Acids Lesson 20 Subtle Items.

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Presentation transcript:

Acids Lesson 20 Subtle Items

Subtle Acid Items 1. Weak bases neutralize a strong acid as well as a strong base would. HCl + NaOH HCl + HCO3- → NaCl + HOH → H2CO3 + Cl- Both reactions go to completion because of the strong acid.

2. H3BO3 H2CO3 HCl triprotic H3BO3 ⇌ H+ + H2BO3- diprotic H2CO3 ⇌ H+ + HCO3- monoprotic HCl → H+ + Cl- Only lose one proton when in water!

 Which neutralizes more NaOH? H3BO3 or HCl? H3BO3 + 3NaOH → Na3BO3 + 3HOH HCl + 1NaOH → NaCl + HOH

 3. Which determines acid strength? Molarity Ka is concentration Molarity Ka is concentration  is strength as indicated in the acid chart

   4. Which determines the pH = -Log[H+] Ka determines the [H+] = -Log[H+] Ka determines the [H+]  Molarity determines the [H+]  Temperature affects the Ka 

5. Pick the best conductor. 1 M NaCN 0.1 M HCl 0.1 M KOH 

 6. Pick the worst conductor. NaOH HCl NaCN NH3 NaOH HCl NaCN NH3  Good Conductors are….. Strong acids Strong Bases Soluble Salts

1 mole H2CO3 and 1mole NaHCO3 are dissolved in 0.5 L of water. What kind of solution results in the above mixture? Buffer Write an equation for the equilibrium. H2CO3 ⇋ H+ + HCO3- Label each chemical species with a concentration. 2 M Low 2 M What limits the ability to buffer against acid? [HCO3-] What limits the ability to buffer against base? [H2CO3]

8. Acid Base HF F- H3BO3 H2BO3- HCN CN- Put an asterisk next to the strongest acid and base What is the relationship between acid strength and strength of conjugate base? * * Inverse

9. What ions are in H2SO4 solution? H2SO4 → H+ + HSO4- HSO4- ⇌ H+ + SO42- [ OH-] because it is in water!

10. Which titration will have the equivalence point with 10. Which titration will have the equivalence point with lowest conductivity? HCl + NaOH → H2SO4 + Ba(OH)2 → NaCl(aq) + HOH High Solubility BaSO4(s) + 2HOH Low Solubility Lowest Conductivity

 11. What is the best acid for titrating 0.10 M NH3? 11. What is the best acid for titrating 0.10 M NH3? 0.00010 M HCl 0.10 M HF 6.0 M HCl 0.10 M HCl  Must be strong and about the same molarity!

12. HCl Molarity pH 10 M -1 1 M 0.1M 1 2 0.01M 0.001M 3 0.0001M 4

13. A 0.00010 M acid has a pH of 4.0. Is the acid strong or weak? Strong pH = -Log[0.00010] = 4.0 The pH is only at 1.0 M!

14. A 0.0010 M acid has a pH of 4.0. Is the acid strong or weak? Weak pH = -Log[0.0010] = 3.0 The pH is only at 1.0 M!

  15. HInd ⇌ H+ + Ind- It’s yellow in HCl and red in HCN Assign each colour Which is the stronger acid; HInd or HCN? HCN + Ind- ⇌ HInd + CN- What is favoured? Reactants yellow red  

16. Describe the buffer present in human blood. H2CO3 NaHCO3 17. What is stomach acid? HCl 18 . What is battery acid? H2SO4

 19. Match the Curve with the Reaction pH Volume 1.0 M NH3 added 14 7 30 60  A. 3HCl + Al(OH)3 → AlCl3 + 3HOH B. HCl + KOH → KCl + HOH C. HCN + KOH → KCN + HOH

 20. Match the Curve with the Reaction pH Volume 1.0 M NH3 added 14 7 30 60 A. 3HCl + Al(OH)3 → AlCl3 + 3HOH B. HCl + KOH → KCl + HOH C. HCN + KOH → KCN + HOH 

21. Write a reaction between NaHCO3 and NaHC2O4 HCO3- + HC2O4- ⇌ H2CO3 + C2O42- Are the reactants or products favoured? products

0.10 M Weak Acid 0.10 M Weak Base x2 x2 Kw = Ka = Kb = Ka 0.10 0.10