Question

Please don't answer if can't help with all :) need help for exam prep:

1a:

If the Ką of a monoprotic weak acid is 3.4 x 10-6, what is the pH of a 0.36 M solution of this acid? pH =

1b:

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0117 M solution. The pH of the resulting solution is 2.

1c:

If a buffer solution is 0.140 M in a weak base (Kb = 3.4 x 10-5) and 0.450 M in its conjugate acid, what is the pH? pH 11.7 I

1d:

Calculate the pH at the equivalence point for the titration of 0.240 M methylamine (CH3NH2) with 0.240 M HCl. The Ky of methy

0 0
Add a comment Improve this question Transcribed image text
Answer #1

Day HA is Week mono protic acid. HA + H₂O A & Hot at 0.36(M) 750 .x at 0.36-2. equilibrium, [A-] [Hot] x² Ka of neida 0.36.x2 Ka КА pH = 14- РОН Given, (1) а Оде Д. ОТЈа (м) - 3 2.398 хүр 4 хв. 01/2 4:18 x 10 of acid 19іях) 1 In briffer solution cond) Following reaction oruurs: f etti NH₂4 CH₂NH₂ of Hel is titrated against 2 As, 0129 (M) CH₃NH2 0.29 (M) CH?Nit2 same of He

Add a comment
Know the answer?
Add Answer to:
Please don't answer if can't help with all :) need help for exam prep: 1a: 1b:...
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
  • pls don't answer if cant help with all :) 1a. 1b. 1c. A certain indicator, HA,...

    pls don't answer if cant help with all :) 1a. 1b. 1c. A certain indicator, HA, has a Ką value of 1.0 x 10-5. The protonated form of the indicator is red and the ionized form is yellow. What is the pKa of the indicator? pKa What is the color of this indicator in a solution with pH = 7? yellow red O orange The half-equivalence point of a titration occurs half way to the equivalence point, where half of...

  • 1. 2. 3. 4. 5. please show all work What is the concentration of the acetate...

    1. 2. 3. 4. 5. please show all work What is the concentration of the acetate ion in a 1.00 M CH3COOH solution given that the K, of CH3COOH is 1.8 x 10-5? a. 4.20 x 10-3 M d. 2.84 x 10-4 M b. 0.996 M e. 5.62 x 10-5 M c. 1.00 M Methylamine (CH3NH2) is a weakly basic compound. Calculate the Ky for methylamine if a 0.253 M solution is 4.07% ionized. a. 2.29 x 103 d. 4.24...

  • some acids + bases questions. please answer all parts! Thank you so much! 3a. Cyanic acid,...

    some acids + bases questions. please answer all parts! Thank you so much! 3a. Cyanic acid, HCNO, is a weak monoprotic acid with Ka = 2.0 × 10−4.Calculate the pH of a 0.820 M solution of this acid. Report your answer to TWO places past the decimal. 3b. Hypobromous acid, HBrO, is a weak monoprotic acid with Ka = 2.8 × 10−9.Calculate the pH of a 0.312 M solution of this acid. Report your answer to TWO places past the...

  • 1.  A weak monoprotic acid has molar mass 180 g/mol. When 1.00 g of this acid is...

    1.  A weak monoprotic acid has molar mass 180 g/mol. When 1.00 g of this acid is dissolved in enough water to obtain a 300 mL solution, the pH of the resulting solution is found to be 2.62. What is the value of Ka for this acid? 2. A weak monoprotic acid has pKa = 3.08. Calculate the percent ionization of a 0.35 M solution of this acid. 3. Calculate the pH of a solution that is 0.050 M in CH3COOH...

  • The pH at the equivalence point of a titration of an unknown monoprotic substance with a...

    The pH at the equivalence point of a titration of an unknown monoprotic substance with a strong titrant is determined to be 6.63. Based on this pH value, explain whether the unknown substance is a strong acid, strong base, weak acid, or weak base. A chemist wants to perform a reaction at pH = 8.3 so they attempt to make a buffered solution. For this buffer, the chemist dissolves 12.5 moles of methylammonium, CH3NH3+, (Ka = 2.3 x 10–11) and...

  • Calculate the pH of a solution consisting of 0.225 M solution of CH3NH2 (methylamine) and 0.200...

    Calculate the pH of a solution consisting of 0.225 M solution of CH3NH2 (methylamine) and 0.200 M CH3NH2 tor (methylammonium chloride). Report answer to 2 decimal places. Kb CH3NH2) - 44 x 10-4 CH3NH2 (aq) + H200 + CH3NH3 (2) + OH(aq) Assuming equal initial concentrations of the given species, which of the following is the weakest acid in aqueous solution? O. HB Ky = 2.0 x 10-6 OB.HD K = 6.0 x 10-2 ОС: НЕ Kg = 4.0 x...

  • 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).

  • All of the following are acid-base conjugate pairs EXCEPT Group of answer choices H2O, H3O+ NH4+,...

    All of the following are acid-base conjugate pairs EXCEPT Group of answer choices H2O, H3O+ NH4+, NH3 CH3COOH, CH3COO- H3O+, OH- HPO42-, PO43- The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31. What is the Ka of the acid? Group of answer choices 4.7 x 10-5 4.1 x 10-7 3.4 x 105 2.4 x 10-4 1.3 x 10-5 You have 250.0 mL of a 0.56 M solution of NaCH3COO. How many milliliters of a 0.50...

  • Rank the following solutions in order of increasing pH. Consider the following data on some weak...

    Rank the following solutions in order of increasing pH. Consider the following data on some weak acids and weak bases: - Ka Ko acid name formula nitrous acid HNO2 4.5*10-4 base name formula methylamine CH3NH2 4.4 x 10-4 acetic acid HCH,CO2 1.8 x 10-5 aniline CH3NH2 4.3 * 10-10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the so the solution that will have the next lowest...

  • 17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a...

    17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a base in water solution (a) Show the reaction where HSO4 acts an acid (Ka) (b) Show the reaction where HSO4 acts a base (Kb)? 18. Show the chemical equilibrium processes for Kal and Ka2 for diprotic H2SO3 and justify which Ka is the larger value 19. A buffer contains a weak acid, HA, that is twice the concentration of its conjugate base, A. If...

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