Question

A. If the pH of a solution is 1.2, find [OH-] B. Find the pH of...

A. If the pH of a solution is 1.2, find [OH-]

B. Find the pH of a 0.058M solution of acetic acid (Ka= 1.8x10^-5)

C. Find the pH of a 0.02M solution of HF (Ka= 6.2x10^-4)

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. The hydroxide ion concentration of an aqueous solution of 0.538 M acetic acid is [OH-]...
a. The hydroxide ion concentration of an aqueous solution of 0.538 M acetic acid is [OH-] = ______ M. b. Calculate the pH of a 0.538 M aqueous solution of hydrofluoric acid (HF, Ka = 7.2×10-4).
A.) Find the pH of a 0.338 M NaF solution. (The Ka of hydrofluoric acid, HF,...
A.) Find the pH of a 0.338 M NaF solution. (The Ka of hydrofluoric acid, HF, is 3.5×10?4.) B.) Determine the [OH?] of a 0.30 M solution of NaHCO3. and Determine the pH of this solution. C.)Find the [OH?] of a 0.46 M  methylamine (CH3NH2) solution. (The value of Kb for methylamine (CH3NH2) is 4.4×10?4.) include units D.) Find the pH of a 0.46? M  methylamine (CH3NH2) solution.
A). Calculate [H3O+], [OH-], pH and pOH for 0.035M solution of Ca(OH)2 B). Calculate the pH...
A). Calculate [H3O+], [OH-], pH and pOH for 0.035M solution of Ca(OH)2 B). Calculate the pH of a 0.028M solution of benzoic acid Ka= 6.5 x 10-5
Calculate the pH of a solution that is 0.125M acetic acid and 0.150M sodium acetate. Calculate...
Calculate the pH of a solution that is 0.125M acetic acid and 0.150M sodium acetate. Calculate the pH if a 50.0mL of 0.150M nitric acid is added to 275mL of the solution of acetic acid and sodium acetate.     Ka=1.8x10-5
A.) Find the percent ionization of a 0.120 M solution of a weak monoprotic acid having...
A.) Find the percent ionization of a 0.120 M solution of a weak monoprotic acid having Ka= 1.2×10−3. B.)Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 0.10. C.) Find the percent ionization of a 0.120 M solution of a weak monoprotic acid having Ka= 0.10. D.) Find the pH of a 0.013 M solution of HF. (The value of Ka for HF is 3.5×10−4.)
A.) What is the pH of a 500mL sample of 0.450M acetic acid solution, given a...
A.) What is the pH of a 500mL sample of 0.450M acetic acid solution, given a Ka=1.8x10^-5? B.) What is the pH after 20.000ml of 0.8M NaOH are added? C.) What is the pH after 140.625mL of 0.8M NaOH are added?
5 acetic acid solutions, 0.10M, 0.50M,1.00M, 3.00M, 6.00M. (PL5) Calculate pH for a solution which has...
5 acetic acid solutions, 0.10M, 0.50M,1.00M, 3.00M, 6.00M. (PL5) Calculate pH for a solution which has [H+] = 0.765M. (PL6) Calculate [H+] for a solution with pH=3.65 A1) Calculate percent dissociation of 5 solutions. Show your work clearly for 0.10M solution. (A2) Draw a graph of percent dissociation vs. concentration. Label everything. (Q1) What is the theoretical pH of 1.00M acetic acid (Ka = 1.8x10^-5) (Q2) What is the theoretical percent dissociation for Q1? (Q3) What is the theoretical pH...
-What concentration of ammonia is required to have a solution with a pH of 11.36? Kb...
-What concentration of ammonia is required to have a solution with a pH of 11.36? Kb = 1.8x10-5 -What is the pH of a 0.014M solution of NaF? Ka for HF = 6.8 x 10-4 -What is the other product of the aqueous base dissociation reaction of ethyl amine? C2H5NH2(aq) + H2O(l) ⇌ ________ + OH-(aq)
calculate the ph of a solution containing 0.15m acetic acid and .25M sodium acetate for acetic...
calculate the ph of a solution containing 0.15m acetic acid and .25M sodium acetate for acetic acid ka=1.8x10^-5 if .0010 mol HCL is added to 1.0 L buffer as in part a calculate the final ph of the buffer. show work with ICE
1.Calculate the pH of an 0.0452 M Ba(OH)2 solution at 298 K 2. calculate the pH...
1.Calculate the pH of an 0.0452 M Ba(OH)2 solution at 298 K 2. calculate the pH of an 0.229 M HNO2 solution at 298 K. Assume ka for HNO2 is 4.5x10^-4 3.Calculate the pH of an 0.292 M NH3 solution at 298 K. assume the Kb for NH3 is 1.8x10^-5
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT