Give two bronsted acid-base that are not Arrhenius bases.
I assume you want a base by the Bronsted acid/base theory that are not bases by the Arrhenius theory.
NH3 is not a base by the Arrhenius theory.
NH3 + H^+ ==> NH4^+
How about SO4^2-?
SO4^2- + H^+ ==> HSO4^-
Sure! Here are two examples of Bronsted acid-base pairs that are not Arrhenius bases:
1. Ammonia (NH3) and Water (H2O): In this case, ammonia acts as a Bronsted base and water acts as a Bronsted acid. When ammonia donates a lone pair of electrons to a water molecule, it forms the ammonium ion (NH4+) and hydroxide ion (OH-).
2. Acetic Acid (CH3COOH) and Sodium Bicarbonate (NaHCO3): Acetic acid acts as a Bronsted acid, and sodium bicarbonate acts as a Bronsted base. When acetic acid donates a proton (H+) to the bicarbonate ion, it forms sodium acetate (CH3COONa) and carbonic acid (H2CO3).
These examples illustrate acid-base reactions where the substances involved do not strictly follow the definition of Arrhenius bases, which are substances that associate with water to produce hydroxide ions (OH-).
To find two Bronsted acids that are not Arrhenius bases, let's first understand the differences between the two concepts:
1. Arrhenius bases: These are substances that release hydroxide ions (OH-) when dissolved in water. Examples of Arrhenius bases include sodium hydroxide (NaOH) and potassium hydroxide (KOH). These bases dissociate in water to produce hydroxide ions, making them suitable for neutralizing acids.
2. Bronsted acids: These are substances that donate protons (H+) to another substance. In Bronsted-Lowry acid-base theory, an acid is a proton donor, and a base is a proton acceptor.
So, to find two Bronsted acids that are not Arrhenius bases, we need to look for substances that can donate protons but do not necessarily release hydroxide ions in water.
Example 1: Acetic Acid (CH3COOH)
Acetic acid is a Bronsted acid because it donates a proton from its acidic hydrogen (H+) to another substance. However, it is not considered an Arrhenius base because it does not produce hydroxide ions when dissolved in water.
Example 2: Hydrochloric Acid (HCl)
Hydrochloric acid is a strong Bronsted acid as it donates a proton to a base. However, it is not an Arrhenius base because it does not release hydroxide ions when dissolved in water.
So, acetic acid (CH3COOH) and hydrochloric acid (HCl) are two examples of Bronsted acids that are not Arrhenius bases.