*Warm Up

*Name the following acids:*HI*HNO3

*HCl

*Write the formula for the following acids:*Hydrofluoric Acid*Nitrous Acid*Hydrobromic acid

Unit 10, Day 2Kimrey3 January 2013

*pH Calculations

*Homework Check*Chloric Acid*HClO4

*Nitric Acid*H2C2O4

*Phosphic Acid*HF*Hydroiodic Acid*HBr*Hydrochloric Acid*Hydrochloric Acid*Perchloric acid*Hydroiodic acid*Sulfic acid / Sulfuric acid*Hydrosulfic acid / Hydrosulfuric

acid*OMIT*Carbonic acid*Perbromic acid*Bromic acid*Acetic acid*OMIT*Hydrophosphic acid

*HF*HNO3

*HNO2

*H2CO3

*HMnO4

*H2Cr2O7

*H2SO3

*H2SO4

*HClO4

*HClO2

*HC2H3O2

*H3PO4

* 7-14*No, Bases aren’t sour* Salt + water*Acetic acid- food*H2SO4 - Battery Acid*NaOH- drano*Mg(OH)2 - antacid

*Objectives

*Identify strong and weak acids *Calculate the pH and pOH of an acid given a concentration. *Determine the concentration of an acid given a pH or pOH.

*Strong Acids and Weak Acids

*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 you need to memorize. *HCl*HBr*HI*H2SO4

*HNO3

*HClO4

*pH

*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

*Logs and anti logs…oh my!

*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

*Example

*Find the pH of a 0.03 M solution of HBr.

*pH = -log[H+]*pH = 1.5

*Example

*What is the concentration of a HCl solution that has a pH of 3?

*[H+]=10-pH

*[H+] = .001M

*pOH

*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

*Example

*Calculate the pOH for a solution of NaOH with a concentration of 1 x 10-4 M.

*pOH = -log[OH-]*pOH = 4

*Example

*Calculate the pOH for a solution of KOH with a concentration of 0.45 M.

*pOH = -log[OH-]*pOH = .35

*Example

*What is the concentration of a solution the has a pOH of 13.5?

*[OH-] = 10-pOH

*[OH-] = 3.16 x 10 -14 M

*pH and pOH

*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

*Example

*What is the pH of a solution that is found to have a pOH of 10?

*pH = 4

*Example

*What is the pH of a .067 M solution of LiOH?

*pOH = 1.17*pH = 12.8

*Example

*What is the pOH of a 0.0056 M solution of HCl?

*pH = 2.25*pOH = 11.75

*Exit Card

*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?