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Acid/Base Practice

Acid/Base Practice. Pop Quiz!. Name 3 characteristics of both acids and bases. Describe what an indicator is and what we have used them for in this class. Calculate the pH of the following: [H+]=1.47 x 10 -4 M [OH-]=3.55 x 10 -6 M [OH-]= 4.2 x 10 -2 M [H+]= 1.78 x 10 -4 M. *.

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Acid/Base Practice

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  1. Acid/Base Practice

  2. Pop Quiz! • Name 3 characteristics of both acids and bases. • Describe what an indicator is and what we have used them for in this class. • Calculate the pH of the following: • [H+]=1.47 x 10-4 M • [OH-]=3.55 x 10-6 M • [OH-]= 4.2 x 10-2 M • [H+]= 1.78 x 10-4 M *

  3. Pop Quiz! • Calculate the [OH-] concentrations of the following: • pOH=7.3 • pOH= 6.32 • pH= 1.5 • Calculate the [H+] concentrations of the following: • pH= 3.45 • pOH=8.2 • pH= 6.1 * *

  4. Pop Quiz! • Complete, balance and name the compounds in the following neutralization reactions • HCl + KOH  • H2SO4 + NaOH  *

  5. Pop Quiz! • If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? • If it takes 50 mL of 0.5 M KOH solution to completely neutralize 135 mL of sulfuric acid solution, what is the concentration of the sulfuric acid solution? *

  6. ANSWERS! • Acids: • Sour taste • Corrosive • pH less than 7 Bases: • Bitter taste • Corrosive • pH greater than 7 • Slippery feel

  7. ANSWERS! • Indicators turn color in a specific range of pH. We can use them in titrations to tell when an endpoint has been reached.

  8. ANSWERS! 3. Calculate the pH a. [H+]=1.47 x 10-4 M -log[H+] = pH -log (1.47 x 10-4) =3.83

  9. ANSWERS! • Calculate the pH • [OH-] =3.55 x 10-6 -log[OH-]=pOH pH + pOH = 14  pH= 14 – pOH -log(3.55x 10-6)= 5.45 14 – 5.45=8.55 EXTRA STEP!!!

  10. ANSWERS! • Calculate the pH • [OH-] = 4.2 x 10-2 -log[OH-]=pOH pH + pOH = 14  pH= 14 – pOH -log(4.2 x 10-2)=1.4 14 –1.4= 12.6 EXTRA STEP!!!

  11. ANSWERS! • Calculate the pH • [H+] = 1.78 x 10-4 -log[H+]=pH -log(1.78x 10-4) =3.75

  12. ANSWERS! • Calculate [OH-] • pOH=7.3 [OH-]= 10-pOH 10-7.3= 5.0 x 10-8

  13. ANSWERS! • Calculate [OH-] b. pOH= 6.32 [OH-]= 10-pOH 10-6.32 =4.79 x 10-7

  14. ANSWERS! • Calculate [OH-] c. pH=1.5 pH + pOH =14 14 – pH = pOH [OH-] = 10-pOH 14 – 1.5 = 12.5 10-12.5= 3.2 x 10-13 EXTRA STEP!!!

  15. ANSWERS! • Calculate [H+] • pH= 3.45 [H+]= 10-pH 10-3.45 =3.55 x 10-4

  16. ANSWERS! • Calculate [H+] b. pOH= 8.2 pH + pOH =14 14 – pOH =pH [H+]= 10-pH 14 – 8.2= 5.8 10-5.8=1.6 x 10-6 EXTRA STEP!!!

  17. ANSWERS! • Calculate [H+] c. pH= 6.1 [H+]= 10-pH 10-6.1=7.9 x 10-7

  18. ANSWERS! • Complete, balance and name. a. HCl + KOH

  19. ANSWERS! • Complete, balance and name. a. HCl + KOH  KCl + H2O ALREADY BALANCED! HCl: KOH: KCl: H2O: HydrochloricAcid PotassiumHydroxide PotassiumChloride Water

  20. ANSWERS! 6. Complete, balance and name compounds b. H2SO4 + NaOH 

  21. ANSWERS! 6. Complete, balance and name compounds b. H2SO4 + NaOH  Na2SO4 + H2O

  22. ANSWERS! 6. Complete, balance and name compounds b. H2SO4 + 2NaOH  Na2SO4 + 2H2O BALANCED! H2SO4: NaOH: Na2SO4: H2O: Sulfuric Acid Sodium Hydroxide Sodium Sulfate Water

  23. ANSWERS! 7. If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? Step 1: Write and balance the neutralization reaction: HCl + NaOH  NaCl + H2O

  24. ANSWERS! 7. If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? Step 2: Identify the known 54 mL of 0.1 M NaOH

  25. ANSWERS! 7. If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? Step 2: Identify the known 54 mL of 0.1 M NaOH

  26. ANSWERS! 7. If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? Step 3: Identify the number of moles of known using molarity and liters.

  27. ANSWERS! 7. If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? Step 4: Use the molar ratio to convert from known moles to unknown moles

  28. ANSWERS! 7. If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of the HCl? Step 5: Calculate the concentration (M) of HCl using the volume given in the problem.

  29. ANSWERS! 8. If it takes 50 mL of 0.5 M KOH solution to completely neutralize 135 mL of sulfuric acid solution, what is the concentration of the sulfuric acid solution? Step 1: Write and balance the neutralization reaction: H2SO4 + 2KOH  K2SO4 + 2H2O

  30. ANSWERS! 8. If it takes 50 mL of 0.5 M KOH solution to completely neutralize 135 mL of sulfuric acid solution, what is the concentration of the sulfuric acid solution? Step 2: Identify the known. 50 ml of 0.5 M KOH

  31. ANSWERS! 8. If it takes 50 mL of 0.5 M KOH solution to completely neutralize 135 mL of sulfuric acid solution, what is the concentration of the sulfuric acid solution? Step 2: Identify the known. 50 ml of 0.5 M KOH

  32. ANSWERS! 8. If it takes 50 mL of 0.5 M KOH solution to completely neutralize 135 mL of sulfuric acid solution, what is the concentration of the sulfuric acid solution? Step 3: Calculate the moles of the known using the volume (in Liters) and molarity.

  33. ANSWERS! 8. If it takes 50 mL of 0.5 M KOH solution to completely neutralize 135 mL of sulfuric acid solution, what is the concentration of the sulfuric acid solution? Step 4: Use the molar ratio to convert from known moles to unknown moles

  34. ANSWERS! 8. If it takes 50 mL of 0.5 M KOH solution to completely neutralize 135 mL of sulfuric acid solution, what is the concentration of the sulfuric acid solution? Step 5: Calculate the concentration (M) of HCl using the volume given in the problem.

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