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Solution Chemistry

Solution Chemistry. Solutions, Problems, Solutions, Problems. Does it ever end?. How can you express concentration?. How can you express concentration?. Mass % composition Molarity Molality Mole fraction Density. Mass % problems:. Find mass % Find amount of solute

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Solution Chemistry

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  1. Solution Chemistry Solutions, Problems, Solutions, Problems. Does it ever end?

  2. How can you express concentration?

  3. How can you express concentration? • Mass % composition • Molarity • Molality • Mole fraction • Density

  4. Mass % problems: • Find mass % • Find amount of solute • Find total mass of solution

  5. Mass % problems: • Find mass % • Mass % = mass of solute x 100 % total mass of solution Don’t forget to add the masses of the solute and solvent for the total mass

  6. Mass % problems: • Find amount of solute • Mass % = mass of solute x 100 % total mass of solution • Multiply by total mass and divide by 100% to solve for mass of solute

  7. Mass % problems: • Find total mass of solution • Mass % = mass of solute x 100 % total mass of solution • Multiply both sides by the mass of solution first to get it out of the denominator.

  8. Molarity problems: • Find molarity • Find amount of solute • Find volume of solution

  9. Molarity problems: • Find molarity • M= moles solute Volume of solution (L)

  10. Molarity problems: • Find amount of solute • M= moles solute Volume of solution (L) • Molarity x volume= moles!

  11. Molarity problems: • Find volume of solution • M= moles solute Volume of solution (L) • Multiply both sides by the volume of solution first to get it out of the denominator. OR!

  12. Molarity problems: • Find volume of solution • Use the molarity as a conversion factor! • moles solute x 1 L = Volume of solution! M

  13. Dilution Problems M x V = Moles • Moles of solute in new solution = moles in the stock solution. Molarity goes down, volume goes up

  14. Dilution Problems Example: What is the concentration of a solution made by diluting 25 ml of a .50 M HCl solution to a new volume of 150 ml?

  15. Dilution Problems Example: What is the concentration of a solution made by diluting 25 ml of a .50 M HCl solution to a new volume of 150 ml? M x V = moles. .50 M x .025 L= .0125 moles HCl M = mol/vol= .0125 mol / .150 L = .083 M

  16. Dilution Problems • What is the concentration of a solution made by diluting 125 ml of a 2.5 M NH3solution to a new volume of 350 ml? • What is the concentration of a solution made by diluting 2.5 ml of a 6.0 M NaClsolution to a new volume of 80. ml? • What is the concentration of a solution made by diluting 30. ml of a 1.0 M Fe(NO3)3solution with 20. ml of water? (The final volume should be 20. + 30. = 50. ml)

  17. Dilution Problems Example: What volume of a 2.0 M NaOH stock solution is required to mix 1.50 L of a .150 M NaOH solution?

  18. Dilution Problems Example: What volume of a 2.0 M NaOH stock solution is required to mix 1.50 L of a .150 M NaOH solution? M x V = moles. .150 M x 1.50 L = .225 moles NaOH .225 moles NaOH x 1 L/ 2.0 moles= .113 L

  19. Dilution Problems • What volume of a 6.0 M NaOH stock solution is required to mix 1.50 L of a .150 M NaOH solution? • What volume of a 2.0 M MgCl2stock solution is required to mix 1.750 L of a .10 M MgCl2solution? • What volume of a 1.0 M HClstock solution is required to mix 100. ml of a .10 M HCl solution?

  20. Volume Stoichiometry • If you mix 10. ml of .10 M HCl with .10 M NaOH, • …it should take 10. ml of the NaOH to react completely.

  21. Volume Stoichiometry • If you mix 10. ml of .10 M HCl with .20 M NaOH, • …it should take only 5.0 ml of the NaOH to react completely.

  22. Volume Problems • If you react 10.0 ml of .10 M HCl with .050 M NaOH, what volume of NaOH solution will be needed? • If you react 10.0 ml of .10 M H2SO4with .050 M NaOH, what volume of NaOH solution will be needed? • If you react 50.0 ml of 1.0 M CaCl2with 1.9 M Na2CO3, what volume of Na2CO3solution will be needed?

  23. Volume Stoichiometry • If 10. ml of .10 M HCl reacts completely with 10. ml NaOH, • …the concentration of the NaOH must be the same, .10 M

  24. Volume Stoichiometry • If 10. ml of .10 M HCl reacts completely with 20. ml NaOH, • …the concentration of the NaOH must be half of that, .050 M.

  25. Volume problems • If 25.0 ml of .30 M HCl reacts completely with 25. ml NaOH, what is the concentration of the NaOH? • If 10.0 ml of .10 M HCl reacts completely with 20. ml NaOH, what is the concentration of the NaOH? • If 15.0 ml of .10 M HCl reacts completely with 50. ml Pb(NO3)2, what is the concentration of the Pb(NO3)2?

  26. Acids and Bases

  27. Acids Bases Examples?

  28. Acids Bases Properties of Acids and Bases

  29. Acids Are electrolyte solutions Make ions in solution Affect indicators Have low pH Taste sour Neutralize bases Can cause serious burns Corrode reactive metals Have more H+ than OH- (in solution) Bases Are electrolyte solutions Make ions in solution Affect indicators Have high pH Taste bitter Neutralize acids Can cause serious burns Corrode aluminum only Have more OH- than H+ (in solution) Properties of Acids and Bases

  30. Acids Are electrolyte solutions Make ions in solution Affect indicators Have low pH Taste sour Neutralize bases Can cause serious burns Corrode reactive metals Have more H+ than OH- (in solution) Bases Are electrolyte solutions Make ions in solution Affect indicators Have high pH Taste bitter Neutralize acids Can cause serious burns Corrode aluminum only Have more OH- than H+ (in solution) Properties of Both

  31. BrØnsted-Lowry Definition • Substances that donate a proton (H+ ion) in a reaction are acids. • Substances that accept a proton (H+ ion) are bases. • Arrhenius acids and bases make H+ and OH- ions in solution. BrØnsted-Lowry bases are also Arrhenius bases.

  32. Conjugates • After an acid has donated a proton, the rest of the species is the conjugate base. HAA- + H+ • After a base has accepted a proton, the resulting species is the conjugate acid. B- + H+ HB

  33. What is the conjugate base of… • HCl • CH3COOH • H2SO4 • HSO4- • H2O • NH4+ • NH3

  34. What is the conjugate base of… ACID(loses H+ to form its)Conjugate base • HCl • CH3COOH • H2SO4 • HSO4- • H2O • NH4+ • NH3

  35. What is the conjugate base of… ACID(loses H+ to form its)Conjugate base • HCl ( H+ and)Cl- • CH3COOH • H2SO4 • HSO4- • H2O • NH4+ • NH3

  36. What is the conjugate base of… ACID(loses H+ to form its)Conjugate base • HCl ( H+ and)Cl- • CH3COOH( H+ and)CH3COO- • H2SO4( H+ and)HSO4- • HSO4-( H+ and)SO4-2 • H2O ( H+ and)OH- • NH4+ ( H+ and)NH3 • NH3( H+ and)NH2-

  37. What is the conjugate acid of… • NO3- • C2O4-2 • HPO4-2 • HSO4- • H2O • F-

  38. What is the conjugate acid of… Base(gains H+ to form its)Conjugate acid • NO3- • C2O4-2 • HPO4-2 • HSO4- • H2O • F-

  39. What is the conjugate acid of… Base(gains H+ to form its)Conjugate acid • NO3-(+H+  ) HNO3 • C2O4-2 • HPO4-2 • HSO4- • H2O • F-

  40. What is the conjugate acid of… Base(gains H+ to form its)Conjugate acid • NO3-(+H+  ) HNO3 • C2O4-2(+H+  ) HC2O4- • HPO4-2(+H+  ) H2PO4- • HSO4-(+H+  ) H2SO4 • H2O (+H+  ) H3O+ • F-(+H+  ) HF

  41. Nomenclature • If the anion name then the acid name • ends in…. is…

  42. Fill in the blanks • HCl is _____________acid • HClO4 is _____________acid • HClO3 is _____________acid • HClO2 is _____________acid • HClOis _____________acid

  43. Fill in the blanks Hydrogen chloride Hydrogen perchlorate • HCl is _____________acid • HClO4 is _____________acid • HClO3 is _____________acid • HClO2 is _____________acid • HClOis _____________acid Hydrogen chlorate Hydrogen chlorite Hydrogen hypochlorite

  44. Nomenclature • If the anion name then the acid name • ends in…. is… • --ide Hydro___ic acid • (hypo--) --ite Hypo___ous acid • --ite ___ous acid • --ate ___ic acid • (per--) –ate Per ___ic acid

  45. Fill in the blanks • HNO3 is _____________acid • HIO4 is _____________acid • H2CO3 is _____________acid • H3PO3 is _____________acid • HBrOis _____________acid

  46. Fill in the blanks • _____________is hydrocyanic acid • _____________is perbromic acid • _____________is phosphoric acid • _____________is sulfurous acid • _____________is hypoiodous acid

  47. Show the conjugate acid/base pairs in the following reactions. • C2O4-2 + H3O+ HC2O4- + H2O • CH3COOH + NH2-  NH3 + CH3COO-

  48. Show the conjugate acid/base pairs in the following reactions. Acid • C2O4-2 + H3O+ HC2O4- + H2O • CH3COOH + NH2-  NH3 + CH3COO- ConjugateBase Conjugate Acid Base

  49. Show the conjugate acid/base pairs in the following reactions. Acid • C2O4-2 + H3O+ HC2O4- + H2O • CH3COOH + NH2-  NH3 + CH3COO- ConjugateBase Conjugate Acid Base Conjugate Acid Base Acid ConjugateBase

  50. [H+] is inversely related to [OH-] • When [H+] increases, [OH-] decreases in a water solution, and vice versa.

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