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In the reaction co32- H2O -- hco3- oh- the carbonate ion is acting as an a arrhenius base b arrhenius acid c bronsted-lowry base d bronsted-lowry acid?
The Bronsted-Lowry definition describes acids as being proton (H+) donators and bases as being proton acceptors. So the answer would be C, because the carbonate anion is accepting a proton (H+ cation) to become the HCO3-
IS PO4 3- a bronsted acid or base?
Phosphate ion (PO4 3-) acts as a base in the Bronsted-Lowry acid-base theory by accepting a proton (H+).
What is the conjugate acid of HCO3- and why?
The conjugated acid of HCO3- is: H2CO3, carbonic acid.Conjugated pairs of acid and base always differ ONE (1) proton (H+): The acid WITH and the base WITHOUT it.So, on the other hand the conjugated base of HCO3- is: CO32-, carbonate.
How can you justify that NH3 is bronsted Lowry base but not arrhenius base?
NH3 acts as a Bronsted-Lowry base because it can accept a proton (H+) to form the NH4+ ion. In contrast, NH3 does not produce hydroxide ions (OH-) in solution, which is a defining characteristic of an Arrhenius base.
What is the CONJUGATE BASE OF CO32-?
The conjugate base of CO32- is HCO3- (bicarbonate ion), which is formed by removing one proton from CO32-.
In the reaction co32- H2O -- hco3- oh- the carbonate ion is acting as an a arrhenius base b arrhenius acid c bronsted-lowry base d bronsted-lowry acid?
The Bronsted-Lowry definition describes acids as being proton (H+) donators and bases as being proton acceptors. So the answer would be C, because the carbonate anion is accepting a proton (H+ cation) to become the HCO3-
IS PO4 3- a bronsted acid or base?
Phosphate ion (PO4 3-) acts as a base in the Bronsted-Lowry acid-base theory by accepting a proton (H+).
What is the conjugate acid of HCO3- and why?
The conjugated acid of HCO3- is: H2CO3, carbonic acid.Conjugated pairs of acid and base always differ ONE (1) proton (H+): The acid WITH and the base WITHOUT it.So, on the other hand the conjugated base of HCO3- is: CO32-, carbonate.
Is ClO2 a bronsted acid or base?
Bronsted Base
Is CIO2- a bronsted acid base or both?
It is a Bronsted base.
What is example of a Bronsted-Lowry base?
Dissolving formic acid in water the formiate ion formed is the conjugate base of the acid.
How can you justify that NH3 is bronsted Lowry base but not arrhenius base?
NH3 acts as a Bronsted-Lowry base because it can accept a proton (H+) to form the NH4+ ion. In contrast, NH3 does not produce hydroxide ions (OH-) in solution, which is a defining characteristic of an Arrhenius base.
What is the definition of a bronsted-Lowry base?
A Bronsted-Lowry base is a proton acceptor.
What equilibrium system has HCO3 acting as a Brnsted Lowry base?
HCO3 acts as a Brønsted-Lowry base in the bicarbonate buffer system, which consists of the equilibrium between carbonic acid (H2CO3) and bicarbonate ion (HCO3-) in aqueous solution. In this system, HCO3- accepts a proton (H+) to form carbonic acid (H2CO3).
What is the CONJUGATE BASE OF CO32-?
The conjugate base of CO32- is HCO3- (bicarbonate ion), which is formed by removing one proton from CO32-.
What is true of a Bronsted -Lowry base?
A Bronsted-Lowery base accepts H+ ions
What theory of acids and bases do conjugate acids and bases belong to?
Conjugate acids and bases belong to the Bronsted-Lowry theory of acids and bases. In this theory, an acid donates a proton (H+) and a base accepts a proton. A conjugate acid is formed when a base accepts a proton, and a conjugate base is formed when an acid donates a proton.
