Question

Determine the pH and the complete solution composition of the following system (added to 1 liter...

Determine the pH and the complete solution composition of the following system (added to 1 liter of pure water), based on the governing equations. Show all the simplifying assumptions you make, then solve the system of equations based on those assumptions:

0.01 M benzoic acid, HBz, and 0.1 M NaCl in water

Homework Answers

Answer #1

Concentration of HBz = 0.01 M

Concentration of NaCl in water = 0.1 M

Dissociation of Benzoic acid in water is given as -

C6H5COOH <===> C6H5COO- + H+ Ka = 6.46 x 10-5

Lets take 1 L of HBz and 1 L of NaCl is poured into 1 L of pure water,

[HBz] = (1 x 0.01) / 3 = 0.0033 M

[NaCl] = (1 x 0.1) / 3 = 0.0333 M

Now HBz will react with NaCl present to give -

C6H5COOH + NaCl <===> C6H5COONa + HCl

0.01 0.1 0 0

0 0.99 0.01 0.01

New composition of solution,

[HBz] = 0

[NaCl] = 0.99 / 3 = 0.33 M

pH = -log [H+]

pH = -log [0.01]

pH = 2

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
A solution of 10-3-mole of sodium propionate (CH3CH2COONa) is added to 1 liter of distilled water....
A solution of 10-3-mole of sodium propionate (CH3CH2COONa) is added to 1 liter of distilled water. If the pKa = 4.87 for propionic acid, what the solution pH? Solve the appropriate equations analytically and graphically and compare the results. Also, using the same graph determine the pH if a 10-3-mole of propionic acid (CH3CH2COOH) were added instead of the sodium propionate. Step by step explanations would be appreciated. Thanks!
2. The composition of an aqueous solution is 0.1M acetic acid + 0.2M sodium acetate. (a)...
2. The composition of an aqueous solution is 0.1M acetic acid + 0.2M sodium acetate. (a) Calculate the pH of the solution (pKa of acetic acid is 4.74). 3 pts. (b) What would the pH be if 2 ml of 10M NaOH was added to 1 liter of this solution? 4 pts. (c). By comparison, what would the pH be if the same amount of NaOH were added to 1 L of pure water? 3 pts.
The following quantities of salts were added to water to make a 1-liter solution: 1X10-2 moles...
The following quantities of salts were added to water to make a 1-liter solution: 1X10-2 moles NaCl, 2X10-2 moles CaCl2, 4.166 grams BaCl2 1. What is the ionic strength of the solution? 2. What is the activity of the Cl species?
What is the pH of a 0.15 M solution of HClO? Ka for HClO = 3.5...
What is the pH of a 0.15 M solution of HClO? Ka for HClO = 3.5 x 10-8   The value of Ka for the weak acid Benzoic acid (C6H6COOH) is 1.5 × 10-5. What are the equilibrium concentrations of all species if 1.50 g of Benzoic acid is dissolved in enough water to make a 250.0 mL solution? What is the pH of the solution? Ammonium ion is the conjugate acid of Ammonia.   What is the pH of a 0.25...
PART A: Determine the pH of an HF solution of each of the following concentrations. 0.260M...
PART A: Determine the pH of an HF solution of each of the following concentrations. 0.260M 4.70×10−2 M 2.30×10−2 M In which cases can you not make the simplifying assumption that x is small? (choose one of the below options) only in (a) only in (b) in (a) and (b) in (b) and (c) PART B: A 8.0×10−2 M solution of a monoprotic acid has a percent dissociation of 0.60%. Determine the acid ionization constant (Ka) for the acid.
you select the amino acid Cysteine (pKa=8.2) and dissolve 0.1 moles in 1 liter of water...
you select the amino acid Cysteine (pKa=8.2) and dissolve 0.1 moles in 1 liter of water in order to make a buffer solution. You then adjust the pH to 7.2, but then accidentally add 0.03 moles of HCl to the solution. is the solution still a good buffer? Please help me understand how to use the number of moles added to solve the problem. I can't seem to understand how the amount of moles added relates to the amino acid's...
Calculate the pH of the solution when the following substances are added together ​ 20 mL...
Calculate the pH of the solution when the following substances are added together ​ 20 mL of 0.1M NaOH and 8 mL of 0.25 M Sodium Acetate 20 mL of 0.1 M NaOH and 8 mL of 0.25 M Acetic acid
Carbonic acid is a weak, monoprotic acid with a pKa of 6.38. Calculate the following pH...
Carbonic acid is a weak, monoprotic acid with a pKa of 6.38. Calculate the following pH values. For any buffer solution, assume the assumptions will be valid and simplify by using the Henderson-Hasselbalch equation. Show your work. Attach additional pages if necessary. a. Determine the pH of 25 mL of a 0.10 M solution of carbonic acid. b. Determine the pH after 20.0 mL of a 0.10 M NaOH solution is added to the 25 mL of 0.10 M carbonic...
Determine the pH of an HF solution of each of the following concentrations. In which cases...
Determine the pH of an HF solution of each of the following concentrations. In which cases can you not make the simplifying assumption that x is small? (Ka for HF is 6.8×10−4.) a) 0.300 M b) 4.70×10−2 M c) 2.60×10−2 M d) In which cases can you not make the simplifying assumption that x is small? only in (a) only in (b) in (a) and (b) in (b) and (c)
Determine the pH of an HF solution of each of the following concentrations. a. .290 M...
Determine the pH of an HF solution of each of the following concentrations. a. .290 M b. 5.20 x 10^-2 M c. 2.10 x 10^-2 M d. in which cases can you not make simplifying assumption that x i small
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT