IX Chemistry - Chapter 2 - Chemical Combinations and Chemical Equation

Laws of Chemical Combinations

There are four laws of chemical combinations these laws explained the general feature of chemical change. These laws are:

1. Law of Conservation of Mass

2. Law of Definite Proportions

3. Law of Multiple Proportions

4. Law Reciprocal Proportions

Antoine Lavoiser has rejected the worn out ideas about the changes that take place during a chemical reaction. He made careful quantitative measurements in chemical reactions and established that mass is neither created nor nor destroyed in a chemical change.

Law of Conservation of Mass

Statement

It is presented by Lavoiser. It is defined as:

"Mass is neither created nor destroyed during a chemical reaction but it only changes from one form to another form."

In a chemical reaction, reactants are converted to products. But the total mass of the reactants and products remains the same. The following experiment easily proves law of conservation of mass.

Practical Verification (Landolt Experiment)

German chemist H. Landolt, studied about fifteen different chemical reactions with a great skill, to test the validity of the law of conservation of mass. For this, he took H.shaped tube and filled the two limbs A and B, with silver nitrate (AgNO3) in limb A and Hydrochloric Acid (HCl) in limb B. The tube was sealed so that material could not escape outside. The tube was weighed initially in a vertical position so that the solution should not intermix with each other. The reactant were mixed by inverting and shaking the tube. The tube was weighed after mixing (on the formation of white precipitate of AgCl). He observed that weight remains same.

HCl + AgNO3 ----------> AgCl + NaNO3

Law of Definite Proportions

Statement

It is presented by Proust. It is defined as:

"When different elements combine to give a pure compound, the ratio between the masses of these elements will always remain the same."

Proust proved experimentally that compound obtained from difference source will always contain same elements combined together in fixed proportions.

Example

Water can be obtained from different sources such as river, ocean, well, canal, tube well, rain or by the chemical combination of hydrogen and oxygen. If different samples of water are analyzed, it will have two elements, hydrogen and oxygen and the ratio between their mass is 1:8.

Law of Multiple Proportions

Statement

This law is defined as:

"When two elements combine to give more than one compounds, the different masses of one element, which will combine with the fixed mass of other element, will be in simple whole number ratio."

Two different elements can combine to form more than one compound. They can do so by combining in different ratios to give different compounds.

Example

Hydrogen and oxygen combine with one another to form water (H2O) and hydrogen peroxide (H2O2). In water and hydrogen oxide 2 g of hydrogen combine with 16g and 32g of oxygen respectively. According to law of multiple proportions, the different masses of oxygen (16g and 32g) which have reacted with fixed mass (2g) of hydrogen will have a simple ratio between each other i.e. 16:32 or 1:2. It means that hydrogen peroxide contains double the number of oxygen atoms than water. This law proves this point of Dalton's Atomic Theory that atoms do not break in a chemical reaction.

Law of Reciprocal Proportions

Statement

This law is defined as:

"When two element A, B combine separately, with the mixed mass of the third element E, the ratio in which these elements combine with E is either the same or simple multiple of the ratio in which A and B combine with each other."

Example

Hydrogen and Nitrogen separately combine to form ammonia (NH3) and dinitrogen oxide (N2O), in these compounds, fixed mass of nitrogen is 14g and combines with 8 g of oxygen and 3 g of hydrogen. The ratio between the mass of oxygen and hydrogen is 8:3. Hydrogen and oxygen also combine with one another to form water (H2O). The ratio between hydrogen and oxygen in water is 16:2. These ratios are not same. Let us observe whether these ratios are simple multiple to each other or not following mathematical operation is carried out.

8:3 ::16:2

8/3 : 16/2

or

8/3 x 2/16

or

1/3 => 1:3

Definitions

Atomic Mass

The mass of an atom of the element relative to the mass of some reference or standard element is called atomic mass. Atoms are very small particles. They have very small mass. If the masses of atoms were to be expressed in gram. It is a very big unit for this very tiny object. Then it was decided by the chemists that masses of the atoms were to be found after comparing with mass to some standard form.

Hydrogen being the lightest element is taken as standard. The mass of the hydrogen atom taken as one.

The atomic mass could be defined as

"Atomic mass of an element is the mass of an atom of that element as compared to the mass of an atom of hydrogen taken as one."

Example

The atomic mass of sodium is 23. It means that an atom of sodium is 23 times heavier than hydrogen atom. Similarly atomic mass of oxygen is 16. It means that an atom of oxygen is 16 times heaviest than that of hydrogen.

Atom

The smallest particle of an element which cannot exist independently and take part in a chemical reaction is known as Atom.

Examples

Hexogen(H), Carbon (C), Sodium (Na), Gold (Au) etc.

Molecule

The particle of a substance (Element or Compound) which can exist independently and show all the properties of that substance is called molecule.

Atoms of the same or different elements react with each other and form molecule.

Atoms of some elements can exist independently, since they have property of molecule so they are called mono atomic molecule.

Examples

Examples of Molecules of the elements are Hydrogen (H2). Nitrogen (N2), Sulphur (S8) etc.

Molecules of different elements are called compounds. For example HCl, H2O, CH4 etc.

Valency

The combining capacity of all elements with other elements is called valency.

Example

H = 1

C = 4

Al = 3

Mg = 2

Na = 1

Chemical Formula

"A brief name used for full chemical name at a compound is called Chemical Formula."

A chemical formula is used to represent an element or a compound in terms of symbols. It also represents the number and type of atoms of elements present in the smallest unit of that substance.

Example

The chemical formula of hydrogen sulphide is H2S. It shows two types of elements (H and S) and number of atoms of element (2H and 1S). Similarly the formula of NaCl show number and type of different atoms present in its smallest unit.

Empirical Formula

"The formula which shows the minimum (simple) ratio between atoms present in a compound is known as Empirical Formula."

Example

For example the empirical formula of hydrogen peroxide is HO that of water is H2O and benzene is CH.

Molecular Formula

The formula of an element or a compound which represents the actual number of atoms present in the molecule of these substances is called molecular formula.

Example

Water, Hydrogen Peroxide, Ethylene Benzene and Sulphur have molecular formula H2O, H2O2, C2H4, C6H6 and S8 respectively.

Molecular Mass

Molecular mass of an element or a compound is defined as the mass of its molecule relative to 1/12th of the mass of C-12. It is the sum of the atomic masses of all the atoms presents in its molecular formula.

Example

Molecular mass of water (H2O) = 2 + 16 = 18 a.m.u

Mass of hydrogen sulphide (H2S) = 2 + 32 = 34 a.m.u

Formula Mass

Formula mass of a compound is the mass of its formula unit relative to 1/12th of the mass of C-12.

Example

Formula mass of Sodium Chloride NaCl = 23 + 35.5 = 58.5 a.m.u

Formula mass of Calcium Chloride CaCl2 = 40 + 35.5x2 = 111a.m.u

Molar Mass

The mass of one mole of a substance is called molar mass.

Example

1 mole of Hydrogen atom (H) = 1.008g

1 mole of Hydrogen molecule (H2) = 2.016g

Thus mass of substance is related to the particles by mole.

Chemical Reaction

A chemical change in which reactants are converted to products is called chemical reaction.

Zn + 2HCl --------> ZnCl2 + H2

The fact that a chemical reaction is taking place can be inferred from the following observation.

1. Evolution of a gas

2. Change in colour

3. Change in temperature.

4. Emission of light.

Types of Chemical Reaction

The chemical reaction is classified into following types:

1. Displacement Reaction

The reaction in which an atom or group of atoms is displaced by another atom or group of atoms in a compound is called displacement reaction.

Fe + CuO ---------> Cu + FeO

2. Double Displacement Reactions

The reactions in which reacting substances exchange their radicals or ions are double displacement reaction. Insoluble salts are formed by mixing soluble salts.

3. Addition Reactions

When two different compounds or elements react together to give only one confound, the reaction will be called addition reaction.

2Mg + O2 --------> 2MgO

4. Decomposition Reaction

The reaction in which some compounds may decompose into elements or simpler compounds on heating is called decomposition reaction.

CaCO3 ---------> CaO + CO2 (Heat)

Chemical Equation

Symbolic representation of chemical change in terms of symbols and formulae is called Chemical Equation.

Method of Equation Writing

A chemical equation can be written as follows:

1. Write the formulae and symbols of the reactants on the left hand side.

2. Write the formulae and sympols of the products on the right hand side.

3. Separate the reactants and products by an arrow which is directed towards the products.

Characteristics of Chemical Equation

1. Chemical equation must be representative of a chemical reaction.

2. It should represent molar quantities.

3. It should be balanced in terms of atoms/molecules of reactants and products.

Reactants

Those substances, which react together in a chemical reaction, are called reactants.

Zn + 2HCl ------> ZnCl2 + H2

In the above reaction Zn and HCl are the reactants.

Products

Those substances, which are formed in a chemical reaction, are called products.

Zn + 2HCl ------> ZnCl2 + H2

In the above reaction, ZnCl2 and H2 are products.

Information obtained from a Chemical Equation

1. A balanced equation indicates that which reactant undergo chemical change. It indicates that which products are formed.

2. It indicates that how many moles of reactants under go chemical change. It indicates that how many moles of products are formed.

Why are Chemical Equations Balanced

A chemical equation must be balanced in order to satisfy the law of conservation of matter, which states that matter can neither be created nor be destroyed during a chemical reaction.

Chapter 2- Biological Molecules

BIOCHEMISRTY

Biochemistry is a branch of biology, which deals with the study of chemical components and chemical processes in living organisms.

WATER (H2O)

MAIN CHARACTERISTICS OF WATER

• Chemically it is “Dihydrogen oxide”

• It is the most abundant component in living cell.

• Its amount varies approximately from 70 to 90% and life activities occur in the cell due to the presence of water.

• It is a polar molecule, means that it has a very slightly negative end (the oxygen atom) and a very slightly positive end (the hydrogen atom).

• Due to its polarity, H2O molecules form hydrogen bonds.

IMPORTANT BIOLOGICAL PROPERTIES OF WATER

(1) BEST SOLVENT

• Water is an excellent solvent for polar substances, when ionic substances dissolved in water, dissociate into positive and negative ions.

• Non-ionic substances, having charged groups in their molecules, are dispersed in water.

• Because of solvent property of water, almost all reactions in cells occur in aqueous media.

(2) HIGH HEAT CAPACITY

• Water has great ability of absorbing heat due to its high specific heat capacity.

• The specific heat capacity of water is the number of calories required to raise the temperature of 1g water through 1ºC.

• The thermal stability plays an important role in water based protoplasm of individual’s metabolic activities.

(3) HIGH HEAT OF VAPORIZATION

• Liquid water requires higher amount of heat energy to change into vapours due to hydrogen bonding which holds the water molecules together.

• It provides cooling effect to plants when water is transpired, or to animals when water is respired.

(4) ACT AS AMPHOTERIC MOLECULE

• Water molecule acts both as acid and a base. As acid, it gives up electron to form H+ ion, while as a base, it gains electron to form OH ions.

H2O ↔ H+ + OH-

• It acts as buffer and prevents changes in the pH of living body.

(5) PROTECTION

• Water is an effective lubricant that provides protection against damage resulting from friction.

• It also forms a fluid cushion around organs that helps to protect them from trauma.

(6) AS REAGENT /TURGIDITY

• Water acts as a reagent in many processes such as photosynthesis and hydrolysis reactions.

• It also provides turgidity to the cells.

ORGANIC COMPOUNDS

Those compounds containing carbon (other than carbonates) are called organic compounds. E.g: carbohydrates, Proteins, Lipids and Nucleic acid.

INORGANIC COMPOUNDS

Those compounds, which are without carbon, are called inorganic compounds. E.g: water, carbondioxide, acids , bases and salts.

MACROMOLECULES

Huge and highly organized molecules which form the structure and carry out the activities of cells are called “Macromolecules” Macromolecules can be divided into four major groups.

• Proteins

• Carbohydrates

• Lipids

• Nucleic acids.

MONOMERS

Macromolecules are composed of large number of low molecular weight building blocks or subunits called “Monomers” E.g: Amino-acids (Protein).

CONDENSATION

The process by which two monomers are joined is called “Condensation”.

In this process two monomers join together when a hydroxyl(OH) group is removed from one monomer and a hydrogen (-H) is removed from other monomer.

This type of condensation is called “Dehydration Synthesis” because water is removed (dehydration ) and a bond is made (synthesis).

HYDROLYSIS

A process during which polymers are broken dawn into their subunits (monomers) by the addition of H2O called “Hydrolysis “. It is just reverse of the condensation.

FUNCTIONAL GROUPS

These are particular group of atoms that behave as a unit and give organic molecules their physical, chemical properties and solubility in aqueous solution. E.g

• Methyl group (CH3-)

• Hydroxyl or Alcohol group (OH-)

• Carboxylic acid or Organic-acid group (COOH-)

• Amino or Amine group (NH2-)

• Carbonyl group (CO=)

• Sulfhydryl group (SH-)

PROTEINS

These are the complex organic compounds having C, H,O and N as elements but sometimes they contain P and S also. Due the presence of N they are called “Nitrogenous Compounds” Proteins constitute more than 50% of dry weight of cell. They are present in all types of cells and in all parts of the cell.

CHEMICAL COMPOSITION OF PROTEINS

• Proteins are polymers of amino-acids and number of amino-acids varies from a few to 3000 or even more in different proteins.

• These amino-acids are linked together by specialized bond or linkage called “peptide linkage”

• Each proteins has a unique sequence of amino-acids that gives the unique properties to molecules.

AMINO ACID

It is the basic structural unit of proteins and all amino-acids have an “Amino group (NH2-) and a “Carboxyl group (COOH-)” attached to the same carbon atom, also known as “Alpha carbon”. The have the general formula as:

1. A hydrogen atom.

2. An amino (NH2) group.

3. A carboxyl group (COOH)

4. “Something else” this is the “R” group.

R

│

H2N ─C ─ COOH

(Amino group) │ (Carboxylic group)

H

“R” may be a “H” as in glycine, or CH3 as in alanine, or any other group. So amino acids mainly differ in the R-group.

POLYPEPTIDES

Amino Acids are linked together to from polypeptides of proteins. The amino group of one amino acids may react with the carboxyl group of another releasing a molecule of water. E.g: Glycine and analine may combine to form a dipeptiede

PEPTIDE LINKAGE/ BOND

The linkage between the hydroxyle group of carboxyl group of one amino-acid and the hydrogen of amino-group of another amino-acid release H2O and C-N link to form a bond called “Peptide bond”.

TYPES OF PROTEINS ON THE BASIS OF STRUCTURE

There are four basic structural levels of proteins.

(A) PRIMARY STRUCTURE

• A polypeptide chain having a linear sequence of amino-acids.

• Disulphide (S-S) bond is other important characteristic of the primary protein.

E.g: Insulin Polypeptide chain.

B) SECONDARY STRUCTURE

• In this type polypeptide chain of amino-acids become spirally coiled.

• This coiling results in the formation of a rigid and tubular structure called “Helix”

C) TERTIARY STRUCTURE

• Polypeptide chain bends and folds upon it self forming a globular shape.

• It is maintained by three types of bonds. Namely ionic, hydrogen and disulfide (S-S).

(D) QUATERNARY STRUCTURE

• This type is usually present in highly complex proteins in which polypeptide tertiary chains are aggregated and held together by hydrophobic interactions, hydrogen and ionic bonds.

E.g: Haemoglobin molecule.

FUNCTIONS OF PROTEIN

• They Build many Structures of the cell E.G: Plasma Membrane.

• All enzymes are proteins and in this way they control the whole metabolism of the cell.

• Skin, nails, hair, feather, horn etc. contain portion called keratin.

• Casein is the milk portion and ovalbumin is the egg white protein.

• Collagen present in bones, cartilage, etc. is the most abundant protein in higher vertebrates.

• Protein acts as antibodies, antigens and fibrin etc.

CARBOHYDRATES

It is a group of organic compounds having carbon, oxygen and hydrogen, in which hydrogen and oxygen are mostly found in the same ratio as in water i.e. 2:1 and thus called “Hydrated carbons” They are found about 1% by weight and generally called Sugars or saccharides” due to their sweet taste except polysaccharides.

CLASSIFICATION OF CARBOHYDRATES

The carbohydrates can be classified into following groups on the basis of number of monomers.

1. Monosaccharide

2. Oligosaccharides

3. Polysaccharides.

(1) MONOSACCHARIDES

• These are called “Simple Sugars”, because they can not be hydrolysed further into simple sugars.

• Their general formula is “Cn H2n On

• They are white crystalline solids with sweet taste and soluble in water.

• They are present in various fruits and vegetables.

E.g: Glucose, Galactose, Fructose and Ribose etc. Monosaccharide can be sub-classified according to umber of carbon atom present in each molecule. They may be triose, (Glycerose), tetrose (erythrose), pentose, (ribose), hexone (glucose) or heptose (Glucoheptose) having 3,4,5 ,6 and 7 carbon atoms respectively.

(2) OLIGOSACCHARIDES

• These carbohydrates yield 2to 10 monosaccharides mnolecules on hydrolysis

• Disaccharides are the most common and abundant carbohydrates of oligosaccharides.

• These sugars are comparatively less sweet in taste, and less soluble in water.

E.g: Maltose, Sucrose and lactose etc.

(3) POLYSACCHARIDES

• These are the most complex and most abundant carbohydrates in nature.

• They are of high molecular weight carbohydrate which on hydrolysis yield mainly monosaccarides or products related to monosaccharide.

• These sugars are formed by the condensation of hundreds of thousands of monosaccharide units.

• They are tasteless and only sparingly souble in H2O.

E.g: Strach, cellulose Glycogen , Dextrin Agar, pectin and Chitin etc.

FUNCTIONS OF CARBOHYDRATES

• Carbohydrates are the potential source of energy.

• They act as storage food molecules and also work as an excellent building, protective and supporting structure.

• They also form complex conjugated molecules.

• They are needed to synthesize lubricants and are also needed to prepare the nectar in some flowers.

LIPIDS

These are naturally occurring compounds, which are insoluble in water but soluble in organic solvents. They contain carbon, hydrogen and oxygen like carbohydrates rate but in much lesser ratio of oxygen than carbohydrates. These biomolecules are widely distributed among plants and animals.

CLASSIFICATION OF LIPIDS

Following are the important groups of lipids.

1. Acylglycerol (fats and oil)

2. Waxes

3. Phospholipids.

4. Terpenoids.

(1) ACYLGLYCEROL (FATS AND OIL)

• These are found in animals and plants, provide energy for different metabolic activates and are very rich in chemical energy.

• They are composed of glycerol and fatty acids. The most widely spread acylglycerol is triacyl glycerol, also called triglycerides or natural lipids.

• There are two types of acylgycerol

(A) SATURATED ACYLGLYCEROL

• They contain no double bond.

• They melt at higher temperature than unsatured acylglycerols.

• Lipids containing saturated acylgycerol are solid and known as Saturated lipids.

E.g: Butter and Animal fat. etc.

(B) UNSATURATED ACYLGLYCEROL

• They contain unsaturated fatty acids i.e they contain one or more than one double bond between carbon atom(C=C-).

• They are liquid at ordinary temperature .

• They are found in plant also called “Oil”

E.g: linolin found in cotton seeds etc.

(2) WAXES

Chemically waxes are mixtures of long chain alkanes and alcohols. Ketones and esters of long chain fathy acids

• Waxes are widespread as protective coatings of fruits and leaves some insects also secrete wax.

• Waxes protect plants form water loss and abrasive damage.

• They also provide water barrier for insects, birds and animals etc.

(3) PHOSPHOLIPIDS

• It is most important class of lipids from biological point of view and is similar to riacylglycerol or an oil except that one fatty acid is replaced by phosphate group.

• The molecule of phospholipids consist of two ends, which are called hydrophilic (water loving end (head) and hydrophobic (water fearing)end (Tail).

• These are frequently associated with membranes and are related to vital functions such as regulation of cell permeability and transport process.

(4) TERPENOIDS

• It is large and important class of lipids containing “Isoprenoid “ unit (C5H8).

• They help in oxidation reduction process, act as components of essential oils of plants and also found in cell membrances as “cholesterol

SUB-CLASSES OF LIPIDS

1. Terpenes

2. Steroids.

3. Carotenoids.

(1) TERPENES

• This group based only on “Isoprenoid” unit and they are usually volatile in nature produce special fragrance.

• Derivatives of this group are found in vitamin A and are also important constituents of chlorophyll and cholesterol biosynthesis.

• They are utilized in synthesis of “Rubber” and “Latex”, and some of these are used in perfumes.

(2) STEROIDS

This group of Terpenoids contains 17 carbon atoms ring called “steroid nucleus”.

(3) CAROTENOIDS

They consist of fatty acid like carbon chain and usually found in plants, for example carotene, xanthophylls etc.

NUCLEIC ACIDS

Nucleic Acids Were First Isolated In 1870 By an Austrian Physician Fridrich Micscher from the nuclei of pus cells. These bio molecules are acidic in nature and present in the nucleus.

TYPES OF NUCLEIC ACIDS

Nucleic acids are of two types.

1. Deoxyribonucleic acid or DNA

2. Ribonucleic acid or RNA

CHEMICAL NATURE OF NUCLEIC ACID

Nucleic acids are complex substances. They are polymers of units called nucleotides. DNA is made up of deoxyribonucleotides, while RNA is composed of ribo nucleotides.

STRUCTURE OF NUCLEOTIDE

Each nucleotide is made of three subunits

a) 5-carbon monosaccharide (a pentose sugar)

b) Nitrogen containing base.

c) Phosphoric acid.

(A) PENTOSE SUGAR

Pentose sugar in RNA is ribose, while in DNA it is deoxyribose.

(B) NITROGENOUS BASE

Nitrogenous bases are of two types

(I) PYRIMIDINES (SINGLE RINGED): These are cytosine (abbreviated as C), thymine (abbreviated as T), and uracil (abbreviated as U).

(II) PURINES (DOUBLE RINGED): These are adenine (abbreviated as A) and guanine(abbreviated as G).

C) PHOSPHORIC ACID

Phosphoric acid (H3PO4) has the ability to develop ester linkage with OH group of pentose sugar.

FORMATION OF NUCLEOTIDE

Formation of nucleotide takes place in two steps. First the mitrogenous base combines with pentose sugar at its first carbon to form a “Nucleoside”. In second step the phosphoric acid combines with the 5th carbon of pentose sugar to form a “Nucleotide”.

(A) MONONUCLEOTIDES

• They exist singly in the cell or as a part of other molecules.

• These are not the part of DNA or RNA and some of these have extra phosphate groups e.g ATP.

B) DINCULEOTIDES

These nucleotides are covalently bounded together and usually act as co-enzymes

E.g NAD (Nicotinamide dinucleotide ).

(C) POLYNUCLEOTIDES

• Nucleotides are found in the nucleic acid as “Polynucleotide” and they have a variety of role in living organisms.

• They usually perform the function of transmitters of genetic information.

CONJUGATED MOLECULES

• Two different molecules, belonging to different categories, usually combine together to form “Conjugated molecules”.

• These conjugated molecules are not only of structural, but also are of functional significance.

• They play an important role in regulation of gene expression.

(A) GLYCOPROTEIN AND GLYCOLIPIDS

Carbolydrates may combine with proteins to form glycoprotein or with lipids to form glycolipid.

FUNCTIONS

a) Most of cellular secretions are glycoprotein’s in nature.

b)Both glycoproteins and glycolipids are integral structural components of plasma membranes.

(B) LIPOPROTEINS

Combination of lipids and proteins form lipoproteins.

FUNCTION

They are basic structural framework of all types of membranes in the cells.

(C) NUCLEOPROTEINS

Nucleic acids have special affinity for basic proteins . they are combined together to form nucleoproteins.

FUNCTIONS

The nucleoproteins (Histone) are present in chromosomes.

THINGS TO BE REMEMBER

• Proteins-Berzelius and G.J murlder.

• Lipids-Bloor in 1943.

• DNA –Hereditary material.

• RNA- carrier of genetic information.

• rRNA – (Ribosomal RNA)- Double stranded.

• Transcription- Formation of mRNA.

• Translation –Formation of Proteins by ribosmes.

IX English - Chapter 2 - Shah Abdul Latif

Question and Answers

Q.1 Who was Shah Abdul Latif? Where and when was he born?

Ans. Shah Abdul Latif was a great saint who is lovingly called "Lal Latif" by his devotees. He was born in a small village called "Hala Haveli" in the year 1689.


Q.2 What do you know about the ancestors of Shah Abdul Latif?

Ans. Shah Abdul Latif's ancestors had migrated to Sindh during the days of Tamerlane. They had come from Hiirat a town in West Afghanistan. They liked Sindh so much so that they decided to make it their permanent home. Many centuries later one of their decendants, Syed Habib Shah, was blessed with a son who grew up to be "Saint Lal Latif".


Q.3 Why is Shah Latif known as "Saint of Bhit"?

Ans. When Shah Latif father died, he left his home and went to live on a Mound at some distance from his village. A mound of sand is called "Bhit" in Sindhi. Due to the fact that he lived on this mound for the rest of his life, Shah Latif came to be known as "The Saint of Bhit."


Q.4 Name the shrines of saints found in Pakistan.

Ans. In every part of our country, there are shrines of such saints:

* In Lahore, The shrines of Data Ganj Bakhsh and Mian Mir Sahib.

* In Pak Pattan, Lived and Died Baba Fareed.

* In Multan, The Shrine of Ghoues Bahaul Haq.

* In Sindh, the Shrines of Shah Abdul Latif and Qalander Lal Shahbaz.

* In Peshawar, in Quetta, and in countless other towns and cities there are the tombs of these man of God.


Q.5 What are the important features of Shah Latif poetry?

Ans. The important features of Shah Latif's poetry is that it is written in the language of the common people, and other great quality of his poetry beside its simplicity is its moving music.

Q.6 What is the message of Shah Latif's poetry? or What according Shah Latif is the goal of life?

Ans. The message of Shah Latif is the message of love. He believed in the brotherhood and equality of men and in pleasing God by good deeds. This according to Shah Latif is the goal of life.


Q.7 When is the Urs of Shah Abdul Latif's held?

Ans. Shah Abdul Latif Urs is held at his shrine every year on 14th Safar, the second, month of the muslim calender.


Q.8 How do Shah Latif's devotees celebrate his Urs?

Ans. Shah Latif's Urs is held at his shrine every year in 14th Safar, the second month of the Muslim calender. Thousands of people gather to listen to the Saint's song sung to the Tambooro and after their prayers. Many learned men read papers that tell about Latif's life and poetry.


Q.9 What do you know about Shah Latif's music?

Ans. Shah Latif was not only a saint and a poet but also a great musician. He found great comfort in music. His skill in this art enabled him to make many improvements and changes in the difficult music of his time. He loved simplicity in music and musical instruments. He did not agree with the idea that music should be difficult. So he made it simple and also vented on instrument called "Tambooro".


Q.10 What do you know about Tamboora?

Ans. The tambooro is a simple musical instrument invented by the Sufi, philosopher Shah Abdul Latif.


Q.11 Write a short note on the poetry of Shah Abdul Latif?

Ans. Shah Abdul Latif started composing poetry while he was only a boy. Shah Abdul Latif was a mystic poet. He was a versatile, genious and had attempted all aspects of poetry.

Shah Abdul Latif was a poet of the people and was successful in awakening them to the discovery of the truth of spiritual life. He had very deed sympathy for the poor and had expressed in his sentiments about them with great pathos and fubings.

His collection of poems was so valued that it was translated into many languages and is called "Risalo of Shah Latif."