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15.4 NOTES Acids and Bases

15.4 NOTES Acids and Bases. C.4 Structure Determines Properties Arrhenius definition of acids and bases Acid – a substance that generates hydrogen ions when dissolved in water Base – generates hydroxide (-OH) when dissolved in water “OH is your home base ”

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15.4 NOTES Acids and Bases

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  1. 15.4 NOTESAcids and Bases

  2. C.4 Structure Determines Properties • Arrhenius definition of acids and bases • Acid – a substance that generates hydrogen ions when dissolved in water • Base – generates hydroxide (-OH) when dissolved in water • “OH is your home base” • Combining the two creates a hydronium ion (H3O+)

  3. Most acids have hydrogen atoms that can be released in water • H ____, H2_____, H3_____ • Ex: HNO3, H2S, H3PO4 • Form anion and hydronium when dissolved in water

  4. Bases have a cation and a hydroxide ion • ___OH, ___(OH)2, ___ (OH)3 • Ex. NaOH,Sr(OH)2, Al(OH)3 • Form cation and OH- when dissolved in water

  5. Neutralization • Mixing equal amounts of acid and base, forming water and a salt as the products • A salt is made from a cation (+) and an anion (-) charge • Neutral solutions • Concentrations of hydronium and hydroxide are small and equal

  6. Acidic solutions (H+) • Hydronium concentration is higher than hydroxide (OH-) • Very acidic solutions have very large hydronium concentrations • Basic solutions • Hydroxide(OH-) concentration in higher than hydronium (H+) • Very basic solutions have very largehydroxide concentrations

  7. The pH scale • Related to hydrogen/hydronium concentration present in solution • pH stands for power of hydronium ion, where power is the power of 10 that expresses the hydrogen ion’s molar concentration

  8. 100 - 1014 • Closer to 0, the more acidic the substance is, the closer to 14, the more basic the substance • pOH can measure alkalinity, or how basic the solution is or how much hydroxide is present • The scale is opposite the pH scale; bases are close to O and acids are close to 14

  9. You can look at this as a number line:

  10. C.7 Interpreting the pH Scale – Complete the following chart.

  11. C.8 Strengths of Acids and Bases • Ionization – when acids and bases break apart into ions

  12. Strong acids and Strong bases- break apart completely in water and don’t reform the original acid or base • There are 6 strong acids • HI, HBr, HCl, HNO3, H2SO4, and HClO4, all other acids are weak • Strong bases start with a cation that is in group 1 or 2 on the periodic table • LiOH, NaOH, KOH, RbOH, Mg(OH)2, Sr(OH)2, Ba(OH)2 • Weak acids/bases- only partially break apart in water

  13. Reversible reactions • Weak acids can proceed at an equal rate in each direction • Dynamic equilibrium • Forward reaction goes at the samerateas the reverse reaction • Forward/reverse rates are equal, not the amounts of products • They take the same amount of time to undergo the reaction • Strong acids/bases typically are not reversible

  14. C.10 Acids, Bases, and Buffers • Some lakes/rivers aren’t affected by acid rain • Buffers • Substances capable of neutralize an acid or base without changing the pH • need: • To neutralize an acid, you add a base • To neutralize a base, you add an acid • Natural buffers are found in blood and stomach

  15. Strength vs. Concentration • Strength – measure of how many ions are produced when acid/base is dissolved in water • Strong acid/base – all (or nearly all) acid/base have reacted with water to produce ions • Weak acid/base – acid/base has partially formed ions in water

  16. Concentration – measure of how many particles (molecules or ions) are dissolved in a solutions • Concentrated acid/base – a very large number of particles are dissolved • Dilute acid/base – a low number of particles are dissolved

  17. True or false • It is possible to have a strong acid that is dilute • True • It is possible to have a weak base that is concentrated true • True

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