Question

Before preparing the buffer solutions, you must determine the amounts of acetic acid (HC2H3O2, M.Wt.= 60.05...

Before preparing the buffer solutions, you must determine the amounts of acetic acid (HC2H3O2, M.Wt.= 60.05 g/mol) and sodium acetate (NaC2H3O2, M.Wt.= 82.03 g/mol) required. The Ka of HC2H3O2 is 1.8 X 10-5 (pKa = 4.74). Explain how you will prepare 100 mL of an HC2H3O2—NaC2H3O2 buffer starting with:

(1) 0.10 M HC2H3O2 and solid NaC2H3O2

(2) 0.30 M HC2H3O2 and solid NaC2H3O2

(3) 0.50 M HC2H3O2 and solid NaC2H3O2

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
Acetic acid (molecular weight = 60.05 g/mol) and sodium acetate (molecular weight = 82.03 g/mol) can...
Acetic acid (molecular weight = 60.05 g/mol) and sodium acetate (molecular weight = 82.03 g/mol) can form a buffer with an acidic pH. In a 500.0 mL volumetric flask, the following components were added together and mixed well, and then diluted to the 500.0 mL mark: 100.0 mL of 0.300 M acetic acid, 1.00 g of sodium acetate, and 0.16 g of solid NaOH (molecular weight = 40.00 g/mol). What is the final pH? The Ka value for acetic acid...
(You may use the Henderson-Hasselbalch equation to perform the following calculations, but you do not have...
(You may use the Henderson-Hasselbalch equation to perform the following calculations, but you do not have to.) The Ka of acetic acid is 1.8  10–5. Review your calculations with your TA or instructor before preparing the buffer solutions in lab. (Note: solid sodium acetate comes as a hydrate (NaC2H3O2·3H2O), and thus has a molar mass of 135.08 g/mol.) Buffer A: Calculate the mass of sodium acetate that must be added to make 100.0 mL of an acetic acid/acetate buffer...
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
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab...
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab was prepared using the following components: 3.46 g of NaC2H3O2∙3H2O (FW. 136 g/mol) 9.0 mL of 3.0 M HC2H3O2 55.0 mL of water If you take half of this solution and add 2 mL of 1.00 M NaOH to it, then what is the pH of this new solution?
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab...
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab was prepared using the following components: 3.46 g of NaC2H3O2∙3H2O (FW. 136 g/mol) 9.0 mL of 3.0 M HC2H3O2 55.0 mL of water If you take half of this solution and add 2 mL of 1.00 M NaOH to it, then what is the pH of this new solution?
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab...
An acetic acid/ sodium acetate buffer solution similar to the one you made in the lab was prepared using the following components: 3.46 g of NaC2H3O2∙3H2O (FW. 136 g/mol) 9.0 mL of 3.0 M HC2H3O2 55.0 mL of water If you take half of this solution and add 2 mL of 1.00 M HCl to it, then what is the pH of this new solution?
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....
You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30...
You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa). What will the pH of this solution be after the addition of 20.0 mL of 1.00 M HCl solution? Ka for acetic acid = 1.8 × 10–5
how many grams of acetic acid (mw 60.05 g/mol) and NaAcetate (MW 82.03 g/mol) are needed...
how many grams of acetic acid (mw 60.05 g/mol) and NaAcetate (MW 82.03 g/mol) are needed to prepare 1.0l of a 250 mM buffer of a pH 5.0 solution (pka 4.75)?
Acetic acid has a Ka of 1.8×10−5. Three acetic acid/acetate buffer solutions, A, B, and C,...
Acetic acid has a Ka of 1.8×10−5. Three acetic acid/acetate buffer solutions, A, B, and C, were made using varying concentrations: [acetic acid] ten times greater than [acetate], [acetate] ten times greater than [acetic acid], and [acetate]=[acetic acid]. Match each buffer to the expected pH. pH = 3.74 ; pH = 4.74 ; pH = 5.74 Part B: How many grams of dry NH4Cl need to be added to 2.30 L of a 0.600 M solution of ammonia, NH3, to...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT