Question

A student has 25.0 ml of 0.45 M sodium lactate and 0.50 M lactic acid buffer....

A student has 25.0 ml of 0.45 M sodium lactate and 0.50 M lactic acid buffer. what is the minimum volume of 0.62 m NaOH that will destroy the buffer?

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
Calculate the pH of a buffer solution prepared by mixing 50.0 mL of 1.00 M lactic...
Calculate the pH of a buffer solution prepared by mixing 50.0 mL of 1.00 M lactic acid and 25.0 mL of 0.75 M sodium lactate.
Calculate the pH of a buffer that is 0.13 M in lactic acid and 0.11 M...
Calculate the pH of a buffer that is 0.13 M in lactic acid and 0.11 M in sodium lactate. Express your answer using two decimal places. Calculate the pH of a buffer formed by mixing 85 mL of 0.12 M lactic acid with 95 mL of 0.16 M sodium lactate. Express your answer using two decimal places.
25.0 ml of hydrochloric acid (4.00M) was added to 550.0 ml of a 0.500 M sodium...
25.0 ml of hydrochloric acid (4.00M) was added to 550.0 ml of a 0.500 M sodium lactate solution. What is the pH of the resulting solution? The pKa for lactic acid is 3.86.
A student needs to prepare a lactic acid buffer at a pH of 4.85. The student...
A student needs to prepare a lactic acid buffer at a pH of 4.85. The student has available lactic acid (pKa = 4.20), a 0.830 M KOH solution and a 0.830 M HCl solution. Will the student need to add KOH or HCl to the lactic acid in order to prepare the buffer? Also Calculate the volume (in mL) of the solution that should be added to 3.166 g of lactic acid (FW 122.12 g/mol, pKa = 4.20) to give...
1.A lactic acid/lactate ion buffer solution contains 0.43 M HC3H5O3 and 0.62 M C3H5O3−, respectively. The...
1.A lactic acid/lactate ion buffer solution contains 0.43 M HC3H5O3 and 0.62 M C3H5O3−, respectively. The Ka value of lactic acid is 1.4×10−4. Calculate the pH of this buffer. 2. Enter the formula of the conjugate base for the acid H2PO4−. Enter the formula of the conjugate base for the acid CH3−NH3+. Enter the formula of the conjugate base for the acid HSO4−. Enter the formula of the conjugate base for the acid HNO2. Enter the formula of the conjugate...
The saponification produces sodium lactate (and not lactic acid) as the final product. What organic product...
The saponification produces sodium lactate (and not lactic acid) as the final product. What organic product was formed after the solution was acidified with HCl?
b) (2 points) Why does saponification produce sodium lactate (and not lactic acid) as the final product? Hint: Examine the acid-base reaction step in the saponification mechanism. The pKa of lactic acid is 3.85 and the pKa of methanol is 16.
A solution of equal concentrations of lactic acid and sodium lactate was found to have pH=3.85....
A solution of equal concentrations of lactic acid and sodium lactate was found to have pH=3.85. (a) What are the values of pKa, and Ka of lactic acid? (b) What would the pH be if the acid had twice the concentration of the salt? (c) Plot a graph showing a mole fraction of Lactic acid and Lactate with respect to pH. (You can use excel or any software of your choice). (d)There are many organic acids and bases in our...
a. How many grams of sodium lactate, NaC3H5O3 should be added to 1.00L of 0.150M lactic...
a. How many grams of sodium lactate, NaC3H5O3 should be added to 1.00L of 0.150M lactic acid, HC3H5O3 to form a buffer solution with a pH of 3.90? (Ka= 1.4 x 10^-4 for lactic acid) b. What is the pH of the buffer solution containing 0.10moles of acetic acid and 0.13moles of sodium acetate in 1.0L after adding 0.02 moles of KOH? c. What will the pH be if 0.15mol HA (pKa= 2.00) and 0.27 mole A- are mixed together...
A student performs the following experiment: 25.0 mL of 0.1 M acetic acid is titrated to...
A student performs the following experiment: 25.0 mL of 0.1 M acetic acid is titrated to the equivalence point with 25.0 mL of 0.1 M NaOH. Calculate the pH at the equivalence point. The equilibrium constant Ka for acetic acid is 1.8*10^-5. Compare this value with the experimental value. Experimental value for acetic acid is pH = 8.8 and volume of base = 24 mL at equivalence point.
A buffer composed of 0.50 mol acetic acid (HC2H3O2) and 0.50 mol sodium acetate (Na+C2H3O2-) is...
A buffer composed of 0.50 mol acetic acid (HC2H3O2) and 0.50 mol sodium acetate (Na+C2H3O2-) is diluted to a volume of 1.0 liter. The pH of the buffer is 4.74. How many moles of NaOH must be added to the buffer to raise its pH to 5.74? A. 0.25 mol B. 0.41 mol C. 0.50 mol D. 0.55 mol E. 0.49 mol
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT