Question

What is the pH of a solution obtained when 150.0 mL of 0.095M Boric acid has...

What is the pH of a solution obtained when 150.0 mL of 0.095M Boric acid has 20.0 mL of 0.087M NaOH added to it? Ka Boric acid = 5.8E-10.

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
A 0.25 M solution of boric acid is mixed with a 0.75 M solution of NaOH....
A 0.25 M solution of boric acid is mixed with a 0.75 M solution of NaOH. What is the pH of the solution if 7.5 mL of boric acid is mixed with 5 mL of NaOH?
What would the pH be of a solution obtained by mixing 0.2 mL 1 M HCl...
What would the pH be of a solution obtained by mixing 0.2 mL 1 M HCl with 10 mL distilled water? What would the pH be of a solution obtained by mixing 0.2 mL 1 M HCl with 10 nM NaOH (aq)? How do these values compare to the pH values you obtained when you added acid to your buffers?
1. calculate the PH for the resulting solution when 75.0ml of 2.15M acetic acid is added...
1. calculate the PH for the resulting solution when 75.0ml of 2.15M acetic acid is added to 80.0ml of 1.35M NaOH. Ka for acetic acid is 1.8*10^-5. 2. calculate the pH whrn 32.2 ml of 1.55 M NaOH is added to the final solution above. 3. calculate the pH when 45.0 ml of 2.23 M NaOH is added to the final solution in 2.
A 150.0 mL buffer solution containing 0.100 M hydrocyanic acid (HCN, Ka = 6.2 x 10-10)...
A 150.0 mL buffer solution containing 0.100 M hydrocyanic acid (HCN, Ka = 6.2 x 10-10) and 0.100 M potassium cyanide (KCN) has 30.0 mL of 0.120 M KOH added to it. What is the pH of the solution after the KOH has been added a. 8.73 b. 9.00 c. 9.21 d. 9.29 e. 9.42
Despite its formula, boric acid, H3BO3, is a monoprotic acid. A 25.00 mL sample of this...
Despite its formula, boric acid, H3BO3, is a monoprotic acid. A 25.00 mL sample of this acid required 15.66 mL of 0.1724 M NaOH to reach the equivalence point where the pH= 11.13. Determine the original concentration of boric acid and the equilibrium constant, Ka.
Despite its formula, boric acid, H3BO3, is a monoprotic acid. A 25.00 mL sample of this...
Despite its formula, boric acid, H3BO3, is a monoprotic acid. A 25.00 mL sample of this acid required 15.66 mL of 0.1724 M NaOH to reach the equivalence point where the pH= 11.13. Determine the original concentration of boric acid and the equilibrium constant, Ka.
Despite its formula, boric acid, H3BO3, is a monoprotic acid. A 25.00 mL sample of this...
Despite its formula, boric acid, H3BO3, is a monoprotic acid. A 25.00 mL sample of this acid required 15.66 mL of 0.1724 M NaOH to reach the equivalence point where the pH=11.13. Determine the original concentration of boric acid and the equilibrium constant, Ka.
What is the pH when 5.0 g of sodium acetate, NaC2H3O2, is dissolved in 150.0 mL...
What is the pH when 5.0 g of sodium acetate, NaC2H3O2, is dissolved in 150.0 mL of water? (The Ka of acetic acid, HC2H3O2, is 1.8×10−5.)
A 25.0 mL sample of a 0.115 M solution of acetic acid is titrated with a...
A 25.0 mL sample of a 0.115 M solution of acetic acid is titrated with a 0.144 M solution of NaOH. Calculate the pH of the titration mixture after 10.0, 20.0, and 30.0 mL of base have been added. (The Ka for acetic acid is 1.76 x 10^-5). 10.0 mL of base = 20.0 mL of base = 30.0 mL of base =
A buffer solution contains 0.54 mol of boric acid (H3BO3) and 0.89 mol of sodium dihydrogen...
A buffer solution contains 0.54 mol of boric acid (H3BO3) and 0.89 mol of sodium dihydrogen borate (NaH2BO3) in 4.80 L. The Ka of boric acid (H3BO3) is Ka = 5.8e-10. (a) What is the pH of this buffer? pH =   (b) What is the pH of the buffer after the addition of 0.18 mol of NaOH? (assume no volume change) pH =   (c) What is the pH of the original buffer after the addition of 0.12 mol of HI?...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT