Therefore the solution can conduct electricity 1 pure

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Therefore, the solution can conduct electricity. 1. Pure water does NOT conduct electricity but salt water does. o Electrolytes can be classified into three categories 1. Strong electrolytes ‘fully ionize’ when dissolved in water. This means that 100% of the substance splits into ions when dissolved in water. NaCl (sodium chloride) solution and HNO 3 (nitric acid) solution are examples. NaCl (s) + H 2 O (l) Na + (aq) + Cl - (aq) 2. Weak electrolytes ‘partially ionize when dissolved in water. This means that less than 100% of the substance splits into ions. Some of the substance remains intact, not existing as ions. Acetic acid, water, hydrofluoric acid, and ammonia are examples. Notice the double arrow . This means the forward and reverse reaction proceed simultaneously.
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3. Non-Electrolytes do NOT ionize when dissolved in water. This means that 100% of the substance stays intact when solvated by solvent molecules. C 6 H 12 O 6 (s) C 6 H 12 O 6 (aq) Most non-electrolytes are polar organic compounds. o Here are some examples. Be able to write chemical equations , with the appropriate symbols, showing a strong, weak and non-electrolyte dissolving in water. Solubility Rules: used to predict whether ionic compounds form ions in solution MEMORIZE table 4.1 on page 128 ASAP You will be asked to predict if a given ionic compound is soluble and ionizes fully (strong electrolyte), or if it does not readily dissolve and partially ionizes (very weak electrolyte). All ionic compounds are somewhat soluble in water, so think of insoluble as 99.99% undissolved ions. Are the following compounds soluble (SE) or insoluble (WE) Hg 2 Cl 2
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KI Pb(NO 3 ) 2 NaBr Ba(OH) 2 CaCO 3 Again memorize Table 4.1 and practice the HW.
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