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Warm Up

Name the following acids: HI HNO 3 HCl Write the formula for the following acids: Hydrofluoric Acid Nitrous Acid Hydrobromic acid. Warm Up. pH Calculations. Unit 10, Day 2 Kimrey 17 May 2013. Identify strong and weak acids

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Warm Up

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  1. Name the following acids: • HI • HNO3 • HCl • Write the formula for the following acids: • Hydrofluoric Acid • Nitrous Acid • Hydrobromic acid Warm Up

  2. pH Calculations Unit 10, Day 2 Kimrey 17 May 2013

  3. Identify strong and weak acids • Calculate the pH and pOHof an acid given a concentration. • Determine the concentration of an acid given a pH or pOH. Objectives

  4. There are two strengths of acids: strong and weak. • Strong acids completely dissociate (break up) in water. • Weak acids do not completely dissociate. • There are 6 strong acids. • HCl • HBr • HI • H2SO4 • HNO3 • HClO4 Strong Acids and Weak Acids

  5. pH is a logarithmic scale that measures the concentration of the [H+] ion in solution. • Goes from 0 -14 • 0 - 6.99 is acidic • 14 – 7.01 is basic • pH = -log[H+] • [H+]=10-pH pH

  6. Don’t freak over logs and anti-logs, your calculator does them for you! • Ex. Find the pH of a HCl solution with a H+ concentration of 1 x 10-6. • pH = -log[H+] • pH = 6 Logs and anti logs…oh my!

  7. When acids break up, the concentration of hydrogen is sometimes explained by using hydronium • Hydronium is H3O • Water + Hydrogen • Just do math the same way! Hydronium

  8. Find the pH of a 0.03 M solution of HBr. • pH = -log[H+] • pH = 1.5 Example

  9. What is the concentration of a HCl solution that has a pH of 3? • [H+]=10-pH • [H+] = .001M Example

  10. Same as pH, but opposite. • Goes from 0 -14 • 0 - 6.99 is basic • 14 – 7.01 is acidic • pOH = -log[OH-] • [OH-]=10-pOH pOH

  11. Calculate the pOH for a solution of NaOH with a concentration of 1 x 10-4 M. • pOH = -log[OH-] • pOH = 4 Example

  12. Calculate the pOH for a solution of KOH with a concentration of 0.45 M. • pOH = -log[OH-] • pOH = .35 Example

  13. What is the concentration of a solution the has a pOH of 13.5? • [OH-] = 10-pOH • [OH-] = 3.16 x 10 -14 M Example

  14. Remember that both the pH and pOH scale go from 0-14. • As the concentration of [H+] or [OH-] goes up the other must go down. • These two relationships allows us to assume that: • pH + pOH = 14 pH and pOH

  15. What is the pH of a solution that is found to have a pOH of 10? • pH = 4 Example

  16. What is the pH of a .067 M solution of LiOH? • pOH = 1.17 • pH = 12.8 Example

  17. What is the pOH of a 0.0056 M solution of HCl? • pH = 2.25 • pOH = 11.75 Example

  18. What is the pH of a solution HI with a concentration of .0089 M? • What is the concentration of a strong acid with a pH of 3.45? • What is the pH of a solution of a NaOH with a concentration of 5.67 x 10-4 M? Exit Card

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