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Anti markovnikov rule describes that in addition to reactions of alkenes or alkynes,the proton is added to carbon atom that has least number of hydrogen atoms to it.

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Aditya . 2 years, 9 months ago

Anti Markovnikov rule describes that in addition to reactions of alkenes or alkynes, the proton is added to the carbon atom that has the least number of hydrogen atoms attached to it.

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-OCH3 group_______ the benzene ring towards electrophilic substitution reaction

Posted by Saumya Mishra -Ganpati Classes 2 years, 9 months ago

CBSE > Class 11 > Chemistry

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How to control exhaustive chlorination?

Posted by Mns Tyagi 2 years, 9 months ago

CBSE > Class 11 > Chemistry

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EQUILIBRIUM 231 SUMMARY When the number of molecules leaving the liquid to vapour equals the number of molecules returning to the liquid from vapour, equilibrium is said to be attained and is dynamic in nature. Equilibrium can be established for both physical and chemical processes and at this stage rate of forward and reverse reactions are equal. Equilibrium constant, Kc is expressed as the concentration of products divided by reactants, each term raised to the stoichiometric coefficient. For reaction, a A + b B c C +d D Kc = [C]c [D]d /[A]a [B]b Equilibrium constant has constant value at a fixed temperature and at this stage all the macroscopic properties such as concentration, pressure, etc. become constant. For a gaseous reaction equilibrium constant is expressed as Kp and is written by replacing concentration terms by partial pressures in Kc expression. The direction of reaction can be predicted by reaction quotient Qc which is equal to Kc at equilibrium. Le Chatelier’s principle states that the change in any factor such as temperature, pressure, concentration, etc. will cause the equilibrium to shift in such a direction so as to reduce or counteract the effect of the change. It can be used to study the effect of various factors such as temperature, concentration, pressure, catalyst and inert gases on the direction of equilibrium and to control the yield of products by controlling these factors. Catalyst does not effect the equilibrium composition of a reaction mixture but increases the rate of chemical reaction by making available a new lower energy pathway for conversion of reactants to products and vice-versa. All substances that conduct electricity in aqueous solutions are called electrolytes. Acids, bases and salts are electrolytes and the conduction of electricity by their aqueous solutions is due to anions and cations produced by the dissociation or ionization of electrolytes in aqueous solution. The strong electrolytes are completely dissociated. In weak electrolytes there is equilibrium between the ions and the unionized electrolyte molecules. According to Arrhenius, acids give hydrogen ions while bases produce hydroxyl ions in their aqueous solutions. Brönsted-Lowry on the other hand, defined an acid as a proton donor and a base as a proton acceptor. When a Brönsted-Lowry acid reacts with a base, it produces its conjugate base and a conjugate acid corresponding to the base with which it reacts. Thus a conjugate pair of acid-base differs only by one proton. Lewis further generalised the definition of an acid as an electron pair acceptor and a base as an electron pair donor. The expressions for ionization (equilibrium) constants of weak acids (Ka ) and weak bases (Kb ) are developed using Arrhenius definition. The degree of ionization and its dependence on concentration and common ion are discussed. The pH scale (pH = -log[H+ ]) for the hydrogen ion concentration (activity) has been introduced and extended to other quantities (pOH = – log[OH– ]) ; pKa = –log[Ka ] ; pKb = –log[Kb ]; and pKw = –log[Kw ] etc.). The ionization of water has been considered and we note that the equation: pH + pOH = pKw is always satisfied. The salts of strong acid and weak base, weak acid and strong base, and weak acid and weak base undergo hydrolysis in aqueous solution.The definition of buffer solutions, and their importance are discussed briefly. The solubility equilibrium of sparingly soluble salts is discussed and the equilibrium constant is introduced as solubility product constant (Ksp ). Its relationship with solubility of the salt is established. The conditions of precipitation of the salt from their solutions or their dissolution in water are worked out. The role of common ion and the solubility of sparingly soluble salts is also discussed. 2020-21

Posted by Mukul Kumar 2 years, 9 months ago

CBSE > Class 11 > Chemistry

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Ashutosh Singh 2 years, 9 months ago

Thoda Chhota likh dete to achha hota

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Kinetic molecular theory

Posted by Vishal Siva 2 years, 9 months ago

CBSE > Class 11 > Chemistry

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Reagents list

Posted by Vaikunta Revathi 2 years, 9 months ago

CBSE > Class 11 > Chemistry

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Oxidation list

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CBSE > Class 11 > Chemistry

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The salt that is added to table salt to make it flow freely in rainy season is (a) KCl (b) KI (c) Ca3(PO4)2 (d) Na3PO4

Posted by Md Zeeshan 2 years, 9 months ago

CBSE > Class 11 > Chemistry

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Give the relationship between ∆U and∆H for gases

Posted by Rajkumar Singh 2 years, 9 months ago

CBSE > Class 11 > Chemistry

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Harmanpreet Kaur 2 years, 9 months ago

∆H=∆U+∆ngRT

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Rajkumar Singh 2 years, 9 months ago

Answer

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Please suggest some amazing and beautiful places in the world... where we should have travel...??

Posted by Ronita 🤟 2 years, 9 months ago

CBSE > Class 11 > Chemistry

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Akshat Gupta 2 years, 9 months ago

My insta id

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I M Unknown 2 years, 9 months ago

Go To Hell

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Ronita 🤟 2 years, 9 months ago

Please tell according to your experience..and knowledge..

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How to do numericals of g= log k

Posted by Lakhvir Kaur 2 years, 9 months ago

CBSE > Class 11 > Chemistry

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G.Venkata Ajay Ajay 2 years, 9 months ago

Write about Bohr therou

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When hydrogen bond were formed

Posted by Anish Thakur 2 years, 9 months ago

CBSE > Class 11 > Chemistry

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Shamsiya Shafeek 2 years, 9 months ago

The Attraction force between two ions i.e one highly electronegative(N.F.O) and other one is hydrogen this is Hydrogen Bonding.This is the strongest Intermolecular Force.Example H2O,HF

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Give the relationship between Delta H and Delta U for gases

Posted by Nandini Rana 2 years, 9 months ago

CBSE > Class 11 > Chemistry