16.
Calculate the pH of the titration solution or 25.00 mL of 0.255 M nitrous acid nitrates...
Calculate the pH of the titration solution or 25.00 mL
of 0.255 M nitrous acid nitrates with 0.214 M KOH at the following
volumes of KOH:
A. 0.00 mL
B. 10.00 mL
C. Mid-point of titration
D. Equivalance point of titration
E. 5.00 mL past equivalence point of titration
Determine the pH during the titration of 73.5 mL of 0.429 M acetic acid (Ka =...
Determine the pH during the titration of 73.5
mL of 0.429 M acetic acid
(Ka = 1.8×10-5) by
0.429 M KOH at the following
points. (Assume the titration is done at 25 °C.)
(a) Before the addition of any KOH
(b) After the addition of 17.0 mL of
KOH
(c) At the half-equivalence point (the titration midpoint)
(d) At the equivalence point
(e) After the addition of 110 mL of
KOH
ADVERTISEMENT
ADVERTISEMENT
Latest Questions
- The marketing team at Stacey Collins Inc. is conducting research to determine the reaction of consumers...
- if expected return is 14%. the dividend is to grow at the rate of 8% it...
- You are the IT director at Big Ten University. As part of a training program, you...
- Critical Thinking The global marketplace has witnessed an increased pressure from customers and competitors in manufacturing...
- A cubic polynomial is of the form: f(x) = Ax^3 + Bx^2 + Cx + D...
- In Java The Problem In his book Irreligion, the mathematician John Allen Paulos tells an amusing...
- (EAC) Brandy's Place has decided to purchase a new branding machine. Brandy will buy one of...
ADVERTISEMENT