Question

A 0.100 mol/kg solution of the acid HX is found to have 0.00055 mol/kg of H3O+....

A 0.100 mol/kg solution of the acid HX is found to have 0.00055 mol/kg of H3O+. Find the Ka for this acid.

Engineering   Chemical-Engineering   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

SOLUTION :

INITIAL CONCENTRATION OF [HX] = X M = 0.1 M

[ H3O+] = 0.00055 M

REACTION :
HX + H2O    H3O+ +

INITIALLY 0.1 M 0 M 0 M

CHANGE - X M X M    X M

EQUILIBRIUM (0.1 -X) M X M X M

  

FOR THIS WEAK ACID REACTION

M

SUMMARY :

M

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. Find the pH of a 0.100 M solution of a weak monoprotic acid having Ka=...
a. Find the pH of a 0.100 M solution of a weak monoprotic acid having Ka= 1.1×10−5. b.Find the percent dissociation of this solution. c. Find the pH of a 0.100 M solution of a weak monoprotic acid having Ka= 1.8×10−3 d. Find the percent dissociation of this solution. e.Find the pH of a 0.100 M solution of a weak monoprotic acid having Ka= 0.16. f.Find the percent dissociation of this solution.
What is the pH of a buffer solution (0.100 L containing 0.166 mol/L pyruvic acid (Ka...
What is the pH of a buffer solution (0.100 L containing 0.166 mol/L pyruvic acid (Ka = 4.1x10-3)) and 0.117 mol L-1 sodium pyruvate before and after the addition of 0.010 L of 0.10 mol/L HCl?
A 0.10 mol/L solution of a weak acid was found to be 4.0% dissociated. Calculate Ka....
A 0.10 mol/L solution of a weak acid was found to be 4.0% dissociated. Calculate Ka.
Find the H3O+ concentration of a 0.210 M hypochlorous acid solution (whose acid dissociation constant is...
Find the H3O+ concentration of a 0.210 M hypochlorous acid solution (whose acid dissociation constant is Ka=2.9×10−8).
1. When 50.00 mL of 0.100 M NaOH reacts with 25.00 mL of 0.300 M HX,...
1. When 50.00 mL of 0.100 M NaOH reacts with 25.00 mL of 0.300 M HX, a weak monoprotic acid, the pH of the resulting solution is 3.74. Calculate the Ka of the acid. 2. Will the equivalence point of ammonia plus HCl be higher, lower, or equal to 7? Explain.
Find the H3O+H3O+ concentration of a 0.220 MM  hypochlorous acid solution (whose acid dissociation constant is Ka=2.9×10−8Ka=2.9×10−8)....
Find the H3O+H3O+ concentration of a 0.220 MM  hypochlorous acid solution (whose acid dissociation constant is Ka=2.9×10−8Ka=2.9×10−8). Express the concentration to two significant figures.
Calculate the Ka for an unknown monoprotic acid HX, given that a solution of 0.49 M...
Calculate the Ka for an unknown monoprotic acid HX, given that a solution of 0.49 M LiX has a pH of 8.90.
When 25.0 mL of 0.100 M NaOH was added to 50.0 mL of a 0.100 M...
When 25.0 mL of 0.100 M NaOH was added to 50.0 mL of a 0.100 M solution of a weak acid, HX, the pH of the mixture reached a value of 3.56. What is the value of Ka for the weak acid?
Calculate the Ka, for an unknown acid HX, given that a 0.25M salt solution NaX has...
Calculate the Ka, for an unknown acid HX, given that a 0.25M salt solution NaX has a pH of 8.48 answer: 2.7x10-4
1. A 0.735 M solution of a weak acid is 12.5% dissociated. (a)Calculate the [H3O+], pH,...
1. A 0.735 M solution of a weak acid is 12.5% dissociated. (a)Calculate the [H3O+], pH, [OH -], and pOH of the solution. (b) calculate the ka of the acid
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT