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Chapter 5: Acids and Bases 5.1

Chapter 5: Acids and Bases 5.1. Pages 220-253. Acids and Bases. Acids: chemical compounds that produce a solution with a pH of < 7 when dissolved in water ( aq ). Properties of Acids Contains H pH of < 7

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Chapter 5: Acids and Bases 5.1

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  1. Chapter 5: Acids and Bases5.1 Pages 220-253

  2. Acids and Bases Acids: chemical compounds that produce a solution with a pH of < 7 when dissolved in water (aq). Properties of Acids • Contains H • pH of < 7 • Produces salt and water when reacts with ionic compounds containing hydroxide (OH) ions (aka a base!) • Tart, sour taste (e.g. lemon juice) • Corrosive

  3. Bases:compounds that produce a solution with a pH > 7 when dissolved in water (aq). Properties of Bases (alkaline) • contain hydroxide ions:OH • pH > 7 • Produce salt and water when reacts with an ionic compound containing positive H ions (aka an acid!). • Slippery • Bitter taste • Corrosive

  4. BASE or ACID?

  5. pH Scale Number scale used to measure how acidic or basic a solution is.

  6. pH Scale • One unit of change represents a 10X change in the degree of how acidic or basic something is. Q: How much more basic is bleach than baking soda? A: 103 or 1000 times more basic. A: 102 or 100 times more acidic Q: How much more acidic is a lemon than a tomato?

  7. pH Indicators • Too dangerous to determine pH by touch or taste! A pH indicator is used to determine how basic or acidic a solution is. pH Indicators • chemicals that change colourdepending on the pH of the solution they are placed in. • Used to indicate whether a solution is an acid or base. My mouth is on fire!

  8. Different Types of pH Indicators 1. Litmus Paper 2. Universal Indicator: turns different colors depending on the pH. 3. Digital pH meter: measures the electrical (ionic) properties of a solution to determine the pH.

  9. Types of pH Indicators Cont’d • Acid-Base Indictors:

  10. Acids: HoW can you Tell?? Compounds don’t take on acidic properties until dissolved in water: HCl(aq). (aq) oraqueous refers to an acid when dissolved in water. How to Identify an Acid: • H on the Left: formula beginning with an H on the left side : Eg: HCl(aq), HNO3 (aq) • Exception: H on the right = when an acid contains carbon, the H may be written on the right side: Eg: CH3COOH(aq)

  11. Different ways to name acids If NO state is indicated: the acid then can be named beginning with hydrogen: Eg: HCl hydrogen chloride BUT… if the state IS indicated “(aq)” than the compound is named by its acidic name and ending in: “ …ic acid” Eg: HCl(aq) hydrochloric acid

  12. How to Name Acids: containing Oxygen 1. Non-Oxygen Acids (acids not containingO): insert “Hydro”(prefix) … “-ic” (suffix) end with acid. Eg: HBr(aq) = hydrobromicacid HF(aq) = hydrofluoricacid 2. Acids Containing Oxygen (O) A. Name starting with hydrogen and ending with –ate: - Drop hydrogen and change the – ate to “– ic acid” Eg: H2CO3 – hydrogen carbonate H2CO3(aq) – carbonic acid

  13. Naming Acids Cont’d B. Name starting with hydrogen and ending with –ite Drop hydrogen and change –iteto “–ous acid” Eg: H2SO3 - hydrogen sulfite H2SO3(aq) – sulfurous acid

  14. Bases How can you tell if a compound is a BASE? • Look for an OH (hydroxide) group on the right side of the formula. Some Common Bases: • NaOH (aq)- sodium hydroxide • Mg(OH)2(aq) - magnesium hydroxide

  15. Ion Production Acidic or Basic solutions conduct electricity: • Bases and acids form ions when they are dissolved in solution: • Acids: produce hydrogen ions (H+) • Bases: produce hydroxide ions (OH-) Ion Concentrations • Solutions with a high concentration of H+ ions are very acidic. • Solution with a high concentration of OH- ions are very basic.

  16. A solution can not have both H+ or OH-, thus acids and bases are chemical opposites. • When separate solutions of H+ and OH- ions are combined, they react and form water. H+ + OH- H2O Neutral Solution: When an acidic and basic solution are combined the solutions can neutralize each other.

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