Therefore, the greater the number of ions in the solution, the greater is the conductance. Conductivity of strong and weak electrolytes Fig. The flow of electric current through an electrolytic solution is called electrolytic conduction. Your email address will not be published. Required fields are marked *, The branch of science which deals with the production of electricity from energy released during spontaneous chemical reactions and the use of electrical energy to bring about non- spontaneous chemical transformations is called, The substance which can lose one or more electrons (i.e., get oxidised) is called, Zinc acts as a reducing agent or reductant while Cu, The substances which allow the passage of electric current are called, These are metallic substances which allow the electricity to pass through them without undergoing any chemical change. If the solute-solvent interactions are strong, the ions of the solute will be highly solvated and their electrical conductivity will be low. Slightly ionized substances are weak electrolytes. When a current is applied to an aqeous solution, strong electrolyte solutions light up a light bulb, weak electrolyte solutions dimly light a bulb, and nonelectrolyte solutions do not light a bulb. Filed Under: Chemistry, Class 12, Electro Chemistry. Author of this website, Mrs Shilpi Nagpal is MSc (Hons, Chemistry) and BSc (Hons, Chemistry) from Delhi University, B.Ed (I. P. University) and has many years of experience in teaching. Find out more about how we use your information in our Privacy Policy and Cookie Policy. On this basis , electrolytes are broadly divided into two types : strong electrolytes and weak ... With increase in temperature, the conductivity of an electrolyte increases. The substance which can lose one or more electrons (i.e., get oxidised) is called reducing agent or reductant while the substance which can gain one or more electrons (i.e, get reduced) is called oxidising agent or oxidant. Thus, in a  redox reaction, one substance acts as a reducing agent and itself gets oxidised while another substance acts as an oxidising agent and itself gets reduced. A strong electrolyte is a compound that can completely dissociate into its ions when dissolved in water. about Citric acid vs. Hydrochloric acid Concentration and Conductivity, about Conductivity of Strong Electrolytes, Weak Electrolytes, and Non-Electrolytes Presentation, about Strong Acid Dissociation and Weak Acid Equilibrium Video, about Migration of ions During a Conductivity Test of NaCl(aq) Computer Animation, about Conductivity Testing of Electrolytes Computer Simulation, about Dissolving an ionic salt in water Computer Simulation and Computer Animation, about Dissolving Ionic Salts in Water Demonstration, about Conductivity of Electrolytes Demonstration, Conductivity of Strong Electrolytes, Weak Electrolytes, and Non-Electrolytes Presentation, Lecture Presentation Power Point Slides to Accompany Demonstrations, Strong Acid Dissociation and Weak Acid Equilibrium Video, Dissolving an ionic salt in water Computer Simulation and Computer Animation, Dissolving Ionic Salts in Water Demonstration, Conductivity of Electrolytes Demonstration, CIDER Communications in Chemistry Education, Identification of physical and chemical processess. The flow of electric current through metallic conductors is due to the flow of electrons in the metal atoms. It increases with increase in temperature. In these reactions, electrons are transferred from one reactant to another. It involves the transfer of matter as ions. Therefore, it is also called ionic conductance. (ii) Nature of the solvent: Electrolytes ionize more in polar solvents.Therefore greater the polarity of the solvent, larger is the ionization and hence greater is the conductance. The best conductors are metals such as copper, silver, tin, etc. Key Terms: Acids, Bases, Electrolytes, Salts, Strong Electrolytes, Weak Electrolytes. For example: A redox reaction is the reaction between zinc and copper (II) salt occurring in a battery. It does not involve the transfer of any matter. A thermomters measures the intitial temperature of the water and the final temperature of the resultant solution. Oxidation is a process which involves loss of electrons and reduction is a process which involves gain of electrons. Weak electrolytes, dissociate to only small extents and give lesser number of ions. Set-up and procedure Perform the experimental set-up according to Fig. About Mrs Shilpi Nagpal. 1. Zinc acts as a reducing agent or reductant while Cu2+ ions act  as oxidising agent or oxidant. In this type of conduction, charge is carried by ions. Compares conductivity of strong and weak acids and bases. Some other examples of redox reactions are, 5Fe2+ +8 H+ MnO4‾ ———> 5 Fe3+ + Mn2+ + 4 H2O. Using these two solutions proved useful to show that strong electrolytes are stronger conductors than weak electrolytes. Your email address will not be published. Some common examples of insulators are rubber, glass, ceramics, wood, wax, etc. The limiting molar conductivity (⋀ m 0 ) for strong and weak elctrolyte can be determined by using Kohlrauch's law which states that "the limiting molar conductivity of an electrolyte can be represented as the sum of the individual contributions of the anion and cation of the electrolyte." We and our partners will store and/or access information on your device through the use of cookies and similar technologies, to display personalised ads and content, for ad and content measurement, audience insights and product development. UO Libraries Interactive Media Group, Citric acid vs. Hydrochloric acid Concentration and Conductivity, Migration of ions During a Conductivity Test of NaCl(aq) Computer Animation, Conductivity Testing of Electrolytes Computer Simulation. In weak electrolytes, an equilibrium is established between the unionised electrolyte and the ions formed in solution. If the solute-solute interactions are large, the extent of dissociation will be less. The average kinetic energy of the ions of the electrolyte increases with increase in temperature. You can change your choices at any time by visiting Your Privacy Controls. For example: CH3COOH, H2CO3, H3BO3, HCN, HgCl2, ZnCl2, NH4OH, etc. (ii) Viscosity of the solvent: The viscosity of the solvent depends upon the solvent-solvent interactions. The reactions which involve both oxidation and reduction are called redox reactions. In this experiment, the differing behaviors of strong and weak electrolytes with regard to conductivity was studied. (1) Strong electrolytes: The electrolytes which are almost completely dissociated into ions in solution are called strong electrolytes. Conductivity of electrolytic (or ionic) solution depends upon the following factors: (i) Nature of electrolyte: The conductance of an electrolyte depends upon the number of ions present in the solution. With increase in temperature, the conductivity of an electrolyte increases. Electrical conductance through metals is called metallic conductance or electronic conductance. (3) the density of metal and Therefore, these substances do not conduct electricity in the solid state but conduct electricity in the molten state or in their aqueous solutions due to the movement of ions. The current, if sufficient enough, will light one or both LEDs on a conductivity meter, shown at right. (2) Weak electrolytes: The electrolytes which do not ionise completely in solution are called weak electrolytes. Information about your device and internet connection, including your IP address, Browsing and search activity while using Verizon Media websites and apps. These interactions are also responsible for the classification of electrolytes as strong electrolytes and weak electrolytes.