Question

How do the buffering capacity and ranges of the formate buffer (0.10M formic acid/formate buffer) compare...

How do the buffering capacity and ranges of the formate buffer (0.10M formic acid/formate buffer) compare to acetate buffer (0.10M 1:1 HAc and NaAc). Ka of formic acid: 1.8x10-4 and Ka of acetic acid: 1.8x10-5

Homework Answers

Answer #1

Solution :-

Using the given ka values we can find the pka values of the acids

Pka= - log ka

Pka of acetic acid = - log [1.8*10^-4] = 4.74

Pka of formic acid = - log[1.8*10^-4] = 3.74

Buffering capacity is the pH range where the buffer works effectively and restrict the sudden pH change when the strong acid or base added to the buffer solution.

Since the Pka of the formic acid is 3.74 therefore its pH range is at about pH 3- 4 where it can effectively works as buffer.

Since the Pka of the acetic acid is 4.74 therefore its pH range is about pH 4 - 5 where acetic acid acetate buffer can effectively acts as buffer.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
How can you increase the buffering capacity of a 0.1 M acetic acid/sodium acetate buffer? Explain...
How can you increase the buffering capacity of a 0.1 M acetic acid/sodium acetate buffer? Explain your answer!
A 1.00L volume of buffer is made with equal concentrations of sodium formate and formic acid...
A 1.00L volume of buffer is made with equal concentrations of sodium formate and formic acid of .35 M. Ka of formic acid is 1.8 x10^-4. a.) calculate the pH of this buffer b.) what does the pH become after the addition of .05 mol of HCl? (assume the volume remains 1.00L)
Formic acid (Ka= 1.7 x 10^-4) and sodium formate were used to prepare a buffer solution...
Formic acid (Ka= 1.7 x 10^-4) and sodium formate were used to prepare a buffer solution of pH 4.31. The concentration of the undissociated formic acid in this buffer solution was 0.80 mol/L. Under these conditions, the molar concentration of formate ion was this: please show work, answer is 1.4 mol/L
Using Henderson Hasselbach, calculate the pH of a buffer that has 0.65M acetic acid and 0.50...
Using Henderson Hasselbach, calculate the pH of a buffer that has 0.65M acetic acid and 0.50 M sodium acetate before and after 0.06 M nitric acid is added. Write the equilibrium and buffering reactions. Ka of HAc = 1.8 x 10 -5 (show all reactions and work, with units)
One beaker contains 10.0 mL of acetic acid/sodium acetate buffer at maximum buffer capacity (equal concentrations...
One beaker contains 10.0 mL of acetic acid/sodium acetate buffer at maximum buffer capacity (equal concentrations of acetic acid and sodium acetate), and another contains 10.0 mL of pure water. Calculate the hydronium ion concentration and the pH after the addition of 0.25 mL of 0.10 M HCl to each one. What accounts for the difference in the hydronium ion concentrations? Explain this based on equilibrium concepts; in other words, saying that “one solution is a buffer” is not sufficient....
A. What is the pH of a 1.0 L buffer made with 0.15 M formic acid...
A. What is the pH of a 1.0 L buffer made with 0.15 M formic acid (HCOOH, Ka = 1.8 x 10-4) and 0.25 M potassium formate, KHCOO? B. What is the pH of the buffer solution in question #13 after 0.096 moles of HCl are added to it?
1. A buffer is made by mixing 1.250 mol formic acid, HCOOH, with 0.750 mol sodium...
1. A buffer is made by mixing 1.250 mol formic acid, HCOOH, with 0.750 mol sodium formate, HCOONa in enough water for a total volume of 1.00L. The Ka of formic acid is 1.87 x 10-4 a. What is the pH of this buffer? b. If 0.075 mol HCl is added to this buffer, what is the pH of the resulting buffer? (assume no volume changes) c. If 0.055 mol NaOH is added to this buffer, what is the pH...
A buffer is made by dissolving 4.800 g of sodium formate (NaCHO2) in 100.00 mL of...
A buffer is made by dissolving 4.800 g of sodium formate (NaCHO2) in 100.00 mL of a 0.30 M solution of formic acid (HCHO2). The Ka of formic acid is 1.8 x 10-4. a) What is the pH of this buffer? b) Write two chemical equations showing how this buffer neutralizes added acid and added base. c) What mass of solid NaOH can be added to the solution before the pH rises above 4.60?
2) Two students want to prepare 2.0 L of a buffer solution which must be buffered...
2) Two students want to prepare 2.0 L of a buffer solution which must be buffered at a pH of 4.75. Student A wants to use acetic acid (CH3COOH, Ka = 1.8 x 10-5) and sodium acetate to prepare the buffer solution, while student B wants to use formic acid (HCOOH, Ka = 1.8 x 10-4) and sodium formate. Which student chose the better conjugate acid-base pair to prepare the buffer? Why? Explain the step-by- step procedure that the students...
How does the acid buffer capacity compare to the base buffer capacity for a buffer with...
How does the acid buffer capacity compare to the base buffer capacity for a buffer with 0.450M HCOOH and 0.550M HCOO-? A) BsubA =BsubB B) BsubA < BsubB C) BsubA > BsubB