*Name the following acids:
*HI
*HNO3
*HCl
*Write the formula for the following acids:
*Hydrofluoric Acid
*Nitrous Acid
*Hydrobromic acid
*
*
Unit 10, Day 2
Kimrey
3 January 2013
*
* 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
*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.
*
*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 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
*
*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
*
*Find the pH of a 0.03 M solution of HBr.
*pH = -log[H+]
*pH = 1.5
*
*What is the concentration of a HCl
solution that has a pH of 3?
*[H+]=10-pH
*[H+] = .001M
*
*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
*
*Calculate the pOH for a solution of NaOH
with a concentration of 1 x 10-4 M.
*pOH = -log[OH-]
*pOH = 4
*
*Calculate the pOH for a solution of
KOH with a concentration of 0.45 M.
*pOH = -log[OH-]
*pOH = .35
*
*What is the concentration of a solution the has a
pOH of 13.5?
*[OH-] = 10-pOH
*[OH-] = 3.16 x 10 -14
M
*
*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
*
*What is the pH of a solution that is
found to have a pOH of 10?
*pH = 4
*
*What is the pH of a .067 M solution
of LiOH?
*pOH = 1.17
*pH = 12.8
*
*What is the pOH of a 0.0056 M
solution of HCl?
*pH = 2.25
*pOH = 11.75
*
*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?
*