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15.4 NOTES Acids and Bases

Explore the properties of acids and bases, learn about the pH scale, and understand buffer systems. Discover Arrhenius' definition, neutralization, strengths of acids and bases, reversible reactions, and the significance of concentration. Uncover how to interpret the pH scale, identify strong and weak acids/bases, and the concept of dynamic equilibrium. Delve into natural buffers, the relationship between strength and concentration, and differentiate between true and false statements in acid-base chemistry.

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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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