Warm Up
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Transcript of Warm Up
*Warm Up
*Name the following acids:
*HI
*HNO3
*HCl
*Write the formula for the following acids:
*Hydrofluoric Acid
*Nitrous Acid
*Hydrobromic acid
*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.
*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
*Hydronium
*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!
*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