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Solubility Rules And Precipitates

Solubility Rules And Precipitates. Solubility Rules & Precipitates. Solubility rules describe whether or not certain ions can form solid products called precipitates . For the questions below use the solubility rules and write the reason : Is Ba (NO 3 ) 2 soluble?

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Solubility Rules And Precipitates

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  1. Solubility Rules And Precipitates

  2. Solubility Rules & Precipitates • Solubility rules describe whether or not certain ions can form solid products called precipitates. • For the questions below use the solubility rules and write the reason: • Is Ba(NO3)2 soluble? • Is PbCl2soluble or insoluble? • Is Hg(NO3)2 soluble of insoluble?

  3. 1. Label each ion combination as soluble or insoluble. • Potassium ion & Bromine ion • Strontium ion & Chlorine ion • Calcium & Carbonate • Silver & Chromate 2. Write the separated ions for these combinations, then label the ion combination as soluble or insoluble • Lead (II) Bromide • Calcium Carbonate • Sodium hydroxide • SrBr2 • Ammonium hydroxide • Fe3(PO4)2 • Pb(CH3COO)2 • NiCl2

  4. 3. Which ion in combination with Pb2+ are soluble compounds? • 4. Are all Nitrates soluble? • 5. Are all Phosphates insoluble? • Consider the following: • A solution of potassium chloride is mixed with a solution of silver nitrate and a white precipitate is formed. What is the precipitate?

  5. Try these ones… • A solution of Potassium iodide is mixed with a solution of lead (II) nitrate. Is there a ppt? If yes, what is it? • A solution of copper (II) nitrate is mixed with a solution of sodium hydroxide. Is there a ppt? If yes, what is it?

  6. Solubility • Solubility is the maximum amount of solute that can be dissolves in a certain amount of solvent at a specific temperature. • Units = g (solute) / g H2O

  7. Three Main Factors that affect Solubility • 1. Nature of the solvent and Solute: • Different solutes will interact with solvents differently depending on the natural characteristics and properties of the solute.

  8. 2. Temperature: • For Solid and Liquid Solute, if you increase the temperature you increase the solubility. • For Gas Solutes, if you increase the temperature you decrease the solubility. • This is because the extra heat will cause the gas to be released from the solution.

  9. 3. Pressure: • For Solid and Liquid solutes, pressure changes have little effect on solubility. • For gases a decrease in pressure will decrease solubility. • For example: When you open a bottle of cola, you decrease the pressure, thus, decreasing the solubility of the carbon dioxide in the cola. The result: carbon dioxide bubbles out of the cola solution. • When dissolved gas escapes from a solution, this process is called effervescence.

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