ACID AND BASES Definition and properties of Acid: Acid is defined as a substance whose aqueous...
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ACID AND BASESDefinition and properties of Acid: Acid is defined as a substance whose aqueous solution possesses the following characteristic properties:1. It conducts electricity2. It reacts with active metal like zinc, magnesium etc to give hydrogen.3. It turns blue litmus red.4. It has sour taste.5. Its acidic properties disappear on reaction with a base.
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Definition and properties of Base: Base is defined as a substance whose aqueous solution possess the following characteristic properties:1. It conducts electricity2. It turns red litmus blue. 3. It has bitter taste. 4. It has soapy(slippery) touch.5. Its basic properties disappear on reaction with an acid.
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Arrhenius concept of acid and bases: It was proposed by Arrhenius in 1884.Arrhenius Concept of Acid : 1. An acid is defined as a substance which contains hydrogen ion.2. When dissolved in water it gives hydrogen ion.3. Example HC l(hydrochloric acid), HNO3 ( nitric acid).4.The acid which dissociate completely into H + and the negative ions are called strong acid. Example HCl, HNO3 .
HCl water H+(aq) + Cl- (aq)
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5. Some acid which do not dissociate completely into H+ ion and negative ion are called weak acid. Example CH3COOH(acetic acid),H2CO3(carbonic acid).
6. There is an equilibrium between ions and undissociated molecules.CH3COOH Water CH3COO- + H+
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Arrhenius Concept of Base : 1. A base is defined as a substance which contains hydroxyl group(OH-).2. When dissolved in water it gives hydroxyl (OH-)ion. Example NaOH (sodium hydroxide), NH4OH (ammonium hydroxide).3. The base which dissociate completely into OH -and the positive ions are called strong base. Example NaOH, KOH . NaOH water Na+(aq) + OH- (aq)4. Some base which do not dissociate completely into OH- ion and positive ion are called weak base. Example NH4OH and Al(OH)3.5. There is an equilibrium between ions and undissociated molecules.
NH4OH Water NH4+(aq) + OH-(aq)
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Neutralization process:1. It is the process in which hydrogen ions and hydroxide ions join to form unionized molecules of water.2. As a result of this properties of acids and base are destroyed. HCl ( water) H+(aq) + Cl- (aq)NaOH water Na+(aq) + OH- (aq)
ThereforeNa+(aq) + OH- (aq) + H+(aq) + Cl- (aq) Na+(aq) + Cl- (aq) + H2O
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Amphoteric substance :1. The substance which acts as both acid and base are called amphoteric or amphiprotic substance.
Example: Water is proton acceptor HCl + H2O H3O+ + Cl-
Example: Water is proton donor. NH3 + H2O NH4
+ + OH-
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Conjugate acid base pair1. A conjugate pair of acid and a base differs by a proton (H+) only. Conjugate acid Conjugate base + H+
Acid 1 Base2 Acid 2 Base1 HCl + H2O H3O+ + Cl-
H2O + NH3 NH4+ + OH
2. Acid 1 and Base1 are conjugate pair I ( for forward reaction).3. Acid 2 and Base2 are conjugate pair II ( backward reaction).
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Lewis concept of acid and base: 1. It was proposed by G.N.Lewis in 1923. 2. It is also called electronic concept.Lewis acid1.A Lewis acid is defined as a substance( an
atom, ion or molecule) which is capable of accepting a pair of electrons .
2.A Lewis acid is electron pair acceptor.Examples : BF3 , AlCl3 ( neutral molecules)
Examples : Ag+ , Cu+2,Fe+3 ( cations)
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Lewis base1. A Lewis base is defined as a substance( an
atom,ion or molecule) which is capable of donating a unshared pair of electrons .
2. A Lewis base is electron pair donor. Examples : NH3 , ROH,H2O, RNH2 ( neutral
molecules). Examples : F- , Cl-,CN- ,OH-,I-, Br - ( anions).Reaction between Lewis acid and Lewis base NH3 is a Lewis base (electron donor) and BF3 is a
Lewis acid (electron acceptor). Reaction between NH3 a Lewis base (electron donor) and BF3 a Lewis acid ( electron acceptor) can be shown as :
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Strength of Acid and Bases : pHThe pH and pOH scales provide a convenient way to express the acidity and basicity of dilute aqueous solutions. The pH and pOH of a solution are defined as as the negative logarithm of hydronium(H3O+) concentration in moles per litre.
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Where [ H3O+] represent the number of moles of [ H3O+] per litre.
Example: If in a solution [ H3O+] = 10 –x moles per litre. Now according the equation pH = - log [ H3O+] = - log 10 -x
= - ( - x log 10) = - (- x ) (as log 10 =1) = x
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Calculate the pH value of 10-2 molar HNO3solution.
HNO3 solution completely ionizes as
HNO3 + H2O H3O+ + NO3-
Now given [ H3O+] = [ HNO3] = 10-2 M
Therefore, pH= -log [ H3O+] = -log(10-2) = - (-2 x log 10) = 2
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pH scale:1 pH scale is from 0 to 14.2 Neutral solution has pH =7.3 pH of acid solution is always less than 7.4 pH of basic solution is always greater than 7.
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The self-ionization of water:
Water ionizes weakly to produce OH- and H+ ions, where Kw is the ionization constant of water, according to:
H2O(l) H+ (aq) + OH-(aq) Kw = 10-14
This means that the product of the concentration (molarity) of [H+] and [OH-] must always be 10-14 .
Kw = 10-14 = [H+] [OH-]
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pH and pOH
The concentration of [H+] and [OH-] can be expressed as the pH and pOH: (p in pH or pOH means ‘potency’, and means that any constant ‘K’ or concentration with a ‘p’ in front of it is represented as pK = -log K , or pH = -log [H+])
pH = - log [H+]pOH = - log [OH-]
We can show that:
pKw = 14.0 =pH + pOH