Question

The acid ionization constant Ka of benzoic acid (C6H5COOH; HA) is 6.5 ⨯ 10-5. (1) Calculate...

The acid ionization constant Ka of benzoic acid (C6H5COOH; HA) is 6.5 ⨯ 10-5.
(1) Calculate the pH of 2.0L of 0.20 M benzoic acid solution.
(2) After adding 8.0 g of NaOH (molar mass: 40 g/mol) to 2.0 L of a 0.20 M benzoic acid solution,
Calculate the pH.
(3) The solution (2) made above is a buffer solution. 2.0 L of 0.1 M NaOH aqueous solution was added to this solution.
After adding more, calculate the pH of the solution.

Engineering   Chemical-Engineering   
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
Starting with 0.250L of a buffer solution containing 0.250 M benzoic acid (C6H5COOH) and 0.20 M...
Starting with 0.250L of a buffer solution containing 0.250 M benzoic acid (C6H5COOH) and 0.20 M sodium benzoate (C6H5COONa), what will the pH of the solution be after the addition of 25.0 mL of 0.100M HCl? (Ka (C6H5COOH) = 6.5 x 10-5) Please solve in detail
Find the pH of a 0.380 M aqueous benzoic acid solution. For benzoic acid, Ka=6.5⋅10−5.
Find the pH of a 0.380 M aqueous benzoic acid solution. For benzoic acid, Ka=6.5⋅10−5.
Calculate the percent ionization of a 0.484 M solution of benzoic acid, C6H5COOH. % Ionization =...
Calculate the percent ionization of a 0.484 M solution of benzoic acid, C6H5COOH. % Ionization = ___%
Calculate the pH when 15.0 mL of 0.20 M benzoic acid (HC7H5O2, Ka = 6.5 ×10–5)...
Calculate the pH when 15.0 mL of 0.20 M benzoic acid (HC7H5O2, Ka = 6.5 ×10–5) is titrated with 20.0 mL of 0.15 M sodium hydroxide (NaOH). The answer is 8.56 but I do not know how to get to that point.
４０．2.20 L of a buffer solution that is 0.190 M in benzoic acid, C6H5COOH, and 0.340...
４０．2.20 L of a buffer solution that is 0.190 M in benzoic acid, C6H5COOH, and 0.340 M in sodium benzoate, C6H5CONa, are diluted to 4.40 L with distilled water. What is the pH of the buffer? Ka of C6H5COOH = 6.4 ✕ 10-5.
You are given a 30.0mL sample of 0.20M C6H5COOH(aq) (benzoic acid). Ka for benzoic acid is...
You are given a 30.0mL sample of 0.20M C6H5COOH(aq) (benzoic acid). Ka for benzoic acid is 6.5x10-5. b) what is the pH after the addition of 15.0mL of 0.30M KOH(aq)? c)if you start with a new 30.0mL sample of 0.20M C6H5COOH(aq), what volume of 0.20M NaOH(aq) is required to reach the halfway to the equivalence point?
A buffer solution is prepared by adding 0.5 moles of benzoic acid (C6H5COOH, Ka = 6.3...
A buffer solution is prepared by adding 0.5 moles of benzoic acid (C6H5COOH, Ka = 6.3 x 10-5) and 0.5 moles of potassium benzoate (C6H5COOK) to enough water to make a 1L solution. How many grams of barium hydroxide is needed to shift the pH of this solution to 6? (This question was previously answered. The answer is not 19.4
A buffer solution is prepared by mixing 20.0mL of 0.032M benzoic acid C6H5COOH soultion with 25.0mL...
A buffer solution is prepared by mixing 20.0mL of 0.032M benzoic acid C6H5COOH soultion with 25.0mL of 0.022 M NaC6H5COO. what is the pH of the buffer produced? (Ka of benzoic acid = 6.2*10^-5)
Benzoic acid, C6H5CO2H, is a weak acid (Ka=6.3x10^-5). Calculate the initial concentration (in M) of benzoic...
Benzoic acid, C6H5CO2H, is a weak acid (Ka=6.3x10^-5). Calculate the initial concentration (in M) of benzoic acid that is required to produce an aqueous solution of benzoic acid that has a pH of 2.54
Question 1: We place 0.895 mol of a weak acid, HA, and 13.0 g of NaOH...
Question 1: We place 0.895 mol of a weak acid, HA, and 13.0 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.01 . Calculate the ionization constant, Kb, of A-(aq). Question 2: HA is a weak acid with a pKa value of 3.76 . What is the pH of a buffer solution that is 0.359 M in HA and 0.844 M in NaA? What is its pH after the...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT