Chemistry In Context
9th Edition
ISBN: 9781259638145
Author: Fahlman, Bradley D., Purvis-roberts, Kathleen, Kirk, John S., Bentley, Anne K., Daubenmire, Patrick L., ELLIS, Jamie P., Mury, Michael T., American Chemical Society
Publisher: Mcgraw-hill Education,
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Textbook Question
Chapter 8.9, Problem 8.41YT
For each acid–base pair, write a balanced neutralization reaction. Then, rewrite the equation in total ionic and net ionic forms. What is the relevance of the final simplified step in each case?
- a. HNO3(aq) and KOH(aq)
- b. HCl(aq) and NH4OH(aq)
- c. HBr(aq) and Ba(OH)2(aq)
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Check out a sample textbook solutionStudents have asked these similar questions
a) Enough of a monoprotic acid is dissolved in water to produce a 1.291.29 M solution. The pH of the resulting solution is 2.832.83. Calculate the Ka for the acid.
b)
i) Determine the [OH−] , pH, and pOH of a solution with a [H+] of 8.6×10−10 M at 25 °C.
ii) Determine the [H+] , pH, and pOH of a solution with an [OH−] of 0.028 M at 25 °C.
iii) Determine the[H+] , [OH−] , and pOH of a solution with a pH of 10.26 at 25 °C.
iv) Determine the [H+] , [OH−] , and pH of a solution with a pOH of 3.28 at 25 °C.
Sulfuric acid is a diprotic acid. It's a two stages of ionization as shown below.
H2SO4 (aq) →→ H+ + HSO4- (aq) pKa = ???
HSO4- (aq) ↔↔ H+ + SO42- pka = 1.991
a) Calculate the concentration of HSO4- & SO42- ion in a 0.5000 M H2SO4 solution.
b) Determine the pH of the solution to the correct number of significant figures.
Q1A: 3.95 g NH4HCO3 is added to 1000 ml of water, What are the H3O+, OH-, NH3, and HCO3-?
What is the concentration of each species present in a 0.010-M solution of phthalic acid, C6H4(CO2H)2?
C6H4(CO2H)2(aq) + H2O(l) ⇌ H3O+(aq) + C6H4(CO2H)(CO2)-(aq)
Ka1 = 1.1 x 10-3
C6H4(CO2H)(CO2)(aq) + H2O(l) ⇌ H3O+(aq) + C6H4(CO2)22-(aq)
Ka2 = 3.9 x 10-6
Chapter 8 Solutions
Chemistry In Context
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