Question

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)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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...
Two buffers are prepared by adding an equal number of moles of formic acid (HCOOH) and...
Two buffers are prepared by adding an equal number of moles of formic acid (HCOOH) and sodium formate (HCOONa) to enough water to make 1.00 L of solution. Buffer A is prepared using 1.00 mol each of formic acid and sodium formate. Buffer B is prepared by using 0.010 mol of each. (Ka(HCOOH)=1.8×10−4.) Calculate the change in pH for each buffer upon the addition of 10 mL of 1.00M HCl.
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?
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
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?
You have 1 M solutions of formic acid and sodium formate. Calculate the volume of sodium...
You have 1 M solutions of formic acid and sodium formate. Calculate the volume of sodium formate required to make 1 liter of a solution with a pH of 4.1 in which the concentration of formic acid is 0.15 M. The pKa of formic acid is 3.75.
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 buffer solution contains 0.27 mol of ascorbic acid (HC6H7O6) and 0.76 mol of sodium ascorbate...
A buffer solution contains 0.27 mol of ascorbic acid (HC6H7O6) and 0.76 mol of sodium ascorbate (NaC6H7O6) in 8.20 L. The Ka of ascorbic acid (HC6H7O6) is Ka = 8e-05. (a) What is the pH of this buffer? pH =    (b) What is the pH of the buffer after the addition of 0.08 mol of NaOH? (assume no volume change) pH =   (c) What is the pH of the original buffer after the addition of 0.39 mol of HI? (assume...
A buffer solution contains 0.56 mol of ascorbic acid (HC6H7O6) and 0.54 mol of sodium ascorbate...
A buffer solution contains 0.56 mol of ascorbic acid (HC6H7O6) and 0.54 mol of sodium ascorbate (NaC6H7O6) in 5.70 L. The Ka of ascorbic acid (HC6H7O6) is Ka = 8e-05. (a) What is the pH of this buffer? (b) What is the pH of the buffer after the addition of 0.10 mol of NaOH? (assume no volume change) (c) What is the pH of the original buffer after the addition of 0.30 mol of HI? (assume no volume change)
Calculate the pH of 0.379 L of a 0.25 M acetic acid - 0.34 M sodium...
Calculate the pH of 0.379 L of a 0.25 M acetic acid - 0.34 M sodium acetate buffer before and after the addition of 0.0058 mol of KOH. Assume that the volume remains constant. (Ka of acitic acid is 1.8⋅10−5)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT