A Simple Chemistry Question..?

Question

1.) According to Arrthenius , what are the characteristics of acids and bases?


2.) How do Hydronium ions form? why do they form in aqueous acid solution?

3.)what are conugate acids and bases?

4.)there are 3 common theories of acids and bases.
explain how each of the ff. theories defines acids and bases.
a.) Arrhenius
b.) Bronsted-loury
c.)Lewis

Answer 1

Lancenigo di Villorba (TV), Italy

WOW! Your Chemistry's teacher have a VERY ACIDIC CHARACTER, is it not?

QUESTION 1)
The ARRHENIUS's ACIDS are defined as Electrolytes which may release HYDROGEN IONS in its solutions.

HA <---> A- + H+

The ARRHENIUS's BASES are defined as Electrolytes which may release OXYDRIL's IONS in its solutions.

BOH <---> B+ + OH-

QUESTION 2)
HYDRONIUM IONS form by dissociation of PROTIC chemical stuff in some solvents : the dissociation belongs to phenomena taking place in its interactions with solvents.

Subs.H + Solv. <---> Subs.- + Solv.H+

Among the PROTIC compounds, ACIDS show a relatively GREAT VALUE of the Equilibrium's Constant related to the overwritten equation.

QUESTION 3)
ACIDS and BASES undergo dissociation while they dissolve in its solutions.
Since many ACIDS and BASES take place to chemical equlibria, the definition assigned to these electrolytes MAY BE EXTENDED to the formed ions as the role assumpted.

HA1 + B1 <---> A2- + HB2+

In the overwritten equation, HA1 is an ACID and B1 is a BASE. As you seen, HA1 interacts forming one ion as A1-, where the latter is defined as a base or "A1- is the Conugate Base of HA1".
As you seen, B1 interacts forming one ion as HB1+, where the latter is defined as a base or "HB1+ is the Conugate Acid of B1".

QUESTION 4)
As it is stated, Acids and Bases belong to Electrolytes. The ELECTROLYTES are defined as soluble chemical stuffs undergoing dissociation permitted by solvent's action : in this manner, they release ions. The IONS are defined as atoms or its aggregations having an NOT-trivial electrical charge.
ARRHENIUS's ACIDS belong to Electrolytes releasing HYDRONIUM IONS by dissociation in its solutions.
ARRHENIUS's BASES belong to Electrolytes releasing OXYDRIL IONS by dissociation in its solutions.
BRONSTED-LOWRY's ACIDS belong to Polar Compounds which may act as HYDRONIUM IONS's DONORS when they interact with other chemical stuffs.
BRONSTED-LOWRY's BASES belong to Polar Compounds which may act as HYDRONIUM IONS's ACCEPTORS when they interact with other chemical stuffs.
LEWIS's ACIDS belong to Polar Compounds which may act as ELECTRON DUET's ACCEPTORS when they interact with other chemical stuffs.
LEWIS's BASES belong to Polar Compounds which may act as ELECTRON DUET's DONORS when they interact with other chemical stuffs.

I hope this helps you.

Answer 2

According to the Arrhenius definition, an acid is any substance, which when dissolved in water, tends to increase the amount of H+.
An Arrhenius base is any substance, which when dissolved in water, tends to increase the amount of OH-.
http://www.nyu.edu/classes/tuckerman/honors.chem/lectures/lecture_21/node2.html

3.) Conjugate Acids of Bases
After losing a proton, the acid species becomes the conjugate base. A base and its protonated partner also form a conjugated acid-base pair. These relationships have been represented by
H+ + Base = Conjugate_acid of Base+
Acid = H+ + Conjugate_base of Acid-

http://www.science.uwaterloo.ca/~cchieh/cact/c123/baseacid.html


4a.) Arrhenius Theory
Ionic compounds dissociate and can become free ions acting as separate entities in solution.
ACID: Substance that produces H+1 in water.
BASE: Substance that produces OH-1 in water.

4b.) Bronsted/Lowry Theory
Not limited to aqueous solutions but for all proton (H+) containing systems.
ACID: Substance that can donate proton (H+1).
BASE: Substance that can accept proton (must contain lone pair of electrons).
Bronsted/Lowry expands Arrenhius to include any proton transfer (water not requirement).

4c.) Lewis Theory
ACID: Substance that can accept a pair of electrons from another atom to form a new bond.
BASE: Substance that can donate a pair of electrons to another atom to form a new bond.
Lewis expands acid/base reactions to include many substances without H in formula.
All Bronsted/Lowry acid/base reactions are also Lewis acid/base reactions.

http://web.fccj.org/~ethall/acidbase/acidbase.htm