HomeworkLib
Question

Hello, Could you please provide a detail explanation as to how to find each of these...

Hello,

Could you please provide a detail explanation as to how to find each of these steps.

The ionization constant of a very weak acid, HA, is 5.2×10-9. Calculate the equilibrium concentrations of H3O+, A-, and HA in a 0.040 M solution of the acid.

Determine the concentrations of all species at equilibrium and the solution pH.

[H3O+] =  mol/L

[A-] =  mol/L

[HA] =  mol/L

pH =

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

Ka for HA= 5.2 x 10 9 H3o+ НА + H2O оочом + 4- нро - Х (ооцо-х) - л + ka- [Hot] [RO] THAJ xxx = 512 X10-9 oo Чо- х? = зох)о-1

0 0
Add a comment
Know the answer?
Add Answer to:
Hello, Could you please provide a detail explanation as to how to find each of these...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • The ionization constant of a very weak acid, HA, is 8.8x10-9. Calculate the equilibrium concentrations of...

    The ionization constant of a very weak acid, HA, is 8.8x10-9. Calculate the equilibrium concentrations of H2O, A', and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H30]= mol/L [A] = moll mol/L [HA] = pH =

  • How do you calculate the pH of a solution containing a weak acid or a weak...

    How do you calculate the pH of a solution containing a weak acid or a weak base? Please write down the general formula for finding the H3O+ ion concentrations in case of a weak acid Please explain the common-ion effect in terms of Le Châtelier. You might want to use the general chemical equation for an acid ionization HA + H2O ↔ A- + H3O+ to help you explain the phenomenon. How do you calculate the degree of ionization? Please...

  • please help me please i dont have questions remaining anymore A solution is prepared by dissolving 0.060 mol of iodoacet...

    please help me please i dont have questions remaining anymore A solution is prepared by dissolving 0.060 mol of iodoacetic acid (Kg = 6.68x10-4) and 0.040 mol of sodium iodoacetate in water to a total solution volume of 1.00 L. First, calculate a pH for the solution by assuming that the concentrations of ICH CO2H and ICH CO2 are equal to the formal concentrations of the substances dissolved. Submit Answer Tries 0/5 Next, calculate the pH for the solution based...

  • Question 1 HA is a weak acid. Its ionization constant, Ky, is 5.1 x 10-13. Calculate...

    Question 1 HA is a weak acid. Its ionization constant, Ky, is 5.1 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.053 M. Question 2 We place 0.134 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.18. Calculate the ionization contant, K. of HA. Question 3 We place 0.577 mol of a weak acid, HA, and 13.6 g of...

  • Question 1    :   HA is a weak acid. Its ionization constant, Ka, is 1.2 x 10-13....

    Question 1    :   HA is a weak acid. Its ionization constant, Ka, is 1.2 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.075 M.   Question 2    :   We place 0.143 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.28 . Calculate the ionization contant, Ka, of HA.   Question 3    :   We place 0.661 mol of a weak acid, HA,...

  • - Given this concentration n ratio what is the pH (show work), Ka and percent ionization...

    - Given this concentration n ratio what is the pH (show work), Ka and percent ionization of this species ( HA+H2O← → A- + H3O+ , acid. Initial concentration: 0.01 mol/L) HA: 9.77x10^-3 mol/L H2O: 55.6 mol/L A- : 2.34x10^-4 mol/L H3O+: 2.34x10^-4 mol/L - Also if we increase the initial concentration how does this affect the ph n the Ka such as increasing it to .1mol/L - is you have initial concentration of .001 if u increase strength what...

  • We place 0.612 mol of a weak acid, HA, and 12.9 g of NaOH in enough...

    We place 0.612 mol of a weak acid, HA, and 12.9 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.42 . Calculate the ionization constant, Ka, of HA.

  • We place 0.577 mol of a weak acid, HA, and 13.6 g of NaOH in enough...

    We place 0.577 mol of a weak acid, HA, and 13.6 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.50 . Calculate the ionization constant, Ka, of HA.

  • We place 0.565 mol of a weak acid, HA, and 11.6 g of NaOH in enough...

    We place 0.565 mol of a weak acid, HA, and 11.6 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.88 . Calculate the ionization constant, Ka, of HA.

  • We place 0.516 mol of a weak acid, HA, and 12.0 g of NaOH in enough...

    We place 0.516 mol of a weak acid, HA, and 12.0 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.20. Calculate the ionization constant, Ka, of HA.

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT