RevieConstarPart ABlood is buffered by carbonic acid and the bicarbonate ion. Normal bloodplasma is 0.024 mol L-1 in HCO3 and 0.0012 mol L-1 in H2CO3 (pKal for H2CO3 at body temperature is 6.1).What is the pH of blood plasma?Express your answer using one decimal place.pH = 7.4SubmitPrevious Answersv CorrectPart BIf the volume of blood in a normal adult is 5.0 L , what mass of HCl can be neutralized by the buffering system in blood before the pH falls below 7.0 (whichdeath)?Express your answer using two significant figures.i (3 E ?MHCI =SubmitPrevious Answers Request Answerx Incorrect; Try Again; 5 attempts remainingPart CGiven the volume from part B, what mass of NaOH can be neutralized before the pH rises above 7.8?Express your answer using two significant figures.i (3 ED ?MNAOH =

Answered: Image /qna-images/answer/6db5bb9e-d3f8-47f7-9a18-ba6e6f638e3e.jpg

Constar • Part A Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 mol L-1 in HCO and 0.0012 mol L-1 in H2CO3 ( pKal for H2CO3 at body temperature is 6.1). What is the pH of blood plasma? Express your answer using one decimal place. pH = 7.4 Submit Previous Answers v Correct • Part B If the volume of blood in a normal adult is 5.0 L, what mass of HCI can be neutralized by the buffering system in blood before the pH falls below 7.0 (which death)? Express your answer using two significant figures. i* (3 EB 1? MHCI = Submit Previous Answers Request Answer x Incorrect; Try Again; 5 attempts remaining • Part C Given the volume from part B, what mass of NAOH can be neutralized before the pH rises above 7.8? Express your answer using two significant figures. MNAOH =

Constar • Part A Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 mol L-1 in HCO and 0.0012 mol L-1 in H2CO3 ( pKal for H2CO3 at body temperature is 6.1). What is the pH of blood plasma? Express your answer using one decimal place. pH = 7.4 Submit Previous Answers v Correct • Part B If the volume of blood in a normal adult is 5.0 L, what mass of HCI can be neutralized by the buffering system in blood before the pH falls below 7.0 (which death)? Express your answer using two significant figures. i* (3 EB 1? MHCI = Submit Previous Answers Request Answer x Incorrect; Try Again; 5 attempts remaining • Part C Given the volume from part B, what mass of NAOH can be neutralized before the pH rises above 7.8? Express your answer using two significant figures. MNAOH =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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If 15.0 mL of glacial acetic acid (pure HC2H3O2) is diluted to 1.70 L with water, what is the pH of the resulting solution? The density of glacial acetic acid is 1.05 g/mLpH=?
The pH of blood plasma is 7.40. Assuming that the principal buffer system in blood is HCO, /H2CO3, A) determine the ratio [HCO,]/[H2CO3] in blood plasma. The ionization con- stant of carbonic acid is K.(H2CO3) = 4.3 x 10-7. B) Based on your result in part (A), how many moles of H2CO3 (assuming that they occupy no volume) would need to be added to 300.0 mL of an aqueous solution that is 0.250 mol L- in NaHCO3 to make a buffer solution of the same pH as blood plasma? To solve the problem you may assume that the solutions behave as ideal dilute solutions (solute-type activity coefficients equal to unity).
pH: 3 [H*]: 10-3 M [OH]: 10-11 M 14 1 1 7 · 10-7 10-7 10-14 10-14 Dip litmus paper into the solution or add a drop of universal indicator. Use the sliders to change the pH of the solution and observe the effect on the indicators. Click Reset to start over. Help Reset The solution turns orange when the univeral indicator is added to it. Is the solution basic, acidic, or neutral?
What volume of 0.837 M KOH solution do you need to make 3.62 L of a solution with a pH of 12.700? Express your answer to three significant figures and include the appropriate units. HÅ V-21.6 4 ml ENC Submit Previous Answers Bequat Answer ? X Incorrect; Try Again; 4 attempts remaining Begin by calculating [OH-] in the final solution using the given pH value. Since KOH is a strong base and completely dissociates into K and OH in an aqueous solution, the molarity of OH equals the molarity of KOH. Finally, rearrange the dilution equation (M₁ V₁M₂V₂) to solve for the initial volume (Vi).
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a) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a solution which is 0.40 M in NH4+ and 0.40 M in NH3? The Kb of NH3 is 1.8 x 10-5. The correct answer should be reported to two places past the decimal. b) Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution (C6H5NH2, Kb = 4.3 x 10-10) with 100. mL of a 0.11 M aqueous nitric acid solution. Your pH should be reported to two places past the decimal point.
How many milliliters of 0.0334 M KOH are needed to completely neutralize the HCI in 430 mL of a hydrochloric acid solution that has a pH of 2.91? mL 0.0334 M KOH
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The pH of blood is 7.4. What is the ratio (to one decimal place) of bicarbonate (conjugate base) to carbonic acid (weak acid) in the blood's buffering equilibrium? Note, the K₂ of carbonic acid is 4.27 x 10-7. Write your answer this way: # to 1 Done Clear Incorrect. The ratio is 10.7 to 1, indicating that there is 10 times more bicarbonate than carbonic acid. Enter the correct answer.
6) The value of Kw at 37 °C (human body temperature) is 2.1 x 10-14. a) At this temperature what is the concentration of (H3O*] ions and [OH] ions? b) At this temperature what is the pH of the neutral solution?
This question has two parts. Part-I (a) Calculate the pH of a 0.20 M HF solution. The Ka of HF is 6.8*10-4. Show the ICE table and all calculations. Part-II (b) Calculate the pH of a solution containing both 0.20 M HF and 0.10 M HCl? The Ka of HF is 6.8*10-4. Show the ICE table and all calculations.