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There are H and OH ions in all solutions In neutral solutions H OH 1 x10 7 M If H gt1 x10 7 M solution is acidic ID: 1011562
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1. pH
2. Concentration [ ] – bracket notation is used to show concentrationThere are H+ and OH- ions in all solutionsIn neutral solutions: [H+] = [OH-] = 1 x10-7 MIf [H+] >1 x10-7 M, solution is acidicIf [OH-] > 1 x10-7 M, solution is basicFor all solutions [H+][OH-] = 1 x10-14
3. For a .0001 M solution of HNO3 what is the [H+] and [OH-] ?
4. Determine the [H+] in a solution that is .003 NaOH. 0.003 M3 x 10-3M3.33 x10-12M3 x 10-17M
5. What is the [OH-] of a .0065M Ca(OH)2 solution?.0065 M.013 M.00325 M1 x 10-6.5
6. What is the [H+] of a .0065M Ca(OH)2 solution?7.7 x10 -13.00651.5 x 10 -12.00325
7. pHShorthand notation for concentration pH = - log [H+]pH range pH less than 7 - acid pH equal to 7 - neutral pH greater than 7 - base
8.
9. ExampleWhat is the pH of a .00036M HCl solution?
10. pOH pOH = -log [OH-]
11. Relationship Between pH and pOH pH + pOH = 14
12. ExampleWhat is the pH and pOH of a .00082 M KOH solution?
13. ExampleWhat is the pH and pOH of a solution whose [H+] = 1.5x10-3M ?
14. What is the pH of a .00075 M KOH solution?7.5 x 10-43.1210.887
15. pH calculations – Solving for H+If the pH of Coke is 3.12, [H+] = ???10-pH = [H+]
16. What is the [H+] of a solution with a pH of 2.5?3.2 x 10-311.53.12 x 10-12.39
17. What is the [OH-] in a solution with a pH of 8.6?5.44 x 10-62 x 10-98.6