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Strengths of Acids Arrhenius & Bronsted-Lowry definition: gives H+, hydronium ions in solution

Strong acids break down 100% in solution HCl hydrochloric acid HNO 3 nitric acid HBr hydrobromic acid. Weak acids do NOT break down completely. Strengths of Acids Arrhenius & Bronsted-Lowry definition: gives H+, hydronium ions in solution. H 2 S. More break down = stronger acid. HCl. H +.

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Strengths of Acids Arrhenius & Bronsted-Lowry definition: gives H+, hydronium ions in solution

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  1. Strong acids break down 100% in solution HCl hydrochloric acid HNO3 nitric acid HBr hydrobromic acid Weak acids do NOT break down completely Strengths of AcidsArrhenius & Bronsted-Lowry definition:gives H+, hydronium ions in solution H2S More break down = stronger acid HCl H+ Cl- H+ H+ S-2 H+ Cl- Cl- H2S Cl- H2S H+

  2. Strong will light a bulb brightly! Weak will make the bulb light dimly. Strong vs Weak

  3. Strong bases break down 100% in solution KOH Ba(OH)2 CsOH NaOH Weak bases do not break down completely Ca(OH)2 LiOH RbOH Strong BasesArrhenius definition = donates OH-Bronsted-Lowry definition = accepts H+Strength is determined the same way as acidsMore break down = stronger base

  4. Battery Acid & HF pH Scale Stomach acid, HCL Lemon juice, vinegar orange juice, • pH = power of hydrogen • pH = -log [H+] • Each time you change a number on the scale you change by a factor of 10 • pH of 3 is 10 times less acidic as pH of 2 • pH of 1 is 100 times more acidic as pH 3 Tomato juice, acid rain Black coffee Urine, saliva PURE water Salt water Baking soda Great Salt Lake Ammonia Soapy Water Bleach Liquid Drain Cleaner

  5. Neutralization • Acid + Base  Salt + H2O • A salt is a metal and non-metal (not just NaCl) • HCl + NaOH  NaCl + H2O • HCl + Ca(OH)2  CaCl2 + H2O

  6. Titrations • Technique used by chemists to determine an unknown molarity of a substance • We can use an indicator (changes color) to tell us when we are neutral (moles of acid = moles of base) link

  7. Titration Calculations Moles of Acid = Moles of Base M1V1=M2V2

  8. Titration Problemsacid = baseM1V1= M2V2 1. What is the molarity of a CsOH solution if 30.0mL of the solution is neutralized by 26.4 mL of a 0.250 M HBr solution?

  9. Titration Problemsacid = baseM1V1= M2V2 2. What is the molarity of a nitric acid if 43.33 mL 0.100 M KOH solution is needed to neutralize 20.0mL of HNO3?

  10. Titration Problemsacid = baseM1V1= M2V2 3. What is the concentration of a household ammonia cleaning solution if 49.9 mL 0.59 M HCl is required to neutralize 25.00 mL solution?

  11. Titration Problemsacid = baseM1V1= M2V2 4. What is the molarity of an NaOH solution if 50 mL of the solution is neutralized by 37 mL of 0.5 M HCl?

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