Question

Calculate the pH of 0.249 M piperazine (C4H10N2, a di-basic compound, "B"). Calculate the concentration of...

Calculate the pH of 0.249 M piperazine (C4H10N2, a di-basic compound, "B"). Calculate the concentration of each form of piperazine in this solution. (Ka1 = 4.65 ✕ 10−6 and Ka2 = 1.86 ✕ 10−10.)

pH=

[B]= M

[BH+]= M

[BH22+]= M

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the pH of 0.242 M piperazine (C4H10N2, a di-basic compound, "B"). Calculate the concentration of...
Calculate the pH of 0.242 M piperazine (C4H10N2, a di-basic compound, "B"). Calculate the concentration of each form of piperazine in this solution. (Ka1 = 4.65 ✕ 10−6 and Ka2 = 1.86 ✕ 10−10.) NOTE: Use three significant figures in all answers and use quadratic formula. pH [B] M [BH+] M [BH22+] M
Calculate the pH and the equilibrium concentration of C6H6O62- in a 6.12×10-2 M ascorbic acid solution,...
Calculate the pH and the equilibrium concentration of C6H6O62- in a 6.12×10-2 M ascorbic acid solution, H2C6H6O6 (aq). For H2C6H6O6, Ka1 = 7.9×10-5 and Ka2 = 1.6×10-12 pH = [C6H6O62-] = M
Calculate the pH at the second stoichiometric point when 130 mL of a 0.030 M solution...
Calculate the pH at the second stoichiometric point when 130 mL of a 0.030 M solution of glutaric acid (Ka1=4.54*10-5, Ka2=5.4*10-6) is titrated with 1.0 M NaOH.
Calculate the concentration of malonate ion (C3H2O42-) in a 0.200 M solution of malonic acid (C3H4O4)....
Calculate the concentration of malonate ion (C3H2O42-) in a 0.200 M solution of malonic acid (C3H4O4). (For malonic acid, Ka1 = 1.4 × 10-3, Ka2 = 2.0 × 10-6.) show your work please
Calculate the [C3H2O42-] and the pH of a 0.10 M solution of malonic acid (H2C3H2O4) (Ka1...
Calculate the [C3H2O42-] and the pH of a 0.10 M solution of malonic acid (H2C3H2O4) (Ka1 = 1.5 x 10-3 ; Ka2 = 2.0 x 10-6). Is there a way to do this without the ICE tables? Please show work. Thanks!
Calculate the concentration of all species in a 0.520 M solution of H2SO3. The acid ionization...
Calculate the concentration of all species in a 0.520 M solution of H2SO3. The acid ionization constants for the acid are Ka1=1.6×10−2 and Ka2=6.4×10−8.
Calculate the pH and the equilibrium concentrations of H2PO4-, HPO42- and PO43- in a 0.0353 M...
Calculate the pH and the equilibrium concentrations of H2PO4-, HPO42- and PO43- in a 0.0353 M aqueous phosphoric acid solution. For H3PO4, Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, and Ka3 = 3.6×10-13 pH = ? [H2PO4-] = ?M [HPO42-] = ?M [PO43-] = ?M
Calculate the concentration of bicarbonate ion in a 0.100 M solution of sodium carbonate. Ka1 and...
Calculate the concentration of bicarbonate ion in a 0.100 M solution of sodium carbonate. Ka1 and Ka2 of carbonic acid are 4.2 x 10-7 and 4.8 x 10-11, respectively.
What is the pH of a solution of 3.4 M H2A (Ka1 = 1.0 × 10^-6...
What is the pH of a solution of 3.4 M H2A (Ka1 = 1.0 × 10^-6 and Ka2 is 1.0 × 10^-10)? Please explain step by step
Calculate the pH in 0.020 M H2SO3(Ka1=1.5×10−2, Ka2=6.3×10−8)
Calculate the pH in 0.020 M H2SO3(Ka1=1.5×10−2, Ka2=6.3×10−8)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT