55/ 55. Human blood is buffered by carbonic acid and bicarbonate ions.Alkalosis is a condition caused by excess production of bicar-bonate in the blood. A patient's blood plasma has a pH = 7.6(pKa for H2CO3 at body temperature is 6.1).MISSED THIS? Read Section 18.2; Watch KCV 18.2B, IWE 18.2, 18.3[HCO3][H2CO3]a. What is the ratio ofin the patient's blood?b. The doctor gives the patient 0.45 g of HCl intravenously toneutralize alkalosis. After treatment, the patient's blood is0.0156 M in HCO3¯ and 0.0012 M in H2CO3. If the volume ofblood in the patient's body is 5.3 L, what is its new pH?

55.a)For buffer solution, pH is calculated by Henderson-Hasselbalch equationThe equation ispH = pKa…

Answered: 55. Human blood is buffered by carbonic…

Chemistry

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ISBN:9781305957404

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

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 125CP: Cacodylic acid, (CH3)2AsO2H, is a toxic compound that is a weak acid with pKa = 6.19. It is used to...

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Cacodylic acid, (CH3)2AsO2H, is a toxic compound that is a weak acid with pKa = 6.19. It is used to prepare buffered solutions. Calculate the masses of cacodylic acid and sodium cacodylate that should be used to prepare 500.0 mL of a pH = 6.60 buffer so that the buffer has a total of arsenic-containing species equal to 0.25 M, that is, so that: [(CH3)2AsO2H] + [(CH3)2AsO2] = 0.25 M
For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
Predict what effect each would have on this equilibrium: Cu2+ (aq) + 4 NH3 (aq) ⇌ [Cu(NH3)4]2+ (aq) Addition of copper(II) nitrate solution Addition of HCl(aq) Addition of 1 M NH3
Calculate the pH of a solution that is 0.40 M H2NNH2 and 0.80 M H2NNH3NO3. In order for this buffer to have pH = pKa, would you add HCl or NaOH? What quantity (moles) of which reagent would you add to 1.0 L of the original buffer so that the resulting solution has pH = pKa?
Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
What is the effect on the concentration of ammonia, hydroxide ion, and ammonium ion when the following are added to a basic buffer solution of equal concentrations of ammonia and ammonium nitrate: (a) KI. (b) NH3. (c) HI. (d) NaOH. (9) NH4Cl
What are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M solution of acetic acid (K2 = 1.8 105)? What is the pH of the solution?
A buffered solution containing disolved aniline, C6H5NH2, and aniline hydrochloride, C6H3NH3Cl, has a ph of 5.71 A. determine the concentration of C6H5NH3+ in the solution if the concentration of C6H5NH2 is 0.290 M. The pKb of aniline is 9.13 C6H5NH3+ = M B. Calculate the change in pH of the solution (delta)pH, if 0.377 g NaOH is added to the buffer for a final volume of 1.05L. assume that any contribution of NaOH to the bolume is negligible (delta)pH =
Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, - log Ka The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: How many grams of dry NH4C1 need to be added to 2.00 L of a 0.600 mol L-' solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.80? Kh for ammonia is 1.8 × 10–5. pKa base] pH = pKa +log acid Express your answer to two significant figures and include the appropriate units. Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. • View Available Hint(s) ? X•10n Value mass of NHẠCI = Units
GW 18b 1. A 20.0 mL sample of a 0.240 M hydrofluoric acid (HF) solution is titrated with 0.200 M NaOH. Determine: (a) pH of the acid solution before any base is added; (b) volume (in mL) of base needed to get to the equivalence point; (c) pH halfway to equivalence point; (d) pH at equivalence point; (e) pH when 0.100 mL NaOH is added beyond the equivalence point. (K₂ of HF = 7.1 × 104)
Consider the following acid-base reaction: H3O+ + HPO42 H₂PO4 + H₂O Identify the Bronsted-Lowry base. OH₂O ⒸHPO4 ²- OH₂PO4 OH3O+ What is the concentration (in Molarity) of a Sulfuric Acid (H₂SO4) solution if a 15.0 mL sample required 26.4 mL of 0.950 M KOH for neutralization? H₂SO4 + 2 KOH --> K₂SO4 + 2 H₂O (balanced) 0.012 M 0.025 M 0.836 M 0.270 M
11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting the resulting solution to a volume of 1.0 L. What is the effect of adding 0.020 mol CH3COO (aq) to this solution? How will pH change (calculate pH before and after the addition. Ka of CH3COOH is 1.76 x10-5)? How will concentrations of CH3COOH and CH3COO at equilibrium change?

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