Question

PRACTICE EXERCISE Niacin, one of the B vitamins, has the molecular structure C-0-H A 0.020 M solution of niacin has a pH of 3
0 0
Add a comment Improve this question Transcribed image text
Answer #1

-C-0-H + H20 FA + H₂O (CG HY NO ) + H30t HCG H y NO₂ Il 0-020 M -X El 0.020 - x +x pH = 3:26 pH = -log[H30] -pH = log [bizot]

Add a comment
Know the answer?
Add Answer to:
PRACTICE EXERCISE Niacin, one of the B vitamins, has the molecular structure C-0-H A 0.020 M...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • Example: K, from pH Niacin is one of the B vitamins. A 0.020 M solution of...

    Example: K, from pH Niacin is one of the B vitamins. A 0.020 M solution of niacin has a pH of 3.26. What is the acid-dissociation constant for niacin? Find the percent dissociation (ionization)

  • Table 18.2 (continued) 18.20 Solutions Tested pH [H(M) [C,H,O, (M) Percent Dissociation | 0.10 M HCH...

    Table 18.2 (continued) 18.20 Solutions Tested pH [H(M) [C,H,O, (M) Percent Dissociation | 0.10 M HCH 0, 2.14 0.010 M HCH 0, 13.09 0.0010 M HC,H,O 284 Question Write the net ionic equation describing the dissociation of acetic acid in aqueous solution. Question Calculate (H) and C.H.O.- for each concentration above, showing a sample cal- culation here Question Write the equilibrium constant expression for acetic acid, and calculate a Kvalue and an apparent percent dissociation for each concentration, showing sample...

  • solution A consists of the conjugated pair hclo 0.020 m / clo- 0.020 m solution B...

    solution A consists of the conjugated pair hclo 0.020 m / clo- 0.020 m solution B consists of the conjugate pair hclo 0.080 m / clo- 0.080 m. for the conjugate pair hclo / clo- the ka = 2.8 x 10-8. it is correct to say that solution a has a buffering capacity _________ than solution b and that the damping range of both solutions is ______________. A. minor ..... between pH 6.55 and pH 8.55 B. major ..... between...

  • A 0.020 M solution of a weak acid HA has a pH of 3.50. What is...

    A 0.020 M solution of a weak acid HA has a pH of 3.50. What is the percent ionization of HA in the solution? For the solution described above, what is the Ka?

  • Practice Exercise 16.29 599.2 ml of a 0.11 M solution of ammonia is mixed with 599.2...

    Practice Exercise 16.29 599.2 ml of a 0.11 M solution of ammonia is mixed with 599.2 mL of a 0.11 M solution of HBr. What is the pH of the resulting solution of NH Br? (K for NH, equals 1.8 x 10) pH = the tolerance is +/-2% Click if you would like to show Work for this questioni Deen Short Work x Incorrect. Does your answer make sense given the Ka? The K, for HF is 6.8 x 10-4....

  • 1. Calculate the pH at 25°C of a 0.757 M solution of a weak acid that...

    1. Calculate the pH at 25°C of a 0.757 M solution of a weak acid that has Ka = 9.28 x 10 2. Determine the Kb of a weak base if a 2.50 M solution of the base has a pH of 9.595 at 25°C. 3. The overall dissociation of malonic acid, H2C3H2O4, is represented below. The overall dissociation constant is also indicated. H2C3H204 = 2 H+ + C3H2042- K = 3.0 x 10-9 To a 0.025-molar solution of malonic...

  • 2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-]...

    2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-] = 3.5 x 10-2M (c) pOH = 10.5 3. What is the pH of a 0.10 M solution of HCIO4? (A strong acid) 4. Write the dissociation reaction and the corresponding K, expression for the following acids in water. (a) H3PO4 (b) C&H OH 5. Write the reaction and corresponding Ko expression for each of the following bases in water. (a) NH3 (b) PO4...

  • Determination of the dissociation Constant (K_a) of a weak Acid. The pH of a 0.10 M...

    Determination of the dissociation Constant (K_a) of a weak Acid. The pH of a 0.10 M solution of formic acid (HCOOH) is 2.39, what is the K_a of the acid? K_a = Hydrofluoric Acid, A weak Acid with K_a = 7.1 times 10^-4 A. For a 0.50 M solution of HF, calculate the equilibrium concentrations of HF, H^+ and F^-. [HF] = [H^+] = [F^-] = % Dissociation =, pH = B. Now consider a 0.050 M solution of HF....

  • ASAP! What is Ka for the weak acid, HA, if a 0.020 M solution of the...

    ASAP! What is Ka for the weak acid, HA, if a 0.020 M solution of the acid has a pH of 3.29 at 25ºC? a. 5.1 × 10-2 b. 6.9 × 10-2 c. 2.6 × 10-4 d. 1.3 × 10-5 e. 1.0 × 10-6 What is the conjugate acid of H2PO4–(aq)? a. H3O+ b. H3PO4 c. HPO42– e. PO43–

  • please explain the steps please 5. Determine the Ky for CN at 25°C. The K, for...

    please explain the steps please 5. Determine the Ky for CN at 25°C. The K, for HCN is 4.9 x 10-10. 6. Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80. 7. Determine the acid dissociation constant for a 0.020 M formic acid solution that has a pH of 2.74. Formic acid is a weak monoprotic acid and the equilibrium equation of interest is HCOOH(aq) + H20(1) =H30+(aq) + HCO2-(aq).

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
ADVERTISEMENT