Question
In: Chemistry
A 1.00 L buffer solution is 0.150 M CH3COOH (pKa = 4.74 ) and 0.200 M...
A 1.00 L buffer solution is 0.150 M CH3COOH (pKa = 4.74 ) and 0.200 M NaCH3COO. What is the pH of this buffer solution after 0.0500 mol KOH are added?
Solutions
Expert Solution
no of moles of CH3COOH = molarity*volume in L
= 0.15*1 = 0.15 moles
no of moles of CH3COONa = molarity*volume in L
= 0.2*1 = 0.2 moles
PH = PKa + log[CH3COONa]/[CH3COOH]
= 4.74 + log0.2/0.15
= 4.74 + 0.1249 = 4.8649
By the addition of 0.05 moles of KOH
no of moles of CH3COOH = 0.15-0.05 = 0.1 moles
no of moles of CH3COONa = 0.2+0.05 = 0.25 moles
PH = PKa + log[CH3COONa]/[CH3COOH]
= 4.74 + log0.25/0.1
= 4.74 + 0.3979 = 5.1379
queen_honey_blossom answered 1 year agoRelated Solutions
Given 1.00 L of a solution that is 0.200 M HC3H5O2 and 0.250 M KC3H5O2, a.)...
Given 1.00 L of a solution that is 0.200 M HC3H5O2 and 0.250 M
KC3H5O2,
a.) What is the buffer capacity of the solution? That is, how
many millimoles of strong acid or strong base can be added to the
solution before any significant change in pH occur?
b.) Over what pH range will this
solution be an effective buffer?
Calculate the pH of 1.00 L of a buffer 0.98 M CH3COONa/0.92 M CH3COOH before and...
Calculate the pH of 1.00 L of a buffer 0.98 M CH3COONa/0.92 M
CH3COOH before and after the addition of the following species
A. pH of starting buffer:
B. pH after addition if 0.040 mol NaOH:
C. pH after further addition if 0.101 mol HCl
Calculate the pH of 1.00 L of the buffer 1.06 M CH3COONa/1.09 M CH3COOH before and...
Calculate the pH of 1.00 L of the buffer 1.06
M
CH3COONa/1.09
M CH3COOH before and
after the addition of the following species. (Assume there is no
change in volume.)
(a) pH of starting buffer:
(b) pH after addition of 0.060 mol NaOH:
(c) pH after further addition of 0.109 mol
HCl:
Calculate the pH of an aqueous solution that is both 1.00 M CH3COOH and 1.00 M...
Calculate the pH of an aqueous solution that is both 1.00 M
CH3COOH and 1.00 M CH3COONa. A
buffer solution is 0.24 M NH3 and 0.20 M NH4Cl. (a) What is the pH
of this buffer? (b) If 0.0050 mol
NaOH is added to 0.500 L of this solution, what will be the pH?
Given a solution of 0.125 M CH3COOH (aq) and a solution of 0.150 M NaCH3COO (aq),...
Given a solution of 0.125 M CH3COOH (aq) and
a solution of 0.150 M NaCH3COO (aq), how would
you prepare 100.0 mL of a buffer solution with a pH of 4.400?
pKa = 4.740 for CH3COOH
(aq).
Select one:
a. Mix 68.6 mL of the CH3COOH (aq) with 31.4
mL of the NaCH3COO (aq)
b. Mix 27.6 mL of the CH3COOH (aq) with 72.4
mL of the NaCH3COO (aq)
c. Mix 72.4 mL of the CH3COOH (aq) with 27.6
mL...
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M KOH solution....
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M
KOH solution. Calculate the pH after the following additions of the
KOH solution: (a) 0.0 mL, (b) 5.0 mL, (c) 10.0 mL, (d) 12.5 mL, (e)
15.0 mL. (25 points)
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M KOH solution....
A 25.0 mL solution of 0.100 M CH3COOH is titrated with a 0.200 M
KOH solution. Calculate the pH after the following additions of the
KOH solution: (a) 0.0 mL, (b) 5.0 mL, (c) 10.0 mL, (d) 12.5 mL, (e)
15.0 mL. (25 points)
Calculate the theoretical buffer capability of 0.1 M CH3COOH/CH3COONa buffer at pH=4.74 and pH=6 (I don't...
Calculate the theoretical buffer capability of 0.1 M
CH3COOH/CH3COONa buffer at pH=4.74 and pH=6 (I don't know does the
pH value affect so I provide it anyway)
pKa of acetic acid is 4.74
To calculate the buffer capability, meansure the change by
adding 0.5mL of 1.0M HCl and by adding 0.5mL NaOH to 10 mL of
buffer, the capability is then the determined as the molarity of
the HCl or NaOH added to the buffer divided by the change of...
A 35. mL of a 0.045 M solution of acetic acid, pKa = 4.74, is titrated...
A 35. mL of a 0.045 M solution of acetic acid, pKa = 4.74, is
titrated with a 0.068 M solution of NaOH. What is the hydroxide ion
concentration of the resulting solution after 30.0 mL of NaOH is
added?
Consider the titration of a 30.0 mL sample of 0.150 M CH3COOH (Ka=1.8×10−5) with 0.200 M...
Consider the titration of a 30.0 mL sample of 0.150 M CH3COOH
(Ka=1.8×10−5) with 0.200 M NaOH. Determine each quantity: Part A:
What is the volume of base required to reach the equivalence point?
Express your answer using one decimal place. Part B: What is the pH
after 10.0 mL of base have been added? Express your answer using
two decimal places. Part C What is the pH at the equivalence point?
Express your answer using two decimal places. Part...
ADVERTISEMENT
ADVERTISEMENT
Latest Questions
- A pension fund manager is considering three mutual funds. The first is a stock fund, the...
- Compute the cost of not taking the following cash discounts. (Use a 360-day year. Do not...
- During his project presentation, Bob falls sick and performs poorly. However, his colleague, Dan, concludes that...
- A sample human input file that contains test values that a human would enter on the...
- A solution is prepared by dissolving 15 ml of methanol in 150.0 ml water at 25...
- Consider a newlywed who is planning a wedding anniversary gift of a trip to Canada for...
- We are evaluating a project that costs $868,000, has a life of eight years, and has...
ADVERTISEMENT