oo Sprint LTE × Workshop 12 Download 6:08 PM 4 of 5 Part 2. Electrolytes Solutio

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oo Sprint LTE × Workshop 12 Download 6:08 PM 4 of 5 Part 2. Electrolytes Solutions that contain ions will conduct electricity and are called electrolytes. In general the higher the concentration of lons in solution the better it will conduct electricity. When ionic solids (salts) dissolve in water they dissociate completely and hydrated positive and negative lons are formed. Salts that are solable in water are strong electrolytes because they dissociate completely in aqueous solution. Examples: Al:(S04)NH NO Commpounds that are soluble but only partially dissociate when dissolved in water will prodace relatively few ions in solution. Such compounds are poor conductors of electricity and are called weak electrolytes. Examples: H00s (carbonic acid), HF (hydrofluoric acid). We will learn more about behavior of such compounds next semester when we discuss Acid/Base chemistry. Finally, compounds that dissolve in water but produce no ions are called nonelectrolytes. Examples: CH CH:0H (ethanol), Ci(sugar). You will learn more about these compounds when you study organic chemistry A. Discuss with your group what it means partially dissociate and pick from the tree diagrams below the diagram that correctly models the behavior of the HFwhen it dissolves in water (water molecules are omitted for clarity). Please explain your choice. B. Imagine you are given equal volumes of the following solutions: .1M KNO (g) 0.1M 0.1MCH0Ho)(methanol) 01MBa(NO)log) Range these solutions in terms of their conductivity-from the worst conductor of electricity to the best Justify your answer

Explanation / Answer

1. as theory tells that a substance which dissociate completeky into its constituents ions are called ionic compound. they are known as strong electrolyte . 2 fig show that . all the atoms are dissociate into the space . whereas few subatance which partially dissociate into the solutions are known as weak electrolytes. so 3 fig shows that condition.

whereas in first figure no dissociation occurs. they are known as non electrolyte.

2. at given volume . the ionic compound dissociate into its constituents compounds and initially the number of charge particle increases hence the conductivity increase. but later on at very high concentration the collision between the motion of charge particle occurs and it will decrease the conductivty. whereas in weak electrolytes the their conductivity increases on increasing the dillution. but at normal concentration their conductivity is poor.

KNO3 - dissociate into its two cahrged particle K+ & NO3-

H2CO3 - weak acid partially dissociate.

Ba(NO3)2- dissociate into 3 particles Ba & two NO3-

CH3OH - it is non electrolyte does not dissociate into constituents particle

now our order is Ba(NO3)2>KNO3>H2CO3>CH3OH

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