Consider the following acid-base equilibrium system: H2PO4+ H20 →HPO42+ H30*1 Identify the Bronsted-Lowry bases in this equilibrium. O H2PO4 -1 and H30*1 O HPO42 and H30+1 O H20 HPO,2 and -1 O H2PO4 and H20

Consider the following acid-base equilibrium system: H2PO4+ H20 →HPO42+ H301 Identify the Bronsted-Lowry bases in this equilibrium. O H2PO4 -1 and H301 O HPO42 and H30+1 O H20 HPO,2 and -1 O H2PO4 and H20

Chemistry

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Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Consider the following acid-base equilibrium system: H2PO4+ H20 →HPO42+ H30*I
Identify the Bronsted-Lowry bases in this equilibrium.
-1
H,PO4
and
H30*l
HPO,2
and
H30+1
H20
HPO42
and
-1
H,PO4
and
H20
MacBook Air
80
F6
F7
F2
F3
F4
F5

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