BIO303 Lab Manual

Contents

1. Preparation of stock solutions
2. Preparation of working solutions
3. Estimation of normal and abnormal glucose levels in urine-part A
4. Estimation of normal and abnormal glucose levels in urine-part B
5. Estimation of albumin levels in urine
6. Estimation of chloride contents in urine
7. Estimation of phosphate contents in urine
8. Kidney function tests
9. Liver function test-I (determination of ALT levels)
10. Liver function test-II (determination of AST levels)

Preparation of stock and working solutions in Laboratory

Weighing balance, volumetric flask, Cylinder, beaker, stirrer, pH meter or litmus paper

Chemicals required

Sodium chloride, Hydrochloric acid, sulfuric acid

Theory

Solution:

“A solution is a homogenous mixture of atoms, ions or molecules of two or more substances.” A homogenous mixture is that which has uniform position throughout its body.

Solvent and Solute

The solvent is the component of a solution that is visualized as dissolving another component called absolute. Usually the component present in the larger quantity is called the solvent, and the component present in the smaller quantity is called the solute.

Types of solution

Unsaturated solution

A solution that is capable of dissolving more solute at a given temperature than it already contains, is known as unsaturated solution.

Saturated solution

A saturated solution is the solution which can dissolve no more amount of the solute, at a given temperature.

Super saturated solution

A solution that contains more dissolved solute than a saturated solution is called super saturated solution.

Concentration and its units

Concentration means the relative amounts of the components of a solution. It tells the ratio of the quantity of one component to the quantity of the other or to the total quantity of solution. It has many units. Some common units are discussed below.

Mass Percentage

The ratio of the mass of the solute to the mass of the solution multiplied by 100 is called mass percentage. Mass Percentage of a solute =Mass of the solute x 100 Mass of solution For liquid-liquid solutions, it is sometimes more convenient to express the concentration in the units of percentage by volume:

Volume Percentage of a liquid = Volume of the liquid x100 Total volume

Parts per Million (ppm)

This is used to express very dilute concentrations of a substance. One ppm is equal to 1mg of solute dissolved per litre of solvent or 1mg of solute dissolved per kg of solvent.

Molarity (M)

Molarity or the molar concentration is the number of moles of solute dissolved per dm3of solution. (1 dm3is equal to 1Liter)

Molarity = Number of moles of solute Volume of solution in liters

Molality (m)

Molality is the number of moles of solute dissolved per kilogram of solvent.

Normality (N)

Normality is the number of equivalents dissolved per liter of solution.

Normality = No. of equivalents Volume of solution in Litres

pH

The pH is defined as follows: “The pH of a solution is the negative logarithm to the base 10 of the hydrogen ion (or Hydronium ion) concentration”. pH = -log10[H+]

pH =-log10[H3O+]

The pH of a neutral solution is 7, the pH of acids is less than 7 while that of bases is higher than