1 / 18

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

rashad
Download Presentation

Warm Up

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related