Q10. Blood pH is controlled by the carbon dioxide-bicarbonate buffer system. CO₂ (g) + H₂O (L) H* (aq) + HCO3(aq) Dr. Robert Ranzenberger likes to run long distances. Predict the following during the exercise. Lactic acid in blood Acidity PH [Choose ] Choose High Low No change Choose Choose 2

Q10. Blood pH is controlled by the carbon dioxide-bicarbonate buffer system. CO₂ (g) + H₂O (L) H* (aq) + HCO3(aq) Dr. Robert Ranzenberger likes to run long distances. Predict the following during the exercise. Lactic acid in blood Acidity PH [Choose ] Choose High Low No change Choose Choose 2

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.11PAE

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7. Describe a buffered solution. Give three examples of buffered solutions. For each of your examples, write equations and explain how the components of the buffered solution consume added strong acids or bases. Why is buffering of solutions in biological systems so important?
MISSED THIS? Read Section 18.8 (Pages 829 - 833). Part A A solution is made that is 1.0x10-3 M in Zn(NO,), and 0.130 Min NH3. After the solution reaches equilibrium, what concentration of Zn?+ (aq) remains? Express your answer using two significant figures. Zn]= 5.1• 10- M Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining
Consider the buffer system of carbonic acid (H₂CO₂) and its salt, KHCO₂, which provides the conjugate base, HCO,. H_COjlog) + HJO W 7 HyO" loạ) + HCOy loa) How does the buffer react when some base is added? The bicarbonate ion (HCO) of the buffer reacts with the base. OHCO and H₂CO, both react with the base. O The buffer does not react. O The carbonic acid (H₂CO₂) of the buffer reacts with the base Question 15 Indicate whether each of the following reactions is an example of reaction of an acid with a metal, reaction of an acid with a carbonate, or acid-base neutralization reaction using the dropdown on the right. Reaction A: ZnCO3(s) + 2HBr(aq) → ZnBr₂(aq) + CO₂(g) + H₂O(l) Reaction B: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) HCI(g) + NaHCO3(s)→ NaCl(aq) + CO₂(g) + H₂O(0) H₂SO4(aq) + Mg(OH)2(s)→ MgSO4(aq) + 2H₂O(1) 3LIOH(aq) + H₂PO₂(aq) → Li₂PO₂(aq) + 3H₂O(0) Cal(s) + H₂SO4(aq) → H₂(g) + CaSO₂(aq) Reaction C: Reaction D: Reaction E: Reaction E
The weak acid, chloroacetic acid, is a useful reagent in organic synthesis owing to a reactive C-CI bond. It has a K. = 1.40x10. Part A Determine the concentration of H* (or H,0") at equilibrium of a 5.68x102 mol L-1 solution of chloroacetic acid. O 3.58x10 mol L O 8.24x10 mol L O 8.92x10 mol L- O 1.90x10 mol L-1
Please answer question 5a,b,c,d (All PARTS). Thank you for your help! 5) You determined that the pH of a 0.1M solution of lactic acid, C,H,OHCOOH, is 2.9. What is the K, of the acid reaction? a. Use an ICE table to calculate the equilibrium concentrations. C,H,OHCOOH C,H,OHCOO H* OM "O M" C E b. What is the equilibrium expression for the reaction? K,= c. Calculate K. d. Is lactic acid a stronger or a weaker acid than acetic acid (pK, = 4.75)? Explain. %3D
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