Part two of acid/base pH calculations Student will : if given pH calculate the hydronium ion concentration hydroxide ion concentration molarity of a solution Ws. 19.2

“If given pH…find antilog” negative # = [hydronium conc.] If pH is 7.40 what is the [hydronium] or the molarity? “If given pH…find antilog” negative # = [hydronium conc.] -7.40 enter [3.9810717 E -8 ] “secret….hydronium concentration is the molarity for an acid” BUT::::: if they also ask for hydroxide concentration one must use the equilibrium constant for water::::::::: Equilibrium Constant for water is Kw = 1 x 10-14 Kw = [H+] [OH-] Yellow 2nd log

The pH of an orange is 4.0pH. What are the [H30] and [OH] in this fruit? What is its Molarity?

2. Lemons have a pH 3.15. What are the hydronium and the hydroxide concentrations? What is its molarity?

What is the molarity if the pH is 12 What is the molarity if the pH is 12.9 for a Calcium hydroxide solution?

4. Given pH 5.5 for an acid solution. What is the molarity?

5. Given pH 8.8 for a base solution what is the molarity?

6. Given pH 6. 7, what is the molarity 6. Given pH 6.7, what is the molarity? What are the [hydronium] and the [hydroxide] ?

If the [H3O] for butter is 6.0 x 10-7 is it acidic, basic, or neutral?

8. If given the [OH] as 3.16 x 10-11, what is the hydronium concentration? What is the pH?

9. If given the [H3O] as 1.6 x 10-6, what is the hydroxide concentration? What is the pH?

Remember: 3 formulas: pH=-log[H3O] pOH=-log[OH] pH + pOH = 14 Remember: [H3O] is hydronium concentration or…..molarity for an Acid or…..H+ proton concentration Remember: [OH] is hydroxide concentration or molarity for a base Remember: if given pH use antilog to calculate [H3O] [OH] put pH in as negative number Remember: Kw = 1x10-14 Kw = [H3O] [OH]

If the pH=5.2 what is the [OH]? 6.31 x 10-6 1.58x 10-9 .716003344 8.8 x 10 -7

Part two of acid/base pH calculations Student will : if given pH calculate the hydronium ion concentration hydroxide ion concentration molarity of a solution Ws. 19.2