Titration notes Name ___________________________________________ Warm up: How many moles of ammonia are in 75 milliliters of a 0.75M solution? How many moles of hydrochloric acid are in 25.0 mL of a 0.500 M solution? Acid base reaction Ammonia, NH3 is a base. It reacts with hydrochloric acid according to the following equation. Calculate the concentration of 25 mL of an HCl solution if it requires 45.5 mL of 0.75M NH3 solution to neutralize it. NH3 (aq) + HCl (aq) → H2O (l) + NH4Cl (aq) Titration What is the purpose of titration? What is the relationship between titration and neutralization? What is the equivalence point? Titration practice Log on to your text – you will not be going to your text but rather will be using the resources! Follow these steps: 1. Select the “menu” hamburger in the top left 2. Choose “resources” 3. Select “chapter 18” and “section 4: Neutralization” from the drop down menus 4. Find and choose the “animation: Neutralization” 5. You are now ready to begin. Start with the HCl/NaOH titration and answer the following before pressing any more buttons. 1. What is the balanced chemical equation for the reaction between hydrochloric acid and sodium hydroxide? 2. Which chemical is the titrant? 3. What is the concentration of the HCl? _________ What volume is in the flask? __________ 4. How many moles of HCl are in the flask? (show your work) 5. What is the concentration of the NaOH? __________________ 6. How many moles of NaOH will you need to neutralize the HCl? 7. Calculate how many milliliters of this NaOH solution you will need to neutralize the acid. 8. Check your work by pressing the correct volume button. Were you right? ___________________ 9. Revise your work above if necessary. What happens at the molecular level at the equivalence point? _______________________________________ _________________________________________________________________________________________ Draw diagrams below to show this Before the equivalence point At the equivalence point .