Write a net ionic equation to show that hypochlorous acid behaves as a Brønsted-Lowry acid in water. BL acid BL base BL base BL acid |c(aq)(s)(l)(g) + H2O |c(aq)(s)(l)(g) + |c(aq)(s)(l)(g)
Write a net ionic equation to show that hypochlorous acid behaves as a Brønsted-Lowry acid in water. BL acid BL base BL base BL acid |c(aq)(s)(l)(g) + H2O |c(aq)(s)(l)(g) + |c(aq)(s)(l)(g)
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Related questions
Part A: Are the following solutions acidic, basic, or neutral?
[OH?] = 1.0Ã10?7 M
[H3O+] = 3.2Ã10?3 M
[H3O+] = 9.6Ã10?4 M
[OH?] = 7.6Ã10?9 M
Part B: Identify the reactant that is a Brønsted-Lowry acid and the reactant that is a Brønsted-Lowry base in each of the following:
CO32?(aq)+H2O?HCO3?(aq)+OH?(aq) Multiple Choice
A. CO32? is the acid (proton acceptor); H2O is the base (proton donor). |
B. H2O is the acid (proton donor); CO32? is the base (proton acceptor). |
C. CO32? is the acid (proton donor); H2O is the base (proton acceptor). |
D. H2O is the acid (proton acceptor); CO32? is the base (proton donor). |
NH3(aq)+H2O(l)?NH4+(aq)+OH?(aq) Multiple choice
A. NH3 is the acid (proton donor); H2O is the base (proton acceptor). |
B. H2O is the acid (proton donor); NH3 is the base (proton acceptor). |
C. H2O is the acid (proton acceptor); NH3 is the base (proton donor). |
D. NH3 is the acid (proton acceptor); H2O is the base (proton donor). |
CH3?COO?(aq)+H3O+(aq)?H2O(l)+CH3?COOH(aq) Multiple choice
A. H3O+ is the acid (proton acceptor); CH3?COO? is the base (proton donor). |
B. CH3?COO? is the acid (proton donor); H3O+ is the base (proton acceptor). |
C. CH3?COO? is the acid (proton acceptor); H3O+ is the base (proton donor). |
D. H3O+ is the acid (proton donor); CH3?COO? is the base (proton acceptor). |
Part C: Calculate the [H3O+] of each aqueous solution with the following [OH?]:
NaOH, 6.0Ã10?3M . Express your answer using two significant figures.
milk of magnesia, 1.2Ã10?5M . Express your answer using two significant figures.
aspirin, 2.4Ã10?11M . Express your answer using two significant figures.
seawater, 4.0Ã10?6M . Express your answer using two significant figures.