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  Introduction  
  • Temperature and Heat
Temperature is defined as the degree of hotness or coldness of a body. It is a scalar quantity Its S.I. unit is kelvin (K). Heat is a form of energy -which causes sensation of hotness or coldness. The flow of heat is always from higher temperature to lower temperature. No heat flows from one body to other, when both the bodies are at the same temperature. The two bodies are said to be in thermal equilibrium. The SI unit of heat is joule. Its CGS unit is calorie, 1 cal = 4.2 joule
  • Measurement of Temperature
A branch of science which deals with the measurement of temperature of a substance is called thermometry. Thermometer is a device used to measure the temperature. Thermometer used for measuring very high temperatures are called pyrometer.
  • Relationship between Different Scales of Temperature
\[\frac{C-0}{100}=\frac{F-32}{212-32}=\frac{K-273.16}{373.16-273.16}\]=\[\frac{R-0}{80-0}=\frac{Ra-460}{672-460}\]\[{{T}^{0}}(K)=({{t}^{0}}C+273.16)\] Normal temperature of human body is 310.15 K\[({{37}^{0}}C={{98.6}^{0}}F)\] STP or NTP implies 273.15 K \[({{0}^{0}}C={{32}^{0}}F)\]
  • Ideal-gas Equation and Absolute Temperature
The equation,   PV= nRT where, n = number of moles in the sample of gas R = universal gas constant; (its value is 8.31\[J\,mo{{l}^{-1}}{{K}^{-1}}\]), is known as ideal-gas equation. It is the combination of following three laws (i) Boyle's law: When temperature is held constant, the pressure is inversely proportional to volume. i.e., \[P\propto \frac{1}{V}\](at constant temperature) (ii) Charters law: When the pressure is held constant, the volume of the gas is directly porportional to the absolute temperature. i.e., \[V\propto T\](at constant pressure) (iii) Avogadro's law: When the pressure and temperature are kept constant, the volume is directly proportional to the number of moles of the ideal gas in the container. i.e., \[V\propto n\](at constant pressure and temperature)
  • Absolute Temperature
The lowest temperature of\[-\,273.16{}^\circ C\] at which a gas is supposed to have zero volume and zero pressure and at which entire molecular motion stops is called absolute zero temperature. A new scale of temperature starting with \[-273.16{}^\circ C\]by Lord Kelvin as zero. This is called Kelvin scale or absolute scale of temperature. \[T\left( K \right)=t{}^\circ C+273.16\]   Thermal Expansion   The increase in the dimensions of a body due to the increase in its temperature is called thermal expansion.
  • Linear expansion: The fractional increase in length per \[{}^\circ C\] rise in temperature is called coefficient of linear expansion. Coefficient of linear expansion, \[\alpha =\frac{\left( \frac{\Delta \ell }{\ell } \right)}{\Delta T}=\frac{d\ell }{\ell dT}\]
 
  • Superficial expansion: On increasing the temperature of a solid, its area increases. This increase in area is referred as superficial expansion. Coefficient a/superficial expansion is defined as the fractional increase in area per \[{}^\circ C\]rise in temperature. i.e., Coefficient of a real expansion \[\beta =\frac{\Delta A/A}{\Delta T}=\frac{dA}{AdT}\]
  • Cubical expansion: On increasing the temperature of a solid, its volume increases. This increase in volume with increase in temperature is called cubical more...

  Introduction  
  • Periodic Motion
Any motion that repeats itself in equal intervals of time is called periodic motion. Aperiodic motion can be represented in terms of sines and cosines, so it is called a harmonic motion. The uniformly rotating earth represents a periodic motion that repeats itself at every 24 hours.  
  • Simple Harmonic Motion (S.H.M.)
Oscillatory motion in which the acceleration of the particle is directly proportional to the displacement and directs towards a fixed point in a direction opposite to displacement is called simple harmonic motion abbreviated as S.H.M. If a particle performs oscillatory motion such that its acceleration (a) and displacement (x) are related as below\[a\propto -x\], then the motion of particle is simple harmonic. An oscillatory motion is always periodic but a periodic motion may not be oscillatory. Examples of S.H.M. (i) clock pendulum, (ii) oscillating liquid in a U-tube, (iii) oscillating block in a liquid, (iv) oscillating frictionless piston fitted in a cylinder filled with ideal gas, etc.            
  • Sound
Sound is a form of energy which produces a sensation of hearing in our ears.
  • Source of Sound and its Propagation
A source of vibration (vibration means a kind of rapid to and fro motion of an object) is normally a source of sound. When we pluck a string of guitar or sitar or veena it produces sound. Similarly vibrations of wings of bee or mosquito. Sound is emitted by vibrating source and is transmitted through a material medium producing sensation of hearing in our ears. The motion of a vibrating source sets up waves in the surrounding medium.
  • Sound Needs a Material Medium for its Propagation
In the absence of medium (air) around the source, sound is not being propagated and light (electromagnetic) waves travel through the vacuum.   Mechanical Waves  
  • A mechanical wave is a periodic disturbance which requires a material medium for its propagation. The properties of these waves depend on the medium so they are known as elastic waves, such as sound-waves, water waves, Waves in stretched string. On the basis of motion of particles the mechanical waves are classified into two parts.
  • Transverse wave: When the particles of the medium vibrate in a direction perpendicular to the direction of propagation of the wave, the wave is known as the transverse wave. For example, waves produced in a stretched string, waves on the surface. These waves travel inform of crests and troughs. These waves can travel in solids and liquids only.
  • Longitudinal wave: When the particles of the medium vibrate along the direction of propagation of the wave then the wave is known as the longitudinal wave. For example sound wave in air, waves in a solid rod produced by scrabbing etc. These waves travel in the form of more...

  Introduction  
  • Optics
The branch of physics which deals with the propagation, nature and behaviour of light is known as optics.  
  • Light
Light is a form of energy -which enables human beings and creatures to 'see' things. When light emitted from an object or reflected from the object enters our eyes we are able to see the object. We can't see an object in dark even if we are in light because there is no light coming from the object to our eyes. Light is an electromagnetic radiation which exhibits properties like a wave as well as a particle. It always propagates in a straight line. Light travels with a speed nearly equal to\[3\times {{10}^{8}}m/s\]According to current theories, no material particle can travel at a speed greater than the speed of light.  
  • Luminous and Non-luminous Objects
Luminous objects are those which emit its own light e.g., sun, glowworm, burning candle, electric lights. Non-luminous objects do not give out its own light but are visible only when light from a luminous object falls on it. e.g., moon, earth, table, paper, etc.  
  • Transparent Translucent and Opaque materials
Transparent materials are those which allow most of light to pass through them. Example: Glass, water, air. Translucent materials allow only a part of light to pass through it. We cannot see distinctly through them. Example: greased paper, Paraffin wax, etc. Opaque materials: do not allow any light to pass through it. They reflect or absorb all the light that falls on them. Example: Books, desk, stone, rubber, trees, etc.   Reflection of Light  
  • Reflection of Light: When light hits an opaque material, the light may be absorbed by the material and converted into heat energy. If light is not absorbed, it is bounced back or reflected at the surface of material. The turning back of light in the same medium is called reflection of light.
  • Laws of reflection
  • The angle of incidence ‘i’ is equal to the angle of reflection ‘r’
  • At the point of incidence, the incident rays, the normal to the surface and the reflected ray all lie in the same plane.
  •  
    • Reflection by Plane Mirrors
    Plane mirror is a looking glass which is highly polished on one surface and is silvered on the other surface. When a light ray strikes the polished surface, it is reflected by the silvered surface. An 'image' is defined as the impression of an object carried over and formed by light reflected from it.
    • Use of plane mirrors
    (a) Plane mirrors are primarily used as looking glasses. (b) Since, a combination of mirrors can produce multiple images, they are used to provide false dimensions in showrooms. (c) They are also used as reflectors in solar cookers. (d) Plane mirrors are used in more...

      Introduction  
    • Electric Charges
    Charge is something associated with matter due to which it produces and experiences electric and magnetic effects. The study of charges at rest is called static electricity or electrostatics while the study of charges in motion is called current electricity. There are two types of electric charge: (i) Positive charge and (ii) Negative charge. The magnitude of elementary positive or negative charge is same and is equal to. \[1.6\times {{10}^{-19}}C\] Charge is a scalar quantity its SI unit is ampere second or coulomb.
    • Basic Properties of Electric Charge
    (1)  Similar charges repel and opposite charges attract. (2)  A charged body attracts light uncharged bodies. (3)  Accelerated charge radiates energy.  
    • Conductors and Insulators
    The materials which allow electric charge (or electricity) to flow freely through them are called conductors. Metals are very good conductors of electric charge. Silver, copper and aluminium are some of tile good conductors of electricity. The materials which do not allow electric charge to flow through them are called nonconductors or insulators. For example, most plastics, rubber, non-metals (except graphite), dry wood, wax, mica, porcelain, dry air etc., are insulators.  
    • Coulomb's Law
    It states that, the electrostatic force of interaction (repulsion or attraction) between two electric charges \[{{q}_{1}}\] and \[{{q}_{2}}\]separated by a distance r, is directly proportional to the product of the charges and inversely proportional to the square of distance between them. \[F\propto {{q}_{1}}{{q}_{2}}\] and \[F\propto 1/{{r}^{2}}\] or  \[F=k\frac{{{q}_{1}}{{q}_{2}}}{{{r}^{2}}}\] \[K=\frac{1}{4\pi {{\varepsilon }_{0}}}\]\[=9\times {{10}^{9}}\frac{N{{m}^{2}}}{cou{{l}^{2}}}\Rightarrow {{\varepsilon }_{0}}=8.85\times {{10}^{-12}}\frac{cou{{l}^{2}}}{N{{m}^{2}}}\] ² Electric Field  
    • Electric Field: The region surrounding an electric charge or a group of charges in which another charge experiences a force of attraction or repulsion is called 'electric field'. \[\overrightarrow{E}=\frac{\overrightarrow{F}}{{{q}_{0}}},\overrightarrow{E}=\underset{{{q}_{0}}\to 0}{\mathop{\lim }}\,\frac{\overrightarrow{F}}{{{q}_{0}}}\] The S.L unit of electric field intensity is N/coul or volt/metre.
    • Electric Lines of Force
    An electric line of force is that imaginary smooth curve drawn in an electric field along which a free isolated unit positive charge moves. Two lines offeree never intersect. If they are assumed to intersect, there will be two directions of electric field at the point of intersection, which is impossible.  
    • Electric Flux ((\[\phi \])
    The total number of electric lines of force through a given area is called the electric flux. (a) For open surface, \[{{\phi }_{0}}=\int{d\phi =\int{\overrightarrow{E}.d\overrightarrow{s}}}\] (b) For closed surface, \[{{\phi }_{0}}=\oint{\overrightarrow{E}.d\overrightarrow{s}}\]
    • Gauss's Law
    The total electric flux linked with a closed surface is \[\left( \frac{1}{{{\varepsilon }_{0}}} \right)\] times the charge enclosed by the closed surface (Gaussian surface), i.e. \[\oint{\overrightarrow{E}.d\overrightarrow{s}=\frac{q}{{{\varepsilon }_{0}}}}\]
    • Electrostatic Potential
    Potential at a point can be physically interpreted as the work done by the field in displacing a unit + ve charge from some reference point to the given point. i.e., \[V=\frac{w}{{{q}_{0}}}\] \[V=-\int\limits_{\infty }^{r}{\overrightarrow{E}.d\overrightarrow{s}}\] i.e. more...

      Magnetism  
    • Magnetism: The phenomenon of attracting magnetic substances like iron, cobalt, nickel etc. is called magnetism. A body possessing the property of magnetism is called magnet. Lodestone or magnetite is natural magnet. Earth is also a natural magnet. In magnetized substance all the atomic magnets are aligned in same direction and thus resultant magnetism is non-zero.
      ·      
    • Bar Magnet
    A bar magnet consists of two equal and opposite magnetic poles separated by a small distance. Poles are not exactly at the ends. The shortest distance between two poles is called effective length (\[{{L}_{e}}\]) and is less than its geometric length (\[{{L}_{g}}\]). For bar magnet \[{{L}_{g}}=2l\]and\[{{L}_{e}}=(5/6){{L}_{g}}\]  
    • Properties of Magnet
    (i) Attractive property: When a magnet is dipped into iron fillings it is found that the concentration of iron filings, i.e., attracting power of the magnet is maximum at two points near the ends and minimum at the centre. The places where its attracting power is maximum are called poles. (ii) Directive property: When a magnet is suspended its length becomes parallel to N-S direction. The pole pointing north is called the north-pole while the other pointing in the geographical south is called the south pole of the magnet. The line joining the two poles of a magnet is called magnetic axis and the vertical plane passing through the axis of a freely suspended or pivoted magnet is called magnetic meridian. (iii) Poles of a magnet always exist in pairs: In a magnet the two poles are found to be equal in strength and opposite in nature. If a magnet is broken into number of pieces, each piece becomes a magnet with two equal and opposite poles. This shows that monopole do not exist. (iv) Repulsive property: A pole of a magnet attracts the opposite pole while repels similar pole.  
    • Demagnetisation of Magnet
    A magnet gets demagnetised, i.e., loses its power of attraction if it is heated, hammered or alternating current is passed through a wire wound over it.  
    • Permanent and Temporary Magnets (Electromagnets)
    The permanent artificial magnets are made of some metals and alloys like Carbon-steel, Alnico, Platinum-cobalt, Alcomax, Ticonal etc. The permanent magnets are made of ferromagnetic substances with large coercivity and retentivity. The temporary artificial magnets like electromagnets are prepared by passing current through coil wound on soft iron core. These cannot retain its strength for a long time. These are made from soft iron, non-metal and alloy. Electromagnets are stronger than permanent magnet.
    • Some Applications of Electromagnets
    (i)   Electric motors (ii)  Doorbells (iii) In scrapyards to separate iron from other metals  
    • Coulomb's Law in Magnetism
    more...

                   Introduction  
    • Metals, Semiconductors and Insulators
    On the basis of electrical conductivity\[(\sigma )\]or resistivity \[(\rho =1/\sigma )\] the solids are classified as (i) Metals - have low resistivity \[\rho \tilde{\ }{{10}^{-2}}\,to\,{{10}^{-8}}\Omega m\], \[\sigma \tilde{\ }{{10}^{2}}\,to\,{{10}^{8}}S{{m}^{-1}}\] (ii) Semiconductors - have intermediate resistivity \[\rho \tilde{\ }{{10}^{5}}\,to\,{{10}^{0}}\Omega {{m}^{{}}}\] \[\sigma \tilde{\ }{{10}^{-5}}\,to\,{{10}^{0}}S{{m}^{-1}}\] (iii) Insulators - have high resistivity \[\rho \tilde{\ }{{10}^{8}}\Omega {{m}^{{}}}\] \[\sigma \tilde{\ }{{10}^{-8}}S{{m}^{-1}}\] i.e. the Semiconductors are the materials whose conductivity is more than insulators but less than conductors.  
    • Types of Semiconductors
    Intrinsic semiconductors or pure semiconductors in semiconductors forbidden energy gap Eg is more than metals or conductors and less than insulators. Silicon (Si) and Germanium (Ge) are the examples of pure semi-conductors. In pure or intrinsic semiconductor, \[{{n}_{e}}={{n}_{h}}={{n}_{i}}\] Where\[{{n}_{e}}=no\].of electrons: \[{{n}_{h}}=no\]. Of holes and\[{{n}_{i}}=no\]. Of intrinsic carrier concentration. Impurity like pentavalent (As, Sb, P) or trivalent (In, B, Al) are added to increase conductivity. Depending on doping type we have (a) n- type semiconductor (b) p- type semiconductor (a) n - type semiconductor: Si or Ge with pentavalent doping. An atom of valency +5 occupies the position of parent atom in crystal lattice. Four valence electrons form 4 covalent bonds but 5th electron is free and weakly bound to parent atom. The ionisation energy (~ 0.01 V for Ge and 0.05V for Si) is small and even at room temperature the electron jumps to conduction band. The dopant is called donor impurity (positively charged). (b) p - type semiconductor: Si or Ge with trivalent doping means one less electron in the 4 covalent bonds, so the 4th neighbour has a vacancy or hole that can be occupied by an electron from another site. Thus a hole is available for conduction. The trivalent atom is negatively charged as it acquires an electron and is called acceptor atom or impurity.
    • Formation of p - n junction: Part of p-type can be converted into n - type by adding pentavalent impurity. There is concentration gradient between p and n sides, holes diffuse from p side to n side (\[(P\to n)\]and electrons move from \[(n\to p)\]creating a layer of positive and negative charges on n and p side respectively called depletion layer. External bias is applied to cause charges to flow.
          Symbol of p-n junction diode            p-n junction under forward bias: When p-side is connected to positive terminal and n - side to negative terminal of external voltage, it is said to be forward biased.   The applied voltage V is opposite to build in Potential\[{{V}_{0}}\], hence depletion layer width decreases and barrier height is reduced to\[({{V}_{0}}-V)\]. There is minority carrier injection, hence charges begin to flow. Current is in the order of mA. (c)  p-n junction under reverse bias: When p-side of p-n junction is connected to -ve terminal more...

    • Substance (or chemical substance):
    A "substance" is a kind of matter that can-not be separated into other kinds of matter by any physical process, e.g. gold, silver, iron, sodium chloride, calcium carbonate etc.
    • Pure substance:
    Is one that is a single substance and has a uniform composition. Such a substance always have the same texture and taste, e.g. water, salt, sugar etc.
    • Testing the purity of a substance:
    The purity of substance can easily be checked by checking its melting points in case of a solid substance or by checking its boiling points in case of a liquid substance.
    • Types of pure substances:
    Two different types of pure substances are (i) Element: An element is a substance which can-not be split up into two or more simpler substances by usual chemical methods of applying heat, light or electric energy, e. g. hydrogen, oxygen, sodium, chlorine etc. (ii) Compound: A compound is a substance made up of two or more elements chemically combined in a fixed ratio by weight e.g. \[{{H}_{2}}O\] (water), \[NaCl\](sodium chloride) etc.
    • Mixture:
    A mixture is a substance which consists of two or more elements or compounds not chemically combined together, e.g. Air is a mixture of nitrogen, oxygen, inert gases, water vapour, carbon dioxide etc.
    • Types of mixtures:
    Mixtures are impure substances. They are of two types: (i) Homogeneous mixture: It has a uniform composition throughout and its components can-not be distinguished visually. e.g. a well-mixed sample of vinegar. (ii) Heterogeneous mixture: It is one that is not uniform throughout. Different samples of a heterogeneous mixture may have different composition, e.g. a mixture of salt and pepper.
    • Solution:
    It is a homogeneous mixture of two or more substances whose composition can be varied, e.g. solution of common salt in water, solution of ammonia in water. Some other examples are lemonade, coke, pepsi etc.
    • Separating the components of a mixture:
    Various methods are used for separating the constituents of a mixture. Depending upon the type of mixture (i.e. whether it is a homogeneous mixture or heterogeneous mixture) different methods used are given below:
    Mixture Separation Method
    1. Insoluble solid in solvent Sedimentation followed by filtration. In case of a fine solid centrifugation is used instead of filtration
    2. Solution of solid in liquid Evaporation, crystallization, distillation
    3. Miscible mixture of liquids. Fractional distillation
    4. Immiscible mixture of liquids. Separating funnel
    5. Mixture of two solids one of which is sublime Sublimation more...
    • Law of conservation of mass: This law was stated by Lavoisier in 1744. It states that "In all physical and chemical changes, the total mass of readouts is equal to total mass of products."
    • Law of constant proportions (or constant composition): This law was first stated by Proust in 1797. According to the law "a chemical compound is always found to be made up of the same elements combined together in the same proportions by weight" e.g. the ratio of hydrogen and oxygen in pure water is always 1: 8 by weight. This law is also called law of definite proportions.
    • Law of multiple proportions: This law was given by John Dalton (1803) and states that "when two elements combine to form two or more compounds, the different mass of one of the elements and the fixed mass of the one with which it combines always form a whole number ratio". This law explains the concept of formation of more than one compound by two elements.
    • Dalton's Atomic theory: Postulates of Dalton s Atomic Theory
    (i) Matter is made up of extremely small indivisible particles called atoms. (ii) Atoms of the same substance are identical in all respects i.e., they possess same size, shape, mass, chemical properties etc. (iii) Atoms of different substances are different in all respects i.e., they possess different size, shape, mass etc. (iv) Atom is the smallest particle that takes part in a chemical reaction. (v) Atoms of different elements may combine with each other in a fixed simple, whole number ratio to form compound atoms. (vi) Atoms can neither be created nor destroyed i.e., atoms are indestructible.
    • Atom: It is the smallest particle of an element which can take part in a chemical change. It may or may not be capable of independent existence.
    • Symbol: The abbreviation used for lengthy names of elements are termed as their symbols. The symbol of an element is the first letter or the first and another letter of English name or Latin name of the element. While writing a symbol, the first letter is always capital and the second is always small.
    • Molecule: It is the smallest particle of an element or compound that is capable of independent existence and shows all the properties of that substance. [The molecules of an element is made up of only one and same type of atoms, while the molecule of a compound is made up of dissimilar atoms]
    • Atomicity: The number of atoms present in a molecule of an element or a compound is known as its atomicity. e.g. the atomicity of oxygen is 2 while atomicity ozone is 3.
    • Ion: It is an electrically charged atom or group of atom. It is formed by the loss or gain of electrons by an atom. Ions are of two types :
    • Cation: It is positively charged ion and is formed by the loss of electron from an atom e.g. \[{{H}^{+}},\]\[N{{a}^{+}},C{{a}^{2+}},A{{l}^{3+}}\]\[,NH_{4}^{+}\], more...

    Classification of Elements and Periodicity in Properties  
    • Classification means identifying similar species and grouping them together.
    • Lavoisier divided elements into two main types known as metals and non-metals.
    • Doberiner's Law of triads:
    According to this law, "in certain triads (group of three elements) the atomic mass of the central element was the arithmetic mean of the atomic masses of the other two elements.” But in some triads all the three elements possessed nearly the same atomic masses, therefore the law was rejected. e.g., atomic masses of Li, Na and K are respectively 7, 23 and 39, thus the mean of atomic masses of 1st and 3rd element is = 7 + 39 = 23
    • Limitations of Doberiner's Triads: He could identify only a few such triads and so the law could not gain importance. In the triad of Fe, Co, Ni, all the three elements have a nearly equal atomic mass and thus does not follow the above law.
    • Newland’s Law of octaves:
    According to this law "the elements are arranged in such a way that the eighth element starting from a given one has properties which are a repetition of those of the first if arranged in order of increasing atomic weight like the eight note of musical scale.)
    • Drawback of Newland’s law of octaves:
    (i) According to Newland only 56 elements exists in nature and no more elements would be discovered in the future. But later on several new element were discovered whose properties did not fit into law of octaves. (ii) In order to fit new elements into his table Newland adjust two elements in the same column, but put some unlike elements under the same column. Thus, Newland's classification was not accepted.
    • Mendeleev’s periodic table:
    Mendeleev arranged 63 elements known at that time in the periodic table. According to Mendeleev "the properties of the elements are a periodic function of their atomic masses." The table consists of eight vertical column called 'groups’ and horizontal rows called 'periods'.
    • Merits of Mendeleev's periodic table:
    (i) At some places the order of atomic weight was changed in order to justify the chemical and physical nature. (ii) Mendeleev left some gap for new elements which were not discovered at that time. (iii) One of the strengths of Mendeleev's periodic table was that, when inert gases were discovered they could be placed in a new group without disturbing the existing order.
    • Characteristics of the periodic table: Its main characteristics are:
    (i) In the periodic table, the elements are arranged in vertical rows called groups and horizontal rows called periods. (ii) There are eight groups indicated by Roman Numerals I, II, III, IV, V, VI, VII, VIII. The elements belonging to first seven groups have been divided into sub-groups designated as A and B on the basis a/similarities. The elements that are present on the left hand more...

      Introduction  
    • The term acid, in fact, comes from the Latin term acere, which means “Sour”. In everyday life we come across many compounds that chemists classify as acids. Bases are compounds which taste bitter eg. Milk of magnesia. Salts also have wide applications for example ammonium chloride is used as electrolyte in dry cells, sodium bicarbonote (baking powder) in the manufacture of glass etc.
      Properties of acids and bases  
    • A. Properties of acids
    • Chemical properties:
    (i) Action of metals: Metals generally react with dilute acids to form their respective salt and hydrogen. \[Metal+Acid\to Salt+Hydrogen\] (ii) Action with metal oxides (Basic oxides) Metal oxides are generally basic oxides. These oxides get neutralised when they react with acids. These reactions are mostly carried upon heating e.g. \[Basicoxide+Acid\to Salt+Water\] \[\left( Neutralization\text{ }reaction \right)\]   (iii) Action with metal carbonates and metal hydrogen carbonates Acids react with carbonates and hydrogen carbonates to form their respective salts, water and carbon dioxide gas. \[Carbonate/bicarbonate+Acid\to Salt+water+carbon\,\,dioxide.\]
    • B. Properties of bases
    • Chemical Properties:
    (i)  Reaction of metals with bases: Metals (e.g. Zn, Al, Sn) dissolve in NaOH (an alkali) to liberate hydrogen gas. \[Zn+2NaOH\to N{{a}_{2}}Zn{{O}_{2}}+{{H}_{2}}\] \[Sod.Zincate\] (ii) Action with acids: Bases combine with acids to form salt and water only. It is a neutralisation reaction.                                           \[Base+Acid\to Salt+Water\] Non - metallic oxides react in the same way hence non- metallic oxides are acidic in nature.
    • Strength of Acids and Bases
    The strength of an acid or a base can be easily estimated by making use of universal indicator which is a mixture of several indicators. The universal indicator show different colours at different concentrations of hydrogen ions in solution.   pH Scale  
    • pH Scale: It is a scale that is used for measuring \[{{H}^{+}}\] ion (Hydrogen ion) concentration of a solution. The term pH stands for "potential" of "hydrogen". It is the amount of hydrogen ions in a particular solution.
    For acids pH< 7 For bases pH > 7 For neutral substances pH = 7
    • Importance of pH in Daily Life
    (i) Blood pH: For proper functioning our body needs to maintain blood pH between 7.35 and 7.45. Values of blood pH greater than 7.8 or less than 6.8 often results in death. (ii) Acid rain: When pH of rain water is less than 5.6, it is called acid rain, when acid rain flows into rivers, it lowers the pH of river water. (iii) pH in our digestive system: We know that hydrochloric acid (HC1) produced in our stomach helps in digestion of food without harming stomach. However excess of acid causes indigestion and leads to pain as well as irritation. To get rid of this people use bases called "antacids". (iv) pH of the soil: For their healthy growth plants require a specific pH. Soils with high peat content or more...


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