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18. H3PO4+ HCO3 <=> H2PO+ H2CO3 K>>1. The conjugate of HCO3 is a. base; H2PO4 b. acid; H3PO4 C. acid; CO32 d. acid; H2CO3

18. H3PO4+ HCO3 <=> H2PO+ H2CO3 K>>1. The conjugate of HCO3 is a. base; H2PO4 b. acid; H3PO4 C. acid; CO32 d. acid; H2CO3

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases
Section: Chapter Questions
Problem 86GQ: Consider the following ions: NH4+, CO32, Br, S2, and ClO4. (a) Which of these ions in water gives an...
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Hi! Can someone answer no. 18? Kindly include an explanation. Thank you! 

3.0 x 108. a. 1.7 x 10-4 b. 1.4 x 10-7 c. 8.1 x 10-5 d. 3.7 x 10-4 b.16. A Bronsted-Lowry base is defined as a proton donor b. a proton acceptor c. a hydroxide donor d. a hydroxide acceptor 17. For nitrous acid, HNO2, Ka = 4.5 x 10-4. What is the equilibrium constant for the following reaction? a. NO2 + H20 <=> HNO2 + OH- a. 4.5 x 10-18 18. H3PO4 + HCO3 <=> H2PO4+ H2CO3 K>>1. The conjugate a. base; H2PO4 b.19. The pH of a 1.25 x 10-3 M NAOH solution is b. 2.2 x 10-11 C. 4.5 x 10-4 d. 2.2 x 103 of HCO3 is b. acid; H3PO4 C. acid; CO32 d. acid; H2CO3 a. 3.10 b. 11.10 C. 2.90 d. 7.00 d .20. Calculate the approximate [OH-] in a solution that is 0.200 M in NaF. Ka for HF is 6.7 x 10-4. d. 1.7 x 10-6 Y 10-12 b. 1.5 x 10-11 c. 1.3 x 10-4
Transcribed Image Text:3.0 x 108. a. 1.7 x 10-4 b. 1.4 x 10-7 c. 8.1 x 10-5 d. 3.7 x 10-4 b.16. A Bronsted-Lowry base is defined as a proton donor b. a proton acceptor c. a hydroxide donor d. a hydroxide acceptor 17. For nitrous acid, HNO2, Ka = 4.5 x 10-4. What is the equilibrium constant for the following reaction? a. NO2 + H20 <=> HNO2 + OH- a. 4.5 x 10-18 18. H3PO4 + HCO3 <=> H2PO4+ H2CO3 K>>1. The conjugate a. base; H2PO4 b.19. The pH of a 1.25 x 10-3 M NAOH solution is b. 2.2 x 10-11 C. 4.5 x 10-4 d. 2.2 x 103 of HCO3 is b. acid; H3PO4 C. acid; CO32 d. acid; H2CO3 a. 3.10 b. 11.10 C. 2.90 d. 7.00 d .20. Calculate the approximate [OH-] in a solution that is 0.200 M in NaF. Ka for HF is 6.7 x 10-4. d. 1.7 x 10-6 Y 10-12 b. 1.5 x 10-11 c. 1.3 x 10-4
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