Preparation of 100 ml Normal Saline from 25% NaCl Solution

Vocabulary-style flashcards covering the preparation and classification of solutions, concentration units, colligative properties, and saline tonicity based on the lecture transcript.

Solution

A homogeneous mixture of two or more substances in which their relative concentration can be changed up to a certain limit.

Solvent

The large part of a solution which has the same physical state as that of the solution and is only one in number.

Solute

The minor part of the solution which dissolves in the solvent and loses its physical state to form a solution.

Crystalloidal

A type of solution classified on the basis of its permeability through a cell membrane.

Colligative properties

Properties that depend on the total number of particles per unit volume and not on its chemical nature, including osmotic pressure, lowering of vapor pressure, elevation of boiling point, and depression of freezing point.

Standard solution

The solution whose strength or concentration is known.

Normal solution

A solution which contains one gram equivalent weight of solute per liter of solution.

Equivalent weight of an element

The ratio defined as $\frac{\text{Molecular Weight}}{\text{Valency}}$.

Molar solution

A solution which contains one gram molecular weight of solute per liter of solution.

Molal solution

A solution which contains one gram molecular weight of solute in $1000\text{ gm}$ ($\text{kg}$) of solvent.

Osmolar Solution

A solution where one osmole of solute is dissolved in $1\text{ liter}$ of solution.

Percent by weight ($w/w$ solution)

This indicates weight in grams of solute per $100\text{ gm}$ solution.

Percent by volume ($w/v$ solution)

This indicates the grams of solute per $100\text{ ml}$ of solution.

Percent by volume ($v/v$ solution)

This indicates the milliliters of solute per $100\text{ ml}$ of solution.

Mole

The molecular weight of a substance expressed in grams.

Molarity

The number of mole per liter of solution, expressed as $\frac{\text{Number of mol}}{\text{liter of soln}}$.

Molality

The number of mole per kilogram of solvent.

Normality

The number of gram equivalent weight per liter of solution.

Osmolarity

The number of Osmole per liter of solution.

Osmolality

The number of osmole per kilogram of solvent.

Osmole

The number of osmotically active substances which in one liter of solution exerts $22.4$ atmospheric pressure on $22.4 \times 760\text{ mmHg}$ pressure.

Normal saline

A 0.9\text{%} NaCl solution commonly used for RBC counting, treatment of dehydration, plasma replacement in burns, and washing wounds.

Isotonic Solution

A solution which has the same osmotic pressure as that of plasma, such as 0.9\text{%} NaCl solution.

Hypotonic Solution

A solution which has less osmotic pressure than that of plasma, such as 0.45\text{%} NaCl solution.

Hypertonic solution

A solution which has greater osmotic pressure than that of plasma, such as 3\text{%} NaCl solution.