Unit 20 3. The carbonate buffer system is very important in regulating blood pH levels. Carbonic acid is diprotic and therefore has two Ką values: H₂CO3(aq) H+(aq) + HCO3-(aq) HCO3(aq) H¹(aq) + CO32-(aq) Kal = 4.2 x 10-7 Ka2 = 4.8 x 10-11 Since the second dissociation has a Ka value significantly smaller than that of the first dissociation, it can be assumed to have no effect on the H₂CO3(aq)/HCO3(aq) equilibrium. blood? nolla The pH of blood is 7.4. What is the ratio of carbonic acid to bicarbonate ion in 22 vols Bang SENE WAY

Unit 20 3. The carbonate buffer system is very important in regulating blood pH levels. Carbonic acid is diprotic and therefore has two Ką values: H₂CO3(aq) H+(aq) + HCO3-(aq) HCO3(aq) H¹(aq) + CO32-(aq) Kal = 4.2 x 10-7 Ka2 = 4.8 x 10-11 Since the second dissociation has a Ka value significantly smaller than that of the first dissociation, it can be assumed to have no effect on the H₂CO3(aq)/HCO3(aq) equilibrium. blood? nolla The pH of blood is 7.4. What is the ratio of carbonic acid to bicarbonate ion in 22 vols Bang SENE WAY

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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What is the pH of a solution of 1.4 M HF in 1.9 M CaF2? (Ka HE = 7.2 x 10-4) IMPORTANT: When entering your answer: • Enter the number only (no units) • Do not leave any spaces • Include the sign if your answer is negative (not necessary for positive values) • Use a leading zero before the decimal when necessary Report your number to 2 decimal places (regardless of the significant figures) Correctly round your answer to the 2nd decimal place (margin of allowed error is only + 0.01, so always use un-rounded numbers in your calculations). If the last digits are zeros they will not display once you click away, but the answer will still be marked correct. Examples: 12.34 or -0.56
Complete the following table. Be sure to show each calculation in detail.
The value of K₂ for the generic acid HX is 1 x 10-³. What is the value of K for its conjugate base X™? 1 x 10-14 1 x 10-10 1 x 10-11 1 x 10-² 1 x 10-7
Calculate the concentrations of all species present in a 0.18 M solution of ethylammonium chloride (C,H-NH,CI). The Ka value of C,H-NH,+ is 1.8e-11. [C,H,NH,] X M [H+] [C,H5NH,+] M [CI -] M [OH - ] M
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Another buffer found in blood is based on the equilibrium between dihydrogen phosphate and monohydrogen phosphate. The reaction is shown below: H2PO4-(aq) + H2O(l) → H3O+(aq) + HPO42-(aq) If the pH of a blood sample was 7.05, what would you calculate as the ratio of [H2PO4-] to [HPO42-]? (Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8, Ka3 = 3.6 × 10-13)
What is the [H3O+] of a solution which is 0.1690 M in CH3CO2H and 0.1590 M in NaCH3CO2? CH3CO2H(aq) + H2O(l) → CH3CO2−(aq) + H3O+(aq) Ka = 1.800e-5
The completed equilibrium table for a 0.270 M solution of propanoic acid is shown. HC,H;O,(aq) C,H,0, (aq) H*(aq) + initial 0.270 change +x +x -x equilibrium 0.270 – x What is the concentration of H† in the solution? [H*] = M Calculate the pH of the solution. pH =
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If the bicarbonate ion (HCO3-) concentration in a sample of blood is 0.270 M, determine the carbonic acid (H2CO3) concentration required to buffer the pH of blood at pH = 7.45. H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Ka = 5.3 × 10-7 Show all calculations including equation(s) used. Provide your final answer to 3 decimal places.
= O ACIDS AND BASES Predicting the qualitative acid-base properties of salts Consider the following data on some weak acids and weak bases: name acetic acid hypochlorous acid solution 0.1 M NACIO 0.1 M C5H5NHCI acid 0.1 M NaNO3 0.1 M KCH3CO₂ 0 Explanation formula HCH3CO₂ 1.8 x 10 -5 HCIO Check 3.0 × 10 pH ✓choose one 1 (lowest) 2 Ka 3 4 (highest) choose one X-5 choose one ◊ 7 0 -8 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. ? base K₂ formula pyridine CHN 1.7 x 107 -9 ammonia name + A ALEKS-... NH3 NH3 AN 30 1.8 × 10 -5 tv h MacBook Air Þ G 0/5 Hannah S Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center AO Accessib
ASA (also known as Aspirin) contains acetylsalicylic acid, C16H12O6. Acetylsalicylic acid is a weak acid, with a Ka of 3.3x10-11. If the concentration of a solution of ASA is 0.015 mol/L, what is its pH at equilibrium and pOH?