What is the conjugate base in the following equation: HBr + H2 O \longrightarrow ⟶ H3 O+ + Br-

would be the conjugate base in this reaction according to the Bronsted-Lowry acid-and-base theory.

Explanation:

Among the reactants, the Bronsted-Lowry acid is the species that supplies protons . The Bronsted-Lowry base would be the species that accept the protons.

On the product side of the equation, the BL-acid donates a proton to produce the conjugate base. The BL-base accepts a proton to produce the conjugate acid.

In this case, each molecule donates a proton to form one ion. Hence,

Each molecule would accept a proton to produce an ion. Hence,

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.

a saline water is fed to a reverse osmosis unit at flow rate o rotameter connected to reject (retentate) line reads 8 installed in reject and permeate line reads 15.2 milli siemens/cm and 300 micro siemens/com respectively.