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Presentation On Solutions

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Published in: Chemistry
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Solutions PPT part I

Sunil / Bangalore

8 years of teaching experience

Qualification: B.Tech/B.E. (Kolhapur Institute of Technology's College of Engineering (KITCE), Kolhapur - 2018)

Teaches: Bio Technology, Biology, Botany, Chemistry, Mathematics, Zoology, Agriculture, Bio Chemistry, Microbiology, Organic Chemistry, AIEEE, CET, IIT JEE Advanced, IIT JEE Mains, Medical Entrance Exams, NEET

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  1. Solutions Part - I
  2. Definition A solution is a homogeneous mixture of two or more than two components. >Classification Solutions are broadly classified into two types; 1. Solutions which contain two components in it are called Binary Solutions. 2. Solutions which contains more than two components called poly solutions Substances which are used to prepare a solution are called as Components. > The component that is present in the largest quantity is known as Solvent. Solvent determines the physical state in which solution exists. > The other component present in lesser quantity in the solution is termed as Solute. >Each component may be solid, liquid or in gaseous state.
  3. Solutions Part - I
  4. Type of Solution Gaseous Solutions Liquid Solutions Solid Solutions Solute Gas Liquid solid Gas Liquid Solid Gas Liquid Solid Solvent Gas Gas Gas Liquid Liquid Liquid Solid Solid Solid Common Examples Mixture of oxygen and nitrogen gases Chloroform mixed with nitrogen gas Camphor in nitrogen gas Oxygen dissolved in water Ethanol dissolved in water Glucose dissolved in water Solution of hydrogen in palladium Amalgam of mercury with sodium Copper dissolved in gold
  5. Definition A solution is a homogeneous mixture of two or more than two components. >Classification Solutions are broadly classified into two types; 1. Solutions which contain two components in it are called Binary Solutions. 2. Solutions which contains more than two components called poly solutions Substances which are used to prepare a solution are called as Components. > The component that is present in the largest quantity is known as Solvent. Solvent determines the physical state in which solution exists. > The other component present in lesser quantity in the solution is termed as Solute. >Each component may be solid, liquid or in gaseous state.
  6. Strength of Solutions The amount of solute dissolved per unit solution or solvent is called Strength of solution. There are various methods of measuring strength of a solution: 1. Mass Percentage (O/ow/w): "It represents mass of a component present in 100 g of solution" Mathematically; Mass of component in the sol. Mass % of a component = x 100 Total Mass of sol. 2. Volume percentage (O/ov/v): "It represents volume of a component in 100 mL of solution" Mathematically; Vol. % of a component = Vol. of component x 100 Total vol. of solution
  7. Type of Solution Gaseous Solutions Liquid Solutions Solid Solutions Solute Gas Liquid solid Gas Liquid Solid Gas Liquid Solid Solvent Gas Gas Gas Liquid Liquid Liquid Solid Solid Solid Common Examples Mixture of oxygen and nitrogen gases Chloroform mixed with nitrogen gas Camphor in nitrogen gas Oxygen dissolved in water Ethanol dissolved in water Glucose dissolved in water Solution of hydrogen in palladium Amalgam of mercury with sodium Copper dissolved in gold
  8. 3. Mass by volume percentage (O/ow/v): "It represents mass of solute in grams present in 100 mL of solution" Mathematically; Mass by vol. % = 4. Parts per Million (ppm): Mathematically; Mass of solute in gm x 100 Vol. of soloin mL No. of parts of the component x 106 Parts per Million = Total no. of all the componens of sol. Concentration in parts per million can be expressed as mass to mass, volume to volume and mass to volume.
  9. Strength of Solutions The amount of solute dissolved per unit solution or solvent is called Strength of solution. There are various methods of measuring strength of a solution: 1. Mass Percentage (O/ow/w): "It represents mass of a component present in 100 g of solution" Mathematically; Mass of component in the sol. Mass % of a component = x 100 Total Mass of sol. 2. Volume percentage (O/ov/v): "It represents volume of a component in 100 mL of solution" Mathematically; Vol. % of a component = Vol. of component x 100 Total vol. of solution
  10. 5. Mole Fraction (x): "It represents the moles of a solute present in one mole of solution" Mathematically; No. of moles of the component Mole fraction= Total no. of moles all the components For example, in a binary mixture, if the number of moles of A and B are nA and nB respectively, the mole fraction of A will be nA+nB nA+nB For a binary solution i.e. solution with two components Total Mole fraction of solution = X 1+ X2 = 1 i.e. = 1
  11. 3. Mass by volume percentage (O/ow/v): "It represents mass of solute in grams present in 100 mL of solution" Mathematically; Mass by vol. % = 4. Parts per Million (ppm): Mathematically; Mass of solute in gm x 100 Vol. of soloin mL No. of parts of the component x 106 Parts per Million = Total no. of all the componens of sol. Concentration in parts per million can be expressed as mass to mass, volume to volume and mass to volume.
  12. 6. Molarity, M: "It represents moles of solute present in 1 L of solution" ' Units of Molarity are mol/ L also represented by 'M' or 'Molar'. ' "Density of a solution is mass of the solution per unit volume" Mass Density, d = Volume V Mathematically; Number of moles of solute Molarity, M = Vol. of sol. in L Given mass Number of moles of solute = Molar mass Given mass Molarity = Molar mass X Vol. Of sol. in L
  13. 5. Mole Fraction (x): "It represents the moles of a solute present in one mole of solution" Mathematically; No. of moles of the component Mole fraction= Total no. of moles all the components For example, in a binary mixture, if the number of moles of A and B are nA and nB respectively, the mole fraction of A will be nA+nB nA+nB For a binary solution i.e. solution with two components Total Mole fraction of solution = X 1+ X2 = 1 i.e. = 1
  14. 7. Molality, m: "It represents moles of solute present per kg of solvent" >Units of molality are mol/ kg which is also represented by m' or 'molal'. Mathematically; Number of moles of solute Molality, m - Mass of solvent in kg Given mass Number of moles of solute = Molar mass
  15. 6. Molarity, M: "It represents moles of solute present in 1 L of solution" ' Units of Molarity are mol/ L also represented by 'M' or 'Molar'. ' "Density of a solution is mass of the solution per unit volume" Mass Density, d = Volume V Mathematically; Number of moles of solute Molarity, M = Vol. of sol. in L Given mass Number of moles of solute = Molar mass Given mass Molarity = Molar mass X Vol. Of sol. in L
  16. 8. Normality, N: "It represents no. of equivalents of solute present in 1 L of solution." Mathematically; Normality, N = Number of gram equivalents of solute Volume of solvent in L Molecular weight (MW) Number of gram equivalents of solute (EW) = Number of equivalents per mole of solute (Valency of solute) 1 Normality, N = — V EW Where, m = mass of given solute to be dissolved V = volume of solution in liters EW = Equivalent weight * Valency doesn't necessarily mean valency in case of acids and bases it means the total H + and OH- that a acid or a base can donate
  17. 7. Molality, m: "It represents moles of solute present per kg of solvent" >Units of molality are mol/ kg which is also represented by m' or 'molal'. Mathematically; Number of moles of solute Molality, m - Mass of solvent in kg Given mass Number of moles of solute = Molar mass
  18. Vapour pressure Definition: Vapour pressure of a liquid/solution is the pressure exerted by the vapours in equilibrium with the liquid/solution at a particular temperature. Mathematically Vapour pressure oc escaping tendency Vapour pressure of liquid solutions and Raoult's Law: (Raoult's law for volatile solutes) Raoult's law states that for a solution of volatile liquids, the partial vapour pressure of each component in the solution is directly proportional to its mole fraction.
  19. 8. Normality, N: "It represents no. of equivalents of solute present in 1 L of solution." Mathematically; Normality, N = Number of gram equivalents of solute Volume of solvent in L Molecular weight (MW) Number of gram equivalents of solute (EW) = Number of equivalents per mole of solute (Valency of solute) 1 Normality, N = — V EW Where, m = mass of given solute to be dissolved V = volume of solution in liters EW = Equivalent weight * Valency doesn't necessarily mean valency in case of acids and bases it means the total H + and OH- that a acid or a base can donate
  20. Consider a solution containing two volatile components 1 and 2 with mole fractions Xl and respectively. Suppose at a particular temperature, their partial vapor pressures are PI and and the vapor pressure in pure state are and Thus, according to Raoult's Law, for component 1 PI = PIOXI Similarly, for component 2
  21. Vapour pressure Definition: Vapour pressure of a liquid/solution is the pressure exerted by the vapours in equilibrium with the liquid/solution at a particular temperature. Mathematically Vapour pressure oc escaping tendency Vapour pressure of liquid solutions and Raoult's Law: (Raoult's law for volatile solutes) Raoult's law states that for a solution of volatile liquids, the partial vapour pressure of each component in the solution is directly proportional to its mole fraction.
  22. According to Dalton's law of partial pressure, the total pressure (ptotal) over the solution phase in the container will be the sum of the partial pressures of the components of the solution and is given as : Substituting the values of PI and , we get total = PIOXI + P - (1 — X2)P10 + P20X2 P total — - PIO- + P total — = p 10 P total
  23. Consider a solution containing two volatile components 1 and 2 with mole fractions Xl and respectively. Suppose at a particular temperature, their partial vapor pressures are PI and and the vapor pressure in pure state are and Thus, according to Raoult's Law, for component 1 PI = PIOXI Similarly, for component 2
  24. Mule The plot of vapour pressure and rnole fraction of an ideal solution at constant ternperature. The dashed line I and Il represent the partial pressure of the cornponents. It can be seen frorn the plot that p and p: are directly proportional to x, and xz, respectively. The total vapour pressure is given by line marked 111 in the figure.
  25. According to Dalton's law of partial pressure, the total pressure (ptotal) over the solution phase in the container will be the sum of the partial pressures of the components of the solution and is given as : Substituting the values of PI and , we get total = PIOXI + P - (1 — X2)P10 + P20X2 P total — - PIO- + P total — = p 10 P total
  26. Mole fraction in vapor phase (yp) If and are the mole fractions of the components 1 and 2 respectively in the vapour phase then, using Dalton's law of partial pressures: Mole fraction of component 1 in vapor phase, = p 1 i.e. Yl - total Mole fraction of component 2 in vapor phase, = p 2 i.e. Y2 - 1 2 2 2 In general total Pi = Yi Ptotal
  27. Mule The plot of vapour pressure and rnole fraction of an ideal solution at constant ternperature. The dashed line I and Il represent the partial pressure of the cornponents. It can be seen frorn the plot that p and p: are directly proportional to x, and xz, respectively. The total vapour pressure is given by line marked 111 in the figure.
  28. Vapour pressures of solutions of solids in liquids and Raoult's Law If a non-volatile solute is added to a solvent to give a solution, the number of solvent molecules escaping from the surface is correspondingly reduced, thus, the vapour pressure is also reduced. The decrease in the vapour pressure of solvent depends on the quantity of non-volatile solute present in the solution, irrespective of its nature. Raoult's law in its general form can be stated as, for any solution the partial vapour pressure of each volatile component in the solution is directly proportional to its mole fraction. In a binary solution, let us denote the solvent by 1 and solute by 2. When the solute is non-volatile, only the solvent molecules are present in vapour phase and contribute to vapour pressure. Let pl be the vapour pressure of the solvent, xl be its mole fraction, po be its vapour pressure in the pure state. Then according to Raoult's law
  29. Mole fraction in vapor phase (yp) If and are the mole fractions of the components 1 and 2 respectively in the vapour phase then, using Dalton's law of partial pressures: Mole fraction of component 1 in vapor phase, = p 1 i.e. Yl - total Mole fraction of component 2 in vapor phase, = p 2 i.e. Y2 - 1 2 2 2 In general total Pi = Yi Ptotal
  30. Vapour pressure of pure solvent Mole fiaction of solvent 1 If a solution obeys Raoult's la" for all concentrations, its vapour pressure would vary linearly from zero to the vapour pressure of the pure solvent.
  31. Vapour pressures of solutions of solids in liquids and Raoult's Law If a non-volatile solute is added to a solvent to give a solution, the number of solvent molecules escaping from the surface is correspondingly reduced, thus, the vapour pressure is also reduced. The decrease in the vapour pressure of solvent depends on the quantity of non-volatile solute present in the solution, irrespective of its nature. Raoult's law in its general form can be stated as, for any solution the partial vapour pressure of each volatile component in the solution is directly proportional to its mole fraction. In a binary solution, let us denote the solvent by 1 and solute by 2. When the solute is non-volatile, only the solvent molecules are present in vapour phase and contribute to vapour pressure. Let pl be the vapour pressure of the solvent, xl be its mole fraction, po be its vapour pressure in the pure state. Then according to Raoult's law
  32. Ideal and Non-ideal solutions Ideal solutions : An ideal solution is the solution in which each component obeys Raoult's law under all conditions of temperatures and concentrations. Properties of Ideal solutions : AH MIXING MIXING Intermolecular attractive forces between the A-A and B-B are nearly equal to those between A-B. Eg. solution of benzene and toluene, solution of n-hexane and n-heptane
  33. Vapour pressure of pure solvent Mole fiaction of solvent 1 If a solution obeys Raoult's la" for all concentrations, its vapour pressure would vary linearly from zero to the vapour pressure of the pure solvent.
  34. Non - ideal solutions : When a solution does not obey Raoult's law over the entire range of concentration, then it is called non-ideal solution. Solutions showing positive deviation from Raoult's Law : Solvent-Solute(A-B) type of force is weaker than Solute - Solute(B-B) & Solvent- Solvent(A-A) forces. The vapour pressure is higher than predicted by the law. AH MIXING MIXING Eg. ethanol and acetone, carbon disulphide and acetone
  35. Ideal and Non-ideal solutions Ideal solutions : An ideal solution is the solution in which each component obeys Raoult's law under all conditions of temperatures and concentrations. Properties of Ideal solutions : AH MIXING MIXING Intermolecular attractive forces between the A-A and B-B are nearly equal to those between A-B. Eg. solution of benzene and toluene, solution of n-hexane and n-heptane
  36. Pressure composition curve for solution showing positive deviation Vapour pressure of solution Mole fraction
  37. Solutions Part - I
  38. Non - ideal solutions : When a solution does not obey Raoult's law over the entire range of concentration, then it is called non-ideal solution. Solutions showing positive deviation from Raoult's Law : Solvent-Solute(A-B) type of force is weaker than Solute - Solute(B-B) & Solvent- Solvent(A-A) forces. The vapour pressure is higher than predicted by the law. AH MIXING MIXING Eg. ethanol and acetone, carbon disulphide and acetone
  39. Solutions showing negative deviations from Raoult's law: Solvent-Solute(A-B) type of force is stronger than the other two. The vapour pressure is lower than predicted by the law MIXING AH MIXING For example,phenol and aniline, chloroform and acetone etc.
  40. >Definition A solution is a homogeneous mixture of two or more than two components. >Classification Solutions are broadly classified into two types; 1. Solutions which contain two components in it are called Binary Solutions. 2. Solutions which contains more than two components called poly solutions Substances which are used to prepare a solution are called as Components. > The component that is present in the largest quantity is known as Solvent. Solvent determines the physical state in which solution exists. > The other component present in lesser quantity in the solution is termed as Solute. >Each component may be solid, liquid or in gaseous state.
  41. Pressure composition curve for solution showing positive deviation Vapour pressure of solution Mole fraction
  42. Pressure composition curves for solution showing negative deviation Vapour pressure of solulion Mole traction
  43. Type of Solution Gaseous Solutions Liquid Solutions Solid Solutions Solute Gas Liquid solid Gas Liquid Solid Gas Liquid Solid Solvent Gas Gas Gas Liquid Liquid Liquid Solid Solid Solid Common Examples Mixture of oxygen and nitrogen gases Chloroform mixed with nitrogen gas Camphor in nitrogen gas Oxygen dissolved in water Ethanol dissolved in water Glucose dissolved in water Solution of hydrogen in palladium Amalgam of mercury with sodium Copper dissolved in gold
  44. Solutions showing negative deviations from Raoult's law: Solvent-Solute(A-B) type of force is stronger than the other two. The vapour pressure is lower than predicted by the law MIXING AH MIXING For example,phenol and aniline, chloroform and acetone etc.
  45. Pressure composition curves for solution showing negative deviation Vapour pressure of solulion Mole traction
  46. >Strength of Solutions The amount of solute dissolved per unit solution or solvent is called Strength of solution. There are various methods of measuring strength of a solution: 1. Mass Percentage (O/ow/w): "It represents mass of a component present in 100 g of solution" Mathematically; Mass of component in the sol. Mass % of a component = x 100 Total Mass of sol. 2. Volume percentage (O/ov/v): "It represents volume of a component in 100 mL of solution" Mathematically; Vol. % of a component = Vol. of component x 100 Total vol. of solution
  47. 3. Mass by volume percentage (O/ow/v): "It represents mass of solute in grams present in 100 mL of solution" Mathematically; Mass by vol. % = 4. Parts per Million (ppm): Mathematically; Mass of solute in gm x 100 Vol. of soloin mL No. of parts of the component x 106 Parts per Million = Total no. of all the componens of sol. Concentration in parts per million can be expressed as mass to mass, volume to volume and mass to volume.
  48. 5. Mole Fraction (x): "It represents the moles of a solute present in one mole of solution" Mathematically; No. of moles of the component Mole fraction= Total no. of moles all the components For example, in a binary mixture, if the number of moles of A and B are nA and nB respectively, the mole fraction of A will be nA+nB nA+nB For a binary solution i.e. solution with two components Total Mole fraction of solution = X 1+ X2 = 1 i.e. = 1
  49. 6. Molarity, M: "It represents moles of solute present in 1 L of solution" ' Units of Molarity are mol/ L also represented by 'M' or 'Molar'. ' "Density of a solution is mass of the solution per unit volume" Mass Density, d = Volume V Mathematically; Number of moles of solute Molarity, M = Vol. of sol. in L Given mass Number of moles of solute = Molar mass Given mass Molarity = Molar mass X Vol. Of sol. in L
  50. 7. Molality, m: "It represents moles of solute present per kg of solvent" >Units of molality are mol/ kg which is also represented by m' or 'molal'. Mathematically; Number of moles of solute Molality, m - Mass of solvent in kg Given mass Number of moles of solute = Molar mass
  51. 8. Normality, N: "It represents no. of equivalents of solute present in 1 L of solution." Mathematically; Normality, N = Number of gram equivalents of solute Volume of solvent in L Molecular weight (MW) Number of gram equivalents of solute (EW) = Number of equivalents per mole of solute (Valency of solute) 1 Normality, N = — V EW Where, m = mass of given solute to be dissolved V = volume of solution in liters EW = Equivalent weight * Valency doesn't necessarily mean valency in case of acids and bases it means the total H + and OH- that a acid or a base can donate
  52. Vapour pressure Definition: Vapour pressure of a liquid/solution is the pressure exerted by the vapours in equilibrium with the liquid/solution at a particular temperature. Mathematically Vapour pressure oc escaping tendency Vapour pressure of liquid solutions and Raoult's Law: (Raoult's law for volatile solutes) Raoult's law states that for a solution of volatile liquids, the partial vapour pressure of each component in the solution is directly proportional to its mole fraction.
  53. Consider a solution containing two volatile components 1 and 2 with mole fractions Xl and respectively. Suppose at a particular temperature, their partial vapor pressures are PI and and the vapor pressure in pure state are and Thus, according to Raoult's Law, for component 1 PI = PIOXI Similarly, for component 2
  54. According to Dalton's law of partial pressure, the total pressure (ptotal) over the solution phase in the container will be the sum of the partial pressures of the components of the solution and is given as : Substituting the values of PI and , we get total = PIOXI + P - (1 — X2)P10 + P20X2 P total — - PIO- + P total — = p 10 P total
  55. Mule The plot of vapour pressure and rnole fraction of an ideal solution at constant ternperature. The dashed line I and Il represent the partial pressure of the cornponents. It can be seen frorn the plot that p and p: are directly proportional to x, and xz, respectively. The total vapour pressure is given by line marked 111 in the figure.
  56. Mole fraction in vapor phase (yp) If and are the mole fractions of the components 1 and 2 respectively in the vapour phase then, using Dalton's law of partial pressures: Mole fraction of component 1 in vapor phase, = p 1 i.e. Yl - total Mole fraction of component 2 in vapor phase, = p 2 i.e. Y2 - 1 2 2 2 In general total Pi = Yi Ptotal
  57. Vapour pressures of solutions of solids in liquids and Raoult's Law If a non-volatile solute is added to a solvent to give a solution, the number of solvent molecules escaping from the surface is correspondingly reduced, thus, the vapour pressure is also reduced. The decrease in the vapour pressure of solvent depends on the quantity of non-volatile solute present in the solution, irrespective of its nature. Raoult's law in its general form can be stated as, for any solution the partial vapour pressure of each volatile component in the solution is directly proportional to its mole fraction. In a binary solution, let us denote the solvent by 1 and solute by 2. When the solute is non-volatile, only the solvent molecules are present in vapour phase and contribute to vapour pressure. Let pl be the vapour pressure of the solvent, xl be its mole fraction, po be its vapour pressure in the pure state. Then according to Raoult's law
  58. Vapour pressure of pure solvent Mole fiaction of solvent 1 If a solution obeys Raoult's la" for all concentrations, its vapour pressure would vary linearly from zero to the vapour pressure of the pure solvent.
  59. Ideal and Non-ideal solutions Ideal solutions : An ideal solution is the solution in which each component obeys Raoult's law under all conditions of temperatures and concentrations. Properties of Ideal solutions : AH MIXING MIXING Intermolecular attractive forces between the A-A and B-B are nearly equal to those between A-B. Eg. solution of benzene and toluene, solution of n-hexane and n-heptane
  60. Non - ideal solutions : When a solution does not obey Raoult's law over the entire range of concentration, then it is called non-ideal solution. Solutions showing positive deviation from Raoult's Law : Solvent-Solute(A-B) type of force is weaker than Solute - Solute(B-B) & Solvent- Solvent(A-A) forces. The vapour pressure is higher than predicted by the law. AH MIXING MIXING Eg. ethanol and acetone, carbon disulphide and acetone
  61. Pressure composition curve for solution showing positive deviation Vapour pressure of solution Mole fraction
  62. Solutions showing negative deviations from Raoult's law: Solvent-Solute(A-B) type of force is stronger than the other two. The vapour pressure is lower than predicted by the law MIXING AH MIXING For example,phenol and aniline, chloroform and acetone etc.
  63. Pressure composition curves for solution showing negative deviation Vapour pressure of solulion Mole traction

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