Acids, Bases, and Salts Flashcards

Vocabulary-style flashcards covering the properties, definitions, examples, and pH values of acids, bases, and salts as described in the lecture notes.

Acid (General Definition)

A substance whose water solution tastes sour, turns blue litmus red, and neutralizes bases.

Base (General Definition)

A substance whose aqueous solution tastes bitter, turns red litmus blue, or neutralizes acids.

Salt (General Definition)

A neutral substance whose aqueous solution does not affect litmus.

Citric Acid

A naturally occurring acid found in fruits like oranges and lemons.

Tartaric Acid

A naturally occurring acid found in tamarind.

Malic Acid

A naturally occurring acid found in apples.

Lactic Acid

A naturally occurring acid found in milk and milk products.

Hydrochloric Acid (Gastric Juice)

The specific acid found in gastric juices.

Lime Water

A common example of a base found in nature.

Acetic Acid

Also known as vinegar, used in the kitchen.

Boric Acid

An acid used for laundry purposes.

Baking Soda (Household Use)

A substance used for the purpose of cooking.

Washing Soda

A substance used for cleaning purposes.

Laboratory Acids

Acids such as $HCl$ and $H_2SO_4$ used in laboratories and industries.

Laboratory Bases

Bases such as $NaOH$ and $KOH$ used in laboratories and industries.

Neutralization Reaction

A reaction where acids and bases are mixed in right proportions to form salt and water.

Natural Salt Sources

Seawater and natural rock deposits containing $NaCl$ and $KCl$.

Acidus / Acere

Latin words from which the term acid is derived, meaning sour.

Hydronium Ion

The ionizable ion ($H_3O^+$) rendered by an acid in its aqueous solution.

Natural Acids

Acids obtained from natural sources such as fruits and animal products.

Mineral Acids

Acids prepared from minerals, such as Hydrochloric acid, Sulphuric Acid, and nitric acid.

Base (Physical feel)

A substance characterized by a bitter taste and a soapy feel.

Hydroxyl Ion

The ion ($OH^-$) rendered by a base in its aqueous solution.

Cations

Positively charged ions that constitute a salt.

Anions

Negatively charged ions (organic or inorganic) that constitute a salt.

pH (Chemical Definition)

The negative logarithm of the $H^+$ ion concentration.

Power of Hydrogen

The literal meaning of the name pH.

Universal Indicator

A substance used to determine the strength of acids and bases quantitatively by showing different colours.

pH Scale Range

The scale for pH varies from $0$ to $14$.

Acidic Solutions (pH range)

Solutions having a pH value ranging from $0$ to $7$ on the scale.

Basic Solutions (pH range)

Solutions having a pH value ranging from $7$ to $14$ on the scale.

Neutral Solutions (pH value)

Solutions having a pH value equal to $7$.

Strongly Acidic Solution (pH value)

A solution having a pH value equal to $0$.

Strongly Basic Solution (pH value)

A solution having a pH value equal to $14$.

Strong Acids

Acids that furnish a higher number of $H^+$ ions.

Degree of Ionisation

A factor that differs for various acids and bases and helps in determining their strength.

Battery Acid

A substance with a pH value of $0$.

Gastric Acid

A substance with a pH value of $1$.

Lemon Juice

A substance with a pH value of $2$.

Apple Juice

A substance with a pH value of $3$.

Tomato Juice

A substance with a pH value of $4$.

Milk (pH value)

A common dairy product with a pH value of $6$.

Water (pH value)

A neutral substance with a pH value of $7$.

Epo

A substance listed on the pH scale with a value of $8$.

Baking Soda (pH value)

A substance with a pH value of $9$.

Milk of Magnesia

A substance with a pH value of $10$.

Ammonia solution

A substance with a pH value of $11$.

Soap

A substance with a pH value of $12$, appearing next to NO4.

Bleach

A substance with a pH value of $13$.

Drain cleaner

A substance with a pH value of $14$.

Scale Base

The pH scale is expressed on a logarithmic scale with base $10$.

Neutralization Principle

The combination of $H^+$ ions and $OH^-$ ions to form water ($H_2O$).

Strong Acid + Strong Base

Resultant pH is equal to $7$.

Strong Acid + Weak Base

Resultant pH is less than $7$ ($< 7$).

Weak Acid + Strong Base

Resultant pH is greater than $7$ ($> 7$).

Weak Acid + Weak Base ($K_a > K_b$)

The resultant pH is less than $7$ ($< 7$).

Weak Acid + Weak Base ($K_a = K_b$)

The resultant pH is equal to $7$.

Weak Acid + Weak Base ($K_a < K_b$)

The resultant pH is greater than $7$ ($> 7$).

General Neutralization Equation

$\text{acid} + \text{base} (\text{alkali}) \rightarrow \text{salt} + \text{water}$.

Formation of Sodium Chloride

The chemical equation is $HCl + NaOH \rightarrow NaCl + H_2O$.