Download to read offline
![ict_presentation_final_final_final[1].pptx](https://cdn.slidesharecdn.com/ss_thumbnails/ictpresentationfinalfinalfinal1-251230145259-2b4839bd-thumbnail.jpg?width=640&height=640&fit=bounds)
5.-Solutions-2-1.pptx chemistry yessssss
- 1.
- 2. A solution isa mixture of 2 or more substances in a single phase. One constituent is usually regarded as the and the others as .
- 3. Solutions are homogeneous mixtures oftwo or more pure substances. In a solution, the solute is dispersed uniformly throughout the solvent.
- 4. • SOLUTE– thepart of a solution that is being dissolved (usually the lesser amount) • SOLVENT– the part of a solution that dissolves the solute (usually the greater amount) IDENTIFYING COMPONENTS OF SOLUTIONS Solution Solute Solvent Air in balloon O2 N2 Ammonia water NH3 H2O Rubbing alcohol (70%) H2O Isopropyl alcohol al Rubbing ) cohol (40% Ethyl alcohol H2O Tincture of Iodine Iodine Alcohol
- 5. Gas Liquid Solid
- 6. SOLUTION SOLUTE SOLVENTEXAMPLE Gas in a gas Oxygen Nitrogen Air Gas in a liquid CO2 H2O Soda water Liquid in a liquid Acetic acid H2O Vinegar Solid in a liquid Sugar H2O Sugar syrup Liquid in a solid Hg Ag Dental amalga m Solid in a solid tin copper Bronze
- 7. 1. Solvent moleculesare attracted to surface ions. 2. Each ion is surrounded by solvent molecules. 3. Enthalpy ( H) changes with each interaction broken or formed. Ionic solid dissolving in water
- 8. The ions are solvated (surroundedby solvent). If the solvent is water , the ions are hydrated. The intermolecular forces.
- 9. solvation isan interaction of a solute with the solvent, which leads to stabilization of the solute in the solution.
- 10.
- 11. Hypotonic (lower solute concentration) to thesolution Hypertonic (higher solute concentration) to the solution
- 12. Isotonic solutions are equal intheir solute concentrations.
- 13. • It isthe process by which a solid, liquid or gas forms a solution in a
- 14. • In solidsthis can be explained as the breakdown of the crystal lattice into individual ions, atoms or molecules and their transport into the solvent.
- 15. • For liquidsand gases, the molecules must be compatible with those of the solvent for a solution to form.
- 16. • Dissolution isa physical change—you can get back the original solute by evaporating the solvent. • If you can’t, the substance didn’t dissolve, it Ni(s) + HCl (aq) NiCl2(aq) + H2(g) NiCl2(s) dr y
- 17. •It refers tothe maximum amount of solute, expressed in grams, that can be dissolved in 100 g of water at a specific
- 18. Soluble a substance that dissolvesin a solvent Insoluble a substance that does not dissolve in a solvent (sand is insoluble in water)
- 19. SUBSTANCES KEROSENE OIL ETHYL ALCOHOLWATER Sugar Salt Detergent Powdered chalk Powdered charcoal Sulfur powder CuSO4 KMnO4 Activity: Solubility
- 20. Immiscible Two liquids that areinsoluble Miscible Two liquids that are soluble in each other SOLVENT WATER KEROSENE ACETONE ALCOHOL oil
- 21. Types of Saturation Kindsof Saturation Definition Saturated Solution A solution with solute that dissolves until it is unable to dissolve anymore, leaving the undissolved substances at the bottom. Unsaturated Solution A solution (with less solute than the saturated solution) that completely dissolves, leaving no remaining substances. Supersaturated Solution A solution (with more solute than the saturated solution) that contains more undissolved solute than the saturated solution because of its tendency to crystallize and precipitate.
- 22. Example 1: SaturatedSolution
- 23. Everyday Examples ofSaturated Solutions • Carbonated water is saturated with carbon, hence it gives off carbon through bubbles. • Adding sugar to water until it no longer dissolves creates a saturated solution. • Continuing to dissolve salt in water until it will no longer dissolve creates a saturated solution. • The Earth's soil is saturated with nitrogen. • Mixing powdered soap into water until it will not dissolve creates a saturated solution. • In beer or sparkling juices there is a saturation of carbon dioxide that is let off as a gas. • Coffee powder added to water can create a saturated solution. • Salt added to vinegar can create a saturated solution when the salt no longer dissolves. • Chocolate powder added to milk can create saturation at the point that no more powder can be added.
- 24. Everyday Examples ofSaturated Solutions • Sugar dissolved into vinegar until it will no longer do so creates a saturate solution. • Water can be saturated with juice powder to create a beverage. • Milk can be saturated with flour at which point no more flour can be added to the milk. • Melted butter can be saturated with salt when the salt will no longer dissolve. • Bathing salts can saturate water when there is no more ability to dissolve them. • Sugar can be added to milk to the point of saturation. • Processed tea powders can be added to water to saturate the water. • Protein powder could be used to create a saturated solution with milk, tea, or water. • Laxative powders could saturate juice or water with which they are mixed. • Cocoa powder could be mixed into water to the point of saturation. • Sugar could be mixed into tea to the point that the tea is saturated. • Coffee can be saturated with sugar when no more will mix in to the coffee.
- 25. Example 2: UnsaturatedSolution
- 26. Example 3: SupersaturatedSolution
- 28. • Chemists usethe rule of the THUMB • “like dissolves like” Polar substances tend to dissolve in polar solvents. Nonpolar substances tend to dissolve in nonpolar solvents. • Nature of Solute and Solvent
- 29. SOLVENT NaCl C12H22O11C10H8 I2 Water SOLVENT WATER KEROSENE ACETONE ALCOHOL Oil Examples
- 30. • Effect ofTemperature Generally, the solubility of solid solutes in liquid solvents increases with increasing
- 31.
- 32. The opposite is trueof gases. • Higher temperature drives gases out of solution. Carbonated soft drinks are more “bubbly” if stored in the refrigerator. Warm lakes have less O2 dissolved in them than cool lakes.
- 33. • Effect ofPressure Small changes in pressure have little effect on the solubility of solids in liquids or liquids in liquids but have a marked effect on the solubility of gases in liquids.
- 34.
- 35. Sg= kPg •Where: • Sgisthe solubility of the gas; • k is the Henry’s law constant for that gas in that solvent; • Pgis the partial pressure of the gas above the liquid.
- 36. The largerthe molecules of the solute are, the larger is their molecular weight and their size. It is more difficult for solvent molecules to surround bigger molecules. If all of the above mentioned factors all excluded, a general rule can be found that larger particles are generally less soluble. If the pressure, and temperature are the same than out of two solutes of the same polarity, the one with smaller particles is usually more soluble.
- 37. SOLVENT REFINED SALTROCK SALT Water SOLVENT REFINED KNO3 KNO3 CRYSTAL S Water
- 38. Stirring onlyincreases the speed of the process - it increases the movement of the solvent that exposes solute , thus enabling solubility. As molecules in liquid substances are in constant move, the process would take place anyway, but it would take more time.
- 39. SOLUTE SET-UP W/ STIRRING UNDISTURBED SET-UP TIMETO DISSOLV E CuSO4 KNO3
- 40. The stronger the intermolecular attractions between solute andsolvent, the more likely the solute will dissolve. Example: ethanol in water Ethanol = CH3CH2OH Intermolecular forces = H-bonds; dipole- dipole; dispersion Ions in water also have ion-dipole forces.
- 41. Concentrations of Solutions •There are a number of ways to express the relative amounts of solute and solvent in a solution. • Percent Composition (by mass) • Molarity • Molality • Mole Fraction
- 42. Percent Composition (bymass) • We can consider percent by mass (or weight percent, as it is sometimes called) in two ways: • The parts of solute per 100 parts of solution. • The fraction of a solute in a solution multiplied by 100.
- 43. Percent Composition (bymass) • We need two pieces of information to calculate the percent by mass of a solute in a solution: • The mass of the solute in the solution. • The mass of the solution.
- 44. Percent Composition (bymass) • Use the following equation to calculate percent by mass:
- 45. Percent Composition (bymass) Examples: • What is the percent by mass of rubbing alcohol in a solution that contains 275 g of rubbing alcohol in 500 g of solution? Solution: Percent by mass = mass of rubbing alcohol mass of solution = 275g 500g = 55.0 % (m/m) x 100% x 100%
- 46. Percent Composition (bymass) Examples: • What is the weight percent of sodium chloride in a solution that is made by dissolving 12.0g of NaCl in 60.0g of H2O? Solution: g solute (NaCl) = 12.0 g g solvent (H2O) = 60.0 g g solution = 72.0 g Percent by mass = 12.0 g NaCl 12.0 g + 60.0 g = 12 g 72 g = 16.0 % NaCl solution x 100% x 100%
- 47. Molarity • Molarity tellsus the number of moles of solute in exactly one liter of a solution. (Note that molarity is spelled with an "r" and is represented by a capital M.) • We need two pieces of information to calculate the molarity of a solute in a solution: • The moles of solute present in the solution. • The volume of solution (in liters) containing the solute.
- 48. Molarity • To calculatemolarity we use the equation:
- 49. 1. Sea watercontains roughly 28.0 g of NaCl per liter. What is the molarity of sodium chloride in sea water? Molarity Examples
- 50. •2. What isthe molarity of 245.0 g of H2SO4 dissolved in 1.000 L of solution? Molarity Examples
- 51. Molality • Molality, m,tells us the number of moles of solute dissolved in exactly one kilogram of solvent. (Note that molality is spelled with two "l"'s and represented by a lower case m.) • We need two pieces of information to calculate the molality of a solute in a solution: • The moles of solute present in the solution. • The mass of solvent (in kilograms) in the solution.
- 52. Molality • To calculatemolality we use the equation:
- 53. •Problem #1: Whatis the molality pf a 0.500M aqueous solution of sucrose (C12H22O11) if the density of the solution is 1.0638 g/mL? Molality Examples
- 54. •Problem #2 :A sulfuric acid solution containing 571.4 g of H2SO4 per liter of solution has a density of 1.329 g/cm3 . Calculate the molality of H2SO4 in this solution Molality Examples
- 55. Normality • Normality ofa solution is the concentration expressed as the number of gram equivalent weights (or number of equivalents, abbreviated equiv) of solute per liter of solution. A one-normal (1 N) solution contains one gram equivalent weight of solute per liter of solution. The equivalent weight is the weight of a substance that will react with, combine with, contain, replace, or in any other way be equivalent to, one mole of hydrogen atom or hydrogen ion or hydroxide ion.
- 56. Normality • To calculatenormality we use the equation: N = no. of equivalents of solute L of solution
- 57. Normality Examples: Problem 1. Whatis the normality of a solution containing 7.00g H3PO4 in 400mL of solution.
Editor's Notes
- #5 Based from the three states of matter
- #10 Dilute-small amount of solute is dispersed in the solvent Concentrated-large amount of solute is dissolved in the solvent
- #12 We say that they are isotonic to each other.
- #20 Two other terms often used to describe the solubility of liquid in liquid are: Immiscible – oil and vinegar Miscible-alcohol and water
- #22 Example 1: Above iillustrates an example of a saturated solution. In Figure 1.1-1.3, there is a constant amount of water in all the beakers. Figure 1.1 shows the start of the saturation process, in which the solid solute begins to dissolve (represented by red arrows). In the next beaker, Figure 1.2, much of the solid solute has dissolved, but not completely, because the process of crystallization (represented by blue arrows) has begun. In the last beaker, Figure 1.3, only a small amount of the solute in solvent remains undissolved. In this process, the rate of the crystallization is faster than the rate of dissolution, causing the amount of dissolved to be less than the amount crystallized.
- #25 Example 2: Next, an unsaturated solution is considered. In the Figure , there is a constant amount of water in all the beakers. Figure 2.1 shows the start of the process, in which solid solute is beginning to dissolve (represented by red arrows). In the next beaker, shown in Figure 2.2, a large amount of solute has dissolved. The size of the red arrows are much larger than those of the blue arrows, which means that the rate of dissolution is much greater than rate of crystallization. In the last beaker, shown in Figure 2.3, the solute solvent has completely dissolved in the liquid solvent.
- #26 Example 3: This is an example of a supersaturated solution. In the Figure, there is a constant amount of water in all the beakers. Figure 3.1 shows a beaker with more solid solute than in the saturated solution (Figure 1.1) dissolving. In Figure 3.2, solid begins to crystallize as it slowly decreases the rate of dissolution. In the last picture, Figure 3.3, the solids become a crystallized form which begins to harden.
- #28 “Like” here means similar in Polarity. Ex. Polar solutes, like NaCl (table salt), tends to dissolve in polar solvents like water but not in oil. Nonpolar solutes like grease stains, readily dissolve in nonpolar solvents like gasoline but not in a polar solvent like water.
- #34 William Henry an English chemist and physicist