Question

Why are most anions basic in ${\mathbf{\text{H}}}_{\mathbf{\text{2}}}\mathbf{\text{O}}$ ? Give formulas of four anions that are not basic.

Short answer

Anions are negatively charged compounds. They have an additional pair of electrons, implying that they have an additional pair of electrons. They are mostly basic because they can accept a proton from water. After that, the water will convert and the solution will become basic.

${\text{Cl}}^{\text{-}}{\text{,I}}^{\text{-}}{\text{,Br}}^{\text{-}}{\text{,NO}}_{\text{3}}^{\text{-}}$

Step-by-step solution

Define the formula

A chemical formula depicts the mass proportions of the various elements in a compound.

Explanation

Anions are chemicals with a negative charge. They have an extra pair of electrons, which means they have an extra pair of electrons. Because they can accept a proton from water, they are mainly basic. The water will then convert to ${\text{OH}}^{\text{-}}$, making the solution basic. Remember that a proton acceptor is a Bronsted-Lowry base.

There are some anions that aren't fundamental. Strong acids frequently have them as the conjugate base.

In water, strong acids completely dissociate. They're reactions that can't be reversed.

${\text{HA+H}}_{\text{2}}\text{O}\to {\text{H}}_{\text{3}}{\text{O}}^{\text{+}}{\text{+A}}^{\text{-}}$

As a result, because there is no reverse reaction, the${\text{A}}^{\text{-}}$ anions will not behave as a conjugate base for it. Instead, they'll simply function as an anion.

Strong acid anions, such as $\text{HClHI,HBr}$, and ${\text{HNO}}_{\text{3}}$are examples of non-basic anions.

${\text{Cl}}^{\text{-}}{\text{,I}}^{\text{-}}{\text{,Br}}^{\text{-}}{\text{,NO}}_{\text{3}}^{\text{-}}$