The arterial blood plasma is buffered by the carbonic acid and bicarbonate ion, with a ratio of 1:20. Assume that the acid has a concentration of 0.1 M with a dissociation constant of 7.9x10-7 ? What is the pH of arterial blood plasma? * Do not round off the pKa. Use the complete value of the pKa in solving for the pH. Your answer This is a required question

The arterial blood plasma is buffered by the carbonic acid and bicarbonate ion, with a ratio of 1:20. Assume that the acid has a concentration of 0.1 M with a dissociation constant of 7.9x10-7 ? What is the pH of arterial blood plasma? * Do not round off the pKa. Use the complete value of the pKa in solving for the pH. Your answer This is a required question

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 6P

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Part A What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.608 mol of Na.A in 2.00 L of solution? The dissociation constant K of HA is 5.66 x 10-7. Express the pH numerically to three decimal places. ▸ View Available Hint(s) pH = 6.181 Submit Previous Answers Correct Since both the acid and base exist in the same volume, we can skip the concentration calculations and use the number of moles in the Henderson- Hasselbalch equation to calculate the pH. The answer will be the same. Part B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places. ▸ View Available Hint(s) 195| ΑΣΦ pH= 6.124 Submit Previous Answers Request Answer * Incorrect; Try Again; 5 attempts remaining
Listen Consider the following buffer system: 1.04 M H3PO4 and 0.85 M H₂PO4-. What is the pH of such a system (K₂ = 7.5 x 10-³)? Your Answer: Answer
PLEASE ANSWER ALL PARTS THANK YOU Given:Kb for ammonia of 1.8 X 10-5 Volume of NH3 in flask (mL): 10.00 Average Volume of HCl it took to get to equivalence point (mL): 20.50 Concentration of HCl (M): 0.100Volume of HCl added to calculate “beyond equivalence pH”(mL): 10.50 a) Calculate the concentration of the ammonia.b) Calculate the pH of the contents of the flask (NH3) before the titration begins.c) Calculate the pH of the contents of the flask in the titration at ¼ way to equivalence. This means use your volume added to get to eq point (mL) value but multiply it by ¼ (so you are not yet at equivalence).d) Calculate the pH of the contents of the flask in the titration at ½ way to equivalence (so also not yet at equivalence)e) Calculate the pH of the contents of the flask in the titration at the equivalence point.f) Calculate the pH of the contents of the flask in the titration beyond the equivalence point. Use your given amount
Question 4: Problem A 50.0 mL of 0.20 M of sodium benzoate (C,H;NaO2) (Ka= 6.46 x 10°) is added with a. 0.00 mL b. 50.00 mL c. 80.00 mL d. 100.00 mL e. 110.00 mL of 0.10 M HCl. Calculate the pH at each addition
Question 4: Problem A 50.0 mL of 0.20 M of sodium benzoate (C-H;NaO2) (Ka= 6.46 x 10°) is added with a. 0.00 mL b. 50.00 mL c. 80.00 mL d. 100.00 mL e. 110.00 mL of 0.10 M HCI. Calculate the pH at each addition
(Incorrect) When 0.20 mol of NaOH is added to 0.50 mol of weak acid HX, in a total volume of 1.00 L, the pH of the resultant solution is 6.65. Calculate Ka for HX. 2,2x107 (Your answer) 1.3x10-7 1.5x107 (Correct answer) 9.0×10-8 3.4×10-7
Calculate the pH during the titration of 100.0 mL of 0.200 M HCl with 0.400 M NaOH. First what is the initial pH (before any NaOH is added)? Answer: 1.69
Calculate the pH of a solution that contains 0.00415 M HI and 0.400M benzoic acid. (Ka for benzoic acid is 6.5x10-5) Answer:
QUESTION 1 How many grams NH4Cl and how many milliliters 2.5 M NaOH should be added to 300 mL water and diluted to 700 mL to prepare a buffer of pH 9.50 with a salt concentration of 0.10 M? (Obtain Ka of ammonia from the appendix of your textbook) QUESTION 2
LESSON: Acid-Base TitrationAnswer the following questions.1. Why is there a need to standardize the NaOH solution?2. Why is there a need to use CO2-free water in a dimensional analysis?
Consider the following table: Name Formula Conjugate Acid Ammonia NH3 Methylamine CH3NH₂ Ethylamine C₂H5NH2 Aniline C6H5NH2 Pyridine оо NH₂+ CH3NH3 Submit Answer + C₂H5 NH3 + C6H5NH,+ C5 H5 N CH;NH* Try Another Version Which base would be the best choice for preparing a pH = 5.00 buffer? ethylamine aniline ammonia pyridine methylamine + Kb 1.8 × 10-5 4.38 x 10-4 5.6 × 10-4 3.8 × 10-10 1.7 × 10-⁹ 1 item attempt remaining
What is the effective pH-buffering range for a buffer prepared from butanoic acid and the sodium salt of its conjugate base (sodium butyrate)?A) 3.8 - 5.8 B) 4.8 - 6.8 C) 5.8 - 7.8 D) 7.4 - 9.4 E) 8.8 - 10.8