1. Warm-up A patient weighing 100 lbs needs to receive 0.06 ml antibiotics per kg body weight. Calculate the dose lbs → kg → dose 100 lbs x 1 kg x 0.06 ml = 2.7149321 1 2.21 lbs kg = 2.71ml

2. Titration is a Quantitative Analysis Method: How to find the concentration of a solution?

3. Review: Constructing Ionic Compound Formulas and Names Cation is first, Anion is second in formula Cation Anion Mg 2+ OH 1 - Criss Cross Applesauce: Cross numbers in front of charges: 2 and 1 And place in formula number place Mg 1 OH 2 Name: 1.Cation (unaltered) 2. Anion name ends with –ide, -ate, -ite Magnesium Hydroxide: Mg(OH) 2

4. Form ionic compounds from the following elements 1.Aluminum and Chlorine AlCl 3 2. Ammonia and Oxygen (NH 4 ) 2 O 3. Potassium and Sulfate K 2 SO 4 4. Calcium and Carbonate CaCO 3

5. Acids and Bases Acids (ionic cps) produce H+ ions when they dissociate HCL→ H + + Cl - Bases (ionic cps) produce OH - ions NaOH → Na + + OH - Acids and Bases neutralize each other Neutralization Rx: Acid + Base → Salt + H 2 O HCl + NaOH → NaCl + H 2 O

6. Write and Balance the Neutralization Rx below HCl + Mg(OH) 2 H 2 SO 4 + Ca(OH) 2 The titration we are doing is an Acid/Base Titration

7. Titration equipment Quantitative analysis technique Burette Titrant Analyte

8. Vocab Burette: measures dispensed amounts, contains titrant Titrant: solution with known molarity that reacts in a known stoichiometry with the analyte Analyte: solution with unknown molarity, to be quantified Indicator: compound that changes color (Phenophthalein, pink) Endpoint: permanent color change when all analyte and titrant have reacted

10. Endpoint Titration titration video

11. Acid/BaseTitration Math M acid x V acid = M base x V base M = Molarity (moles/liter) Solve for missing molarity This formula works only for monoprotic acids/bases!!! (A/B that release 1 H+/OH-)

12. P1: 500 ml of an 2.5M HCl titrated 300 ml of NaOH of unknown concentration to the endpoint, what’s the concentration of the NaOH?

13. Warm-up Dissociate the following A/B H 2 SO 4 → Al(OH) 3 → H 3 PO 4 → 30 ml of 2M HCL is used to neutralize 25ml of an unknown KOH. What the concentration of the base?

14. Multiprotic Acids/Bases A/B that release more than one ion or ions with multiple charges Examples: Sulfuric Acid H 2 SO 4 → 2H + + SO 4 2- diprotic acid Al(OH) 3 → Al 3+ + 3OH - triprotic base

15. Titration Formula changes when you use di/triprotic a/b P2: 10 ml of 0.5 M Ca(OH) 2 are used to titrate 10 ml of HCl. Calculate the concentration of the acid. Ma x V a = 2 Mb x Vb Ma = 2Mb x Vb = 2x 0.5M x 10 ml = 1M HCL Va 10 ml

16. P3: 20 ml of 0.5 M Ca(OH) 2 are used to titrate 10 ml of H 2 SO 4. Calculate the concentration of the acid. 2Ma x V a = 2 Mb x Vb Ma = 2Mb x Vb = 0.5M x 20 ml = 1M H2SO4 2 Va 10 ml

17. P4: 15 ml of 0.5 M Ca(OH) 2 are used to titrate 10 ml of H 3 PO 4. Calculate the concentration of the acid. 3Ma x Va = 2 Mb x Vb Ma = 2Mb x Vb = 2x 0.5M x 15 ml = 0.5M 3Va 3 x 10 ml

18. P5: 30 ml of 0.7 M Carbonic Acid are used to titrate 10 ml of Aluminum Hydroxide. Calculate the concentration of the base.

19. 55 ml of 0.7 M Sulfuric acid are used to titrate 15 ml of Sodium Hydroxide. Calculate the concentration of the base.

20. Warm-up 50 ml of an 0.25M KOH were used to titrate 30 ml of HF of unknown concentration to the endpoint, what’s the concentration of the HF? Draw a picture Write the neutralization Rx Write and solve original titration formula Substitute, solve