Consider the following buffer system: 0.0024 M H2CO3 and 0.024 M HCO3-. What is the pH...
Consider a solution consisting of the following two buffer systems: H2CO3 HCO3– + H+ pKa = 6.4 H2PO4– HPO42– + H+ pKa = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present? ***Please explain why the right answer is right and why the other ones are wrong. a. [H2CO3] > [HCO3- ] and [H2PO4- ] > [HPO42- ] b. [HCO3- ] > [H2CO3] and [HPO42- ] > [H2PO4-...
The pH of blood plasma is 7.40. The principal buffer system is HCO3?/H2CO3. Calculate the ratio [HCO3?]/[H2CO3] in blood plasma. (Ka of H2CO3, carbonic acid, is 4.5 × 10?7) Enter your answer in the provided box.
You need 100.00 mL of a buffer at pH 10.50 based on carbonate (H2CO3; ka1 = 4.3 x 10^-7, ka2 = 5.6 x 10^-11). you have available the following materials: solid sodium bicarbonate (84.006 g/mol), 2.000 M HCl, and 2.000 M NaOH and of course di water. To ensure adequate buffering capacity, the buffer component present at lower concentration should be at 0.200 M. provide a recipie indicating volumes of liquids and/or masses of solids for technician to use in...
9. Consider a 0.15 M solution of H2SO4. Which of the following statements is NOT true? A) This solution would turn litmus to red. B) This solution could neutralize a base. C) This solution has a pH of 11.20. D) This solution could dissolve metal. E) none of the above 10. What is the concentration of the hydronium [Halo ons in a neutral solution? 11. What is the concentration of hydronium ions in an acidic solution? A) 0.0 M B)...
i want answer to all questions please Answer: 29) Consider the following generalized buffer solution equilibrium: When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? A) BH B)H C) HO D)B E None of the species would increase in concentration. Answer: ( 30) What is true about a solution whose pH is less than 7 at 25°C? A) It has...
Question 1 (5 points) Consider the following buffer system: 0.5 M H3PO4 and 0.2 M H2PO4-. What is the pH of such a system (Ka = 7.5 x 10-3)? a) pH = 3.42 b) pH = 5.36 O c) pH = 2.02 d) pH= 1.72
Lab 5 Buffers 1. Dissolved ions in salt solutions can act as acids or bases and react with water to produce hydronium ions or hydroxide ions that contribute to the pH of the salt solution. Since strong acids and strong bases completely ionize in solution, the reverse reaction essentially does not occur, meaning that the resulting conjugate base of a strong acid or conjugate acid of a strong base do NOT act as acids or bases. Ions that are conjugate...
Calculate the pH of the following buffer system. 0.500 M NH3 ( Kb=1.8×10^(-5) ) 0.500 M NH4 Br A. 4.74 B. 9.26 C. 7.00 D.0.30 E. 13.70 I got 4.74
can you answer the following? ULTIPLE CHOICE. Choose the one alternative that best comp letes the statement or answers the question. 1) The conjugate base of HS04 is A) so42 ) HSO4 C) H2s04 D) OH E) H3S04 2) What is the pH of an aqueous solution at 25.0 "C in whichH is 0.00250 M? 2) A) -3.40 8) 3.40 C) 225 D) 2.60 E) -2.60 3) What is the pH of an aqueus solution at 25.0 C that contains...
21. What are the characteristics of the carbonic acid-bicarbonate buffer system (select all that apply? a CO2 is eliminated by the lungs b. Neutralizes HCl acid to yield carbonic acid and salt c. H2CO3 formed by neutralization dissociates into H2O and CO2 d. Shifts H+ in and out of cell in exchange for other cations such as potassium and sodium e. Free basic radicals dissociate into ammonia and OH-, which combines with Ho to form water 22. What are characteristics...