1. Neutralization Reactions Ex: HCl + NaOH NaCl + HOH

2. These are double replacement reactions Ions switch partners. Water is formed. http://www.youtube.com/watch?v=8IRI5gPR5EY&safe=active

3. Neutralization Forms Water H + + OH -  H 2 O H + + OH -  H 2 O from acid from base neutral from acid from base neutral This “net” reaction for neutralization is found on Table I. It is an exothermic reaction.

4. Forming a Salt (+) cation from the base (-) anion from the acid combine to form a salt.

5. If equal concentrations of hydrogen ion H + and hydroxide ions OH - are mixed, it results in a neutral solution. Ex:.1M LiOH +.1M HCl = Neutral Solution pH = 7

6. Completing and Balancing Neutralization Equations Write charges for ions in acid and base. Write charges for ions in acid and base. Switch ion partners. (+ ions stay in front!!) Switch ion partners. (+ ions stay in front!!) Do not bring over subscripts except if part of a polyatomic ion! Do not bring over subscripts except if part of a polyatomic ion! Criss-Cross charges to balance formulas. Criss-Cross charges to balance formulas. Balance entire equation. Balance entire equation. Name the acid, base and salt. Name the acid, base and salt.

7. You Try It Complete equation and balance formulas Complete equation and balance formulas Balance equation. Balance equation. Name acid base and salt Name acid base and salt Ex:KOH + H 2 SO 4 KOH + H 2 SO 4 HOH + K 2 SO 4 Ex: Mg(OH) 2 + HNO 3 Mg(OH) 2 + HNO 3 HOH + Mg(NO 3 ) 2

8. Hydrolysis Opposite reaction to neutralization Opposite reaction to neutralization Salt + Water Acid + Base

9. Parent Acid/Base If you know the salt involved you should be able to determine which acid and base it would form if water is added. If you know the salt involved you should be able to determine which acid and base it would form if water is added. Salt + Water Acid + Base Ex: NaCl with water (HOH) would form HCl and NaOH

10. You Try It Name the “parent” acid and base that would be produced from these salts. Name the “parent” acid and base that would be produced from these salts. Ex:Potassium chloride Ex:Potassium chloride Magnesium carbonate

11. Let’s Practice Which substance is always a product when an Arrhenius acid in an aqueous solution reacts with an Arrhenius base in an aqueous solution? Which substance is always a product when an Arrhenius acid in an aqueous solution reacts with an Arrhenius base in an aqueous solution? (1) HBr (2) KBr (3) H 2 O (4) KOH

12. Which word equation represents a neutralization reaction? Which word equation represents a neutralization reaction? (1) base + acid → salt + water (2) base +salt → water + acid (3) salt + acid → base + water (4) salt + water → acid + base

13. What are the products of a reaction between KOH(aq) and HCl(aq)? What are the products of a reaction between KOH(aq) and HCl(aq)? (1) H 2 and KClO (2) KH and HClO (3) H 2 O and KCl (3) H 2 O and KCl (4) KOH and HCl

14. Sulfuric acid, H 2 SO 4 (aq), can be used to neutralize barium hydroxide, Ba(OH) 2 (aq). What is the formula for the salt produced by this neutralization? Sulfuric acid, H 2 SO 4 (aq), can be used to neutralize barium hydroxide, Ba(OH) 2 (aq). What is the formula for the salt produced by this neutralization? (1) BaS (1) BaS (3) BaSO 3 (2) BaSO 2 (2) BaSO 2 (4) BaSO 4

15. Which compound could serve as a reactant in a neutralization reaction? Which compound could serve as a reactant in a neutralization reaction? (1) NaCl (1) NaCl (2) CH 3 OH (3) KOH (3) KOH (4) CH 3 CHO

16. Answer: 3

17. Titrations Purpose: To determine the concentration of an acid or base through a neutralization reaction.

18. Acid/Base Titration Buret is filled with a “standard solution” of known concentration (M). Erlenmeyer Flask contains solution of unknown conc.. Indicator (phenolphthalein) added to the flask.

19. Acid/Base Titrations Slowly “titrate” or drip liquid into flask from buret until indicator changes color. This is the “endpoint” or “equivalence point”. (Moles H + = Moles OH - ) Record total volume (V) used from buret.

20. Titration Formula M x V = M x V M A x V A = M B x V B Molarity Acid x Volume Acid = Molarity Base x Volume Base

21. Titration Applet http://group.chem.iastate.edu/Greenbowe/se ctions/projectfolder/flashfiles/stoichiometry /acid_base.html http://group.chem.iastate.edu/Greenbowe/se ctions/projectfolder/flashfiles/stoichiometry /acid_base.html

22. You Try It! A 50 ml sample of.2M HCl is neutralized by 75ml of NaOH. What is the conc. of the base? HCl NaOH HCl NaOH.2M x 50ml = M B x 75ml.2M x 50ml = M B x 75ml M B =.13M

23. Important Note Multiply acid/base side of equation by number of H + or OH - ions it produces when dissociating!!! Multiply acid/base side of equation by number of H + or OH - ions it produces when dissociating!!! Ex: Ex: H 2 SO 4 produces 2 H + so you would multiply the acid side by “2”

24. You Try It! How much of a.1M H 2 SO 4 solution is needed to neutralize 50 ml of a.05 KOH solution? H 2 SO 4 KOH H 2 SO 4 KOH 2 x.1M x V A =.05M x 50ml 2 x.1M x V A =.05M x 50ml V A = 12.5 ml

25. Titration Demonstration http://www.youtube.com/watch?v=5BZ0MPI geEE&safe=active http://www.youtube.com/watch?v=5BZ0MPI geEE&safe=active

26. Let’s Practice During which process can 10.0 milliliters of a 0.05 M HCl(aq) solution be used to determine the unknown concentration of a given volume of NaOH(aq) solution? During which process can 10.0 milliliters of a 0.05 M HCl(aq) solution be used to determine the unknown concentration of a given volume of NaOH(aq) solution? (1) evaporation (1) evaporation (2) filtration (3) distillation (3) distillation (4) titration

27. The data collected from a laboratory titration are used to calculate the The data collected from a laboratory titration are used to calculate the (1) rate of a chemical reaction (2) heat of a chemical reaction (3) concentration of a solution (4) boiling point of a solution

28. A student completes a titration by adding 12.0 ml of NaOH(aq) of unknown concentration to 16.0 ml of 0.15 M HCl(aq). What is the molar concentration of the NaOH(aq)? (1) 0.11 M (1) 0.11 M (2) 1.1 M (3) 0.20 M (3) 0.20 M (4) 5.0 M