Before the Bell Rings HW check will be at end of class.

ETD 63 2019 What is the pH of a 0.012 M HCl solution? What is the pH of a solution if [OH-] is 1.0 x 10-3 M? How many grams of HNO3 are needed to give a pH of 3.65 in a 11.5L tank? (Molar mass for HNO3 is 63.1g/mol)

ETD 63Ans 2019 What is the pH of a 0.012 M HCl solution?

ETD 63Ans 2019 What is the pH of a solution if [OH-] is 1.0 x 10-3 M? What is the pH of a 0.012 M HCl solution? What is the pH of a solution if [OH-] is 1.0 x 10-3 M?

ETD 63 2019 How many grams of HNO3 are needed to give a pH of 3.65 in a 11.5L tank? (Molar mass for HNO3 is 63.1g/mol) What is the pH of a solution if [OH-] is 1.0 x 10-3 M? What is the pH of a 0.012 M HCl solution?

Learning Targets I can explain how to do a titration and what the equivalence point represents.

Tests Come finish/take missing tests. Corrections for all tests can be done. June 14th- Last day for corrections or late work to be done

Notebook Check Our final notebook check will be due next class. Grade yourself, checking ETDs #46-63 1 point for ETD# 1 point for question 1 point for answer This is optional for seniors.

Homework Review

Titration Notes

Titration Knowledge Background: When an acid and base are mixed, they form water and a salt (neutralization reaction) NaOH + HCl  H2O + NaCl We can determine how much base is needed to neutralize an acid using a titration

Titration Curves Delivery measured volume of a solution of known concentration (titrant) to analyze an unknown solution (analyte) Titrant = the thing being added (base in buret) Analyte = solution that’s being added to (acid in Beaker) Titrant added to the analyte until the solution has reached the Equivalence Point!

Equivalence point = Point where moles of acid = moles of base (reaction to completion) Not always pH of 7!!!!! Middle, near vertical part of the curve

Why is the pH not always 7 at Equiv. Pt.? Equivalence Point is where moles of acid = moles of base (NOT where [H+] = [OH-]) Strong Acid vs. Strong Base HCl gives off 100% of it’s H+; NaOH gives off 100% of it’s [OH-] 0.5M of HCl gives off [H+] of 0.5 0.5M NaOH gives off [OH-] of 0.5 [H+] = [OH-] = pH of 7

Why is the pH not always 7? Strong Acid vs. Weak Base: HCl gives off 100% of it’s H+; NH3 results in only 50% [OH-] 0.5M of HCl gives off [H+] of 0.5 0.5M NH3 gives off [OH-] of 0.25 [H+] > [OH-] = pH less than 7 at equivalence pt.

Easy way to remember Whatever is strong, the equivalence pH will be on that side of the scale. For example, a strong acid with a weak base will end up on the acidic side of the pH scale (pH<7). A strong base and a weak acid will end up being basic at equivalence (pH >7). Strong and strong, weak and weak, will both be an equivalence of about pH=7.

Learning Targets I can explain how to do a titration and what the equivalence point represents.

Home work Notebook check #46-#63 Make your notecard for the final Due next class Make your notecard for the final 3” x 5” card, front and back. Work on the semester final review packet