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Using Tables F & G

Using Tables F & G. Table G. Expresses solubility as a function of temperature. Valid only for a specific amount of the solvent – 100 grams of water. Table G problems.

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Using Tables F & G

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  1. Using Tables F & G

  2. Table G • Expresses solubility as a function of temperature. • Valid only for a specific amount of the solvent – 100 grams of water.

  3. Table G problems • May have to do with the amount of solute or solvent required for a given amount of the other. Involve setting up a proportion. • Precipitation problems.

  4. Problem: How much KCl will dissolve in 300 grams of water at 50C? Use the graph to set up a proportion. 42 g KCl is to 100 g H2O as X g KCl is to 300 g H2O.

  5. Finding amount Solute 42 g KClX g KCl 100 g H2O 300 g H2O X = 126 g KCl =

  6. How much H2O is required to just dissolve 200 g NaNO3 at 20C? 88 g NaNO3 is to 100 g H2O as 200 g NaNO3 is to X g of H2O.

  7. Finding amount H2O 88 g NaNO3 = 200 g NaNO3 100 g H2O X g H2O X = 227.3 g H2O

  8. Precipitation problems • A saturated solution of KNO3 is prepared in 100 g of water at 50C and then cooled down to 10C. How much KNO3 will precipitate?

  9. 88 g KNO3 in 100 g H2O at 50C. 20 g KNO3 in 100 g H2O at 10C. 88 g – 20 g = 68 g KNO3 precipitates.

  10. Table F problems • Solubility guidelines for ionic substances in water. • The extent to which ionic compounds will dissolve in water depends on several factors. The solubility ranges from very low solubility – basically insoluble – to pretty soluble. • Use guidelines to predict if a given compound is soluble or insoluble.

  11. To use Table F • Separate the ionic compound into the positive ion and the negative ion. • Scan for both in Table F. • Left hand side is soluble compounds with exceptions. Right hand side is insoluble compounds with exceptions.

  12. Predict solubility of • LiCl • NH4F • Ca(HCO3)2 • BaSO4 • K2CO3 • CaCO3 • Mg3(PO4)2 • Ca(OH)2 Soluble – cmpd with a Group I ion Soluble – cmpd with NH4+ Soluble – cmpd with HCO3- Insoluble – sulfates with Ba+ Soluble – cmpd with a Group 1 ion Insoluble - most carbonates Insoluble – most phosphates Soluble – hydroxide with Ca+2

  13. Why do we need to predict solubility? • So we can determine the precipitate in a double replacement reaction.

  14. Predicting Products AgNO3(aq) + KCl(aq)  ? AgCl(s) + KNO3(aq)

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