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Solutions
- 1.
- 2. RECAPITULATION •WHAT IS MATTER? •WHATARETHE FIVE PHASES OF MATTER? •HOW DOWE CLASSIFYMATTER?
- 4. SOLUTIONS •is made upof more than one component, but each component is evenly distributed. •Solutions of this kind are known as homogenous solutions. •homogenous mixture of two or more substances evenly distributed in each other
- 5. CLASSIFICATIONS OF SOLUTIONS ACCORDINGTO PHASES •gaseous solution •solid solutions •liquid solutions
- 6. DILUTE • solute ispresent in small amounts CONCENTRATED • the solute is present in considerably significant amounts
- 7. SOLUBILITY •is the measureof how much solute will dissolve in a solvent at a specific temperature •The famous saying “like dissolves like” is important in predicting the solubility of a
- 8. MISCIBILITY VS. SOLUBILITY Miscibility •termused when two liquids are completely soluble with one another in all Solubility •term used when a solid or gas is completely soluble in liquid in all proportions
- 9. Factors Affecting Solubilityof a SoluteA. Temperature •In the previous experiment, you were able to dissolve excess solute upon heating. Thus, temperature affects the solubility of substances. The solubility of a solid in liquid usually increases with increasing temperature since most dissolution process that involves a solid solute over a liquid solvent is endothermic. However, in the case of the solubility of gas in liquid,
- 10. B. Nature ofSolvent •The ability of a solute to be dissolved in a given solvent is affected by the type of bond of both the solute and solvent. In general, polar liquids dissolve polar compounds and the same is true with nonpolar liquids. Thus goes the saying “like dissolves like”. This is the guiding rule in preparing solutions. Since water is a polar liquid, it dissolves polar compounds such as sugar (C6H12O6) and salt (NaCl). Sometimes, in spite of all attempts, a substance does not appreciably
- 11. C. Pressure •The effectof pressure on the solubility of a solid or liquid solute is not as noticeable as that of a gaseous solute. The solubility of gases in water usually increases with increasing pressure. This relationship is first noticed by William Henry (1775-1836) in 1803 and its law is called after his name— Henry’s law or Pressure-Solubility Law. This law states that in a given temperature, the mass of a gas that dissolves in a given volume of liquid is directly related to its pressure.
- 12. Factors Affecting theRate of Dissolution A. Surface area Surface area does not affect the amount of solute that will dissolve, but it does affect the solute’s rate of dissolution.Thus, in order to make a solid solute dissolve faster, we frequently powder it, thereby increasing the surface area.This is why powdered coffee dissolves faster than granulated coffee even without stirring.
- 13. B. Rate ofStirring •The rate at which a solute dissolves can be increased by stirring the mixture. This process brings fresh solvent into contact with the solute and so permits a faster rate of dissolution.
- 14. C. Temperature •Generally, solubilityincreases with increasing temperature for most cases of solid in liquid. The increase in temperature causes an increase in kinetic energy of the solute, solvent and the solution thus facilitating rapid interaction with one another.
- 15. •A. Identify thecondition that will make the solute in each mixture dissolve faster.Write stirring, crushing, or using heat energy in your notebook. 1. maggi cubes and water 2. powdered milk and water 3. salt and water 4. instant coffee and water 5. sugar and pure buko juice
- 16. given questions inyour notebook. •1. Mother told you to prepare a glass of milk for your small brother. After putting amounts of sugar into the glass, you noticed that the sugar particles are still there. What should you do to make the sugar dissolve faster? •2. In your EPP subject, your group was assigned to cook fish “sinigang”. Your classmate bought rock salt instead of fine salt. What should you do to the rock salt so that it will dissolve faster in your
- 17. Saturated, Unsaturated and SupersaturatedSolutions•Unsaturated solution contains less solute than it has the capacity to dissolve. •Saturated solution is one that contains as much of the solute as it can hold at a given temperature. •supersaturated solution contains more solute than is present in a saturated solution. This is a rather unstable condition. In this case, the excess solid will eventually separate from the solution as a precipitate in a process known as precipitation or as crystals in a
- 20. Concentration of asolution •The amount of solute present in a given quantity of solvent or solution. •Four most common units of concentration: percent composition, mole fraction, molarity, and molality.
- 21. LET’S PRACTICE •What isthe mass percent of a solution of 7.6 grams sucrose in 83.4 grams of water? •How many grams of sucrose must be added to 375 grams of water to prepare a 2.75 % by mass solution of sucrose? • If concentration by mass of 600 g NaCl solution is 40 %, find amount of solute by mass in this solution.
- 22. Solve for theunknown. Show all work and report answers with units. 1.What is the percent by mass of 5.0 g of iron (II) sulfate dissolved in 75.0 g of water? 2.A solution is made by adding 25 mL of benzene to 80 mL of toluene. What is the percent by volume of benzene? 3.A solution is formed by adding 35 g of ammonium nitrate to 250 g of water.What is the percent by mass of ammonium nitrate?
- 23. 3.What is themass percent of each component in the mixture formed by adding 12 g of calcium sulfate, 18 g of sodium nitrate, and 25 g of potassium chloride to 500 g of water? 4.An experiment requires a solution that is 80% methyl alcohol by volume. What volume of methyl alcohol should be added to 200 mL of water to make this solution?