Quick Answer: What Is The Conjugate Acid For Co3 2?

Is h2so4 acid or base?

According to Arrhenius concept, an acid is a substance that, on dissolving in water, dissociates either partially or completely into H+ (or H3O+) ions; while a base is a substance that dissociates into OH- ions.

Since H2SO4 dissociates into 2H+ and SO4- – on dissolving in water, we see that H2SO4 is an acid..

Is Na2CO3 an acid or base?

Na2CO3 is neither an acid nor a base. It is a salt. A salt in chemistry is formed by the reaction of an acid and a base.

Is BR an acid or base?

KaAcidBase1.0 * 109Hydrobromic acidBr-1.3 * 106Hydrochloric acidCl-1.0 * 103Sulfuric acidHSO4 -2.4 * 101Nitric acidNO3 -28 more rows

What kind of bond is co3 2?

Ionic bond: The chemical bond between oppositely charged ions (for example between K+ (cation) and CO3 charge 2- (anion)) is known as an ionic bond. In K2CO3, two positive ions of potassium (K) and 1 negative ion of carbonate (CO3) forms the ionic bond.

What is the conjugate acid of HS?

Hydrosulfuric acid is the conjugate acid of the hydrogen sulfite ion it dissociates into in solution.

Why conjugate base of weak acid is strong?

A strong acid like HCl donates its proton so readily that there is essentially no tendency for the conjugate base Cl– to reaccept a proton. … A strong base like the H– ion accepts a proton and holds it so firmly that there is no tendency for the conjugate acid H2 to donate a proton. Hence, H2 is a very weak acid.

What is the conjugate acid of carbonate?

A conjugate acid is a substance that is formed when a base receives a proton, or H+ . Carbonic acid, or H2CO3 , will be the conjugate acid of hydrogen carbonate.

What is the chemical formula for the conjugate acid of the carbonate ion co2 − 3?

Carbonate Ion is a polyatomic ion with formula of CO3(2-). Carbonate is a carbon oxoanion. It is a conjugate base of a hydrogencarbonate.

Is co3 2 an acid or base?

[CO3](2-) is carbonate ion. It can accept a proton (H+) to form bicarbonate ion, [HCO3](-), making carbonate ion a Bronsted-Lowry base.