Saladaga, Mykhaela
Radon
Palisbo, Vel
Chemistry
III-
Online Treasure Hunt
ACIDS AND BASES
1. What are the physical and chemical behavior of acids and bases?
The term acid comes from the Latin term acere, means "sour". They can be
corrosive to metals and to your skin, have pH of less than 7, it can turns blue litmus
paper to red, and become less acidic when mixed with bases. An acid is a material that
can release a proton or hydrogen ion (H+) and they neutralize bases in a
neutralization reaction.
Bases taste bitter, they feel slippery or soapy, has a pH above 7, can turn red
litmus paper to blue, and become less basic when mixed with acids. A base, or alkali, is
a material that can donate a hydroxide ion (OH-). Bases neutralize acids in a
neutralization reaction and they denature protein.
2. How do we differentiate an acid from a base?
We can differentiate an acid from a base by using pH level or indicator, The
pH measures the acidity (for acids) or alkalinity (for bases) of a solution.
An acid has a pH of 7.34 or less while a base has a pH of 7.46 or greater.
Acids are often referred to as “proton donors” while the bases are the “proton
acceptors.
3. How are the strength of acids and bases identified?
Strong acids completely dissociate in water, forming H+ and an anion. An
incompletely ionized acid are called weak acids, because there is a smaller
concentration of ionized hydrogens available in the solution. This means they
only partially dissociates in water to give H+ and the anion.
Strong bases are the ones who are completely ionize into hydroxide ions
and a conjugate acid. They dissociate 100% into the cation and OH-. Strong
bases are the hydroxides of Groups I and II. Most weak bases are anions of weak
acids. Weak bases do not furnish OH- ions by dissociation. They react with water
to furnish the OH- ions.
4. How are acids and bases quantified?
By using pH scale, it is a measure of the acidity or basicity of a solution. It is
defined as the cologarithm of the activity of dissolved hydrogen ions (H+). the pH
indicator causes the color of the solution to change depending on the
solution’s pH level. The pH scale is not an absolute scale; it is relative to a set of
standard solutions whose pH is established by international agreement.
5. What are pH indicators?
An acid-base indicator is a weak acid or a weak base. The undissociated form of
the indicator is a different color than the iogenic form of the indicator. An Indicator
does not change color from pure acid to pure alkaline at specific hydrogen ion
concentration, but rather, color change occurs over a range of hydrogen ion
concentrations. This range is termed the color change interval. It is expressed as a pH
range.
6. What are common applications/uses of acids and bases?
ACIDS
Used in:
BASES
Used in:
Sulfuric
Acid
Car
Batteries
sodium
hydroxide
Soaps
Acetic
Acid
vinegar
magnesium
hydroxide
Antacid
Tartaric
Acid
Baking
Aluminum
hydroxide
Deodorants
Ascorbic
VitaminC
Sodium
Dish
carbonate
Detergents
Acid
Nitric
Acid
Fertilizers
Carbonic
Acid
Softdrinks
Citric
Acid
Citrus
Fruits
Sodium
hypochlorite
Bleach