Presentation is loading. Please wait.

Presentation is loading. Please wait.

Solubility Do Now: p.4. Remember…likes dissolve like Things that dissolve in water – Soluble ionic – Acids (ex HCl) – Bases (ex. NaOH) – Polar covalent.

Similar presentations


Presentation on theme: "Solubility Do Now: p.4. Remember…likes dissolve like Things that dissolve in water – Soluble ionic – Acids (ex HCl) – Bases (ex. NaOH) – Polar covalent."— Presentation transcript:

1 Solubility Do Now: p.4

2 Remember…likes dissolve like Things that dissolve in water – Soluble ionic – Acids (ex HCl) – Bases (ex. NaOH) – Polar covalent molecules

3 When Ionic Compound dissolved in water they dissociate= hydration Cl -

4 Identify the nature of each of the following as PC, NPC, or ionic. CH 4 NaCl H 2 O CCl 4 CH 3 OH H 2 S CaBr 2 C 6 H 14 NH 3 NH 4 OH C 4 H 10 PH 3 CH 3 CH 2 OH Nonpolar Cov. Ionic Polar Covalent Nonpolar Cov. Polar Cov. Ionic Nonpolar Cov. Polar Cov. Ionic Nonpolar Cov. Polar Cov. Now try p.8

5 Solubility = the max amount of solute that can be dissolved in a solvent Many solids and gases dissolve in water As you increase the temperature, you can dissolve more solid Does this work the same with gas? NOT the same for gases – as you increase temp, gas molecules KE Where can you go to find if an ionic compound is soluble or insoluble in water? Table F

6 Summary: Factors Affecting Solubility Nature of the solvent and the solute: Nature of the solvent and the solute: LIKE DISSOLVES LIKE Temperature Temperature Pressure (for systems with gases) Pressure (for systems with gases)

7 Factors that affect the rate at which something dissolves Temperature Stirring or agitation Surface area (crushing/grinding)

8 Solubility curves show the relationship between solubility and temperature. Can you guess which of these compounds are gases?! How do you know?!

9 Reading a solubility curve?! Table G tells you the max amount of solute you can dissolve in 100 g of H 2 O at a given temperature

10 How much KCl will dissolve in 100g of water at 50  C? Problem: X = 42g KCl

11 How much KCl will dissolve in 300g of water at 50  C? Hint: Use the graph to set up a proportion Problem: 42 g KCl = X g KCl 100 g H 2 O 300 g H 2 O X = 126g KCl

12 How much H 2 O is required to just dissolve 200 g NaNO 3 at 20  C? 88 g NaNO 3 = 100 g H 2 O 200 g NaNO 3 X g of H 2 O X = g H 2 O

13 On the line – saturated (full, cannot hold any more solute Below the line – unsaturated (can hold more solute) Above the line – supersaturated (holding more solute then it should – very unstable)

14 Unsaturated solution

15 Saturated Solution Is in equilibrium between solid particles dissociating into ions and ions forming crystals Cl - (aq)

16 Supersaturated Solution very unstable ( this picture is showing the addition of 100 g of glucose to 100ml of water at 25 0 C) Note: at 25 0 C, only 91g of glucose will dissolve in 100 ml of water Let’s see what happens Let’s see what happens

17 Precipitation problems A saturated solution of KNO 3 is prepared in 100 g of water at 50  C and then cooled down to 10  C. How much KNO 3 will precipitate? A saturated solution of KNO 3 is prepared in 100 g of water at 50  C and then cooled down to 10  C. How much KNO 3 will precipitate?

18 88 g KNO 3 in 100 g H 2 O at 50  C 20 g KNO 3 in 100 g H 2 O at 10  C 88 g – 20 g = 68 g KNO 3 precipitates


Download ppt "Solubility Do Now: p.4. Remember…likes dissolve like Things that dissolve in water – Soluble ionic – Acids (ex HCl) – Bases (ex. NaOH) – Polar covalent."

Similar presentations


Ads by Google