acid – a compound that produces ions when dissolved in examples: vinegar – lemon juice – ...
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Acid – a compound that produces ions when dissolved in
Examples: Vinegar – Lemon juice – Tea – Ant venom –
taste Turns litmus paperReacts with metals to form gas solutions of acids are (must be mixed
with water!)Reacts with to form and
Sugar, corn syrup, modified corn starch, citric acid, tartaric acid, natural and artificial flavors, yellow 5, yellow 6, red 40, blue 1
What ingredients make these…
so sour?
H + polyatomic ionBegin with
ion without the
Add suffix if there was an Add suffix if there was an
HNO3
acids – completely in water (create a lot of ) 3 binary acids
Ternary acidsStrong if # of atoms - # of atoms ≥
H2SO4 HNO3
acids – ionize only in
solution Binary acids – all others not listed above Ternary acids
Weak if # of atoms - # of atoms ≥
H3PO3 HNO2
Base – a compound that produces ions
when dissolved in
Examples: Milk of Magnesia – neutralizes
stomach acid
Drain cleaner–
bases – completely in water (create a lot of ions).
All hydroxides with groups and metals (except ).
bases - only
All bases not listed above as strong.
An acid must contain a and ionize in water to produce
An base must contain aand dissociates in water to produce
Only compounds with can be classified as a base. What about ammonia, ?
Can only be applied to reactions that occur in
Would classify some compounds as acids, such as
Classify each of the following as anArrhenius acid (A – acid) or base (A – base).
Ca(OH)2
HBr
H2SO4
LiOH
A Bronsted – Lowry is any substance that can a
A Bronsted – Lowry is any substance that can a
HCl + H2O H3O+ + Cl-
acid – formed
when a
accepts a H+ from an acid.
base – a
that remains after an acid gives up a
H+.
Conjugate acid – base pair – 2 substances
related to each other by the
of a single H+.
Defined by how many H+ they can donate.
Type # of H+ donated
Example
Monoprotic 1 HNO3
Diprotic 2 H2SO4
Triprotic 3 H3PO3
Give the formula and name of the conjugate base of the following B-L acids.
(After the B-L acid donates a H+)
HI
HCO3-
Give the formula and name of the conjugate acids of the following B-L bases.
(After the B-L base accepts a H+)
H2PO4-
ClO3-
Water can sometimes act as a B-L acid and sometimes as a B-L base.
The of water:
H2O + H2O H3O+ + OH-
[H+] are often small, so the pH scale is easier to use to represent acidity and basicity.
pH range is from to
log 102 =
log 10-3 =
If [OH-] = 1.0 x 10 –10 M, what is the pOH?
What is the pH?
Is the solution basic, neutral, or acidic?
Acids LOSE H+ to become conjugate bases.
This is a H atom.
When a H+ is lost from an acid, this (-) electron remains.
The (+) proton is taken with the H.
+o
-
What is the conjugate base for the acid HBr?
HBr H+ + Br-
H Br
H Br+ -
Proton is keptby H.
Electron is leftby H.
Conjugate base
+
What is the conjugate base for the acid HNO2?
HNO2 H+ + NO2-
HNO
2
H+ -
Proton is keptby H.
Electron is leftby H.
Conjugate base
NO2
+
What is the conjugate base for the acid HSO3
-?
HSO3- H+ + SO3
2-
H SO3
H+ 2-
Proton is keptby H.
Electron is left by H (added to the one that was there already).
Conjugate base
SO3+
-
Bases GAIN H+ to become conjugate bases.
What is the conjugate acid for CN-?
CN- + H+ HCN
H CN++ -
H CN
The + and the – cancelout in the final molecule.
What is the conjugate acid for NH3?
NH3 + H+ NH4
+
H NH3
++
H
There is no – on the NH3 to cancelthe + from H, so the final moleculeis positive.NH
3
+
Example 1: Determine the pH of a 0.01 M HCl solution.
Example 2: Determine the pH of a 0.0010 M NaOH solution.
Example 3: Determine the pH of a 0.150 M KOH solution.
Example 4: Find [H3O+] for a solution that has a pH of 3.0.
Example 5: Find [H3O+] for a solution that has a pH of 8.2.
Example 6: Find [H3O+] and pOH for a solution that has a pH of 4.85.
What happens with you mix an acid with a base? A reaction
HCl + NaOH +
Products are always a ( and ) and
This is called a reaction
What happens with you mix an acid with a base? A ____________________________________________ reaction
Write the balanced chemical equation for the neutralization reaction between:nitric acid and potassium hydroxide
Write the balanced chemical equation for the neutralization reaction between:sulfuric acid and magnesium hydroxide
Titration – a process in which an acid-base neutralization reaction is used to determine the of a solution.
1. How many mL of 0.45 M HCl acid must be added to 25.0 mL of 1.00 M KOH to make a neutral solution?
2. What is the molarity of nitric acid if 15.0 mL of the solution is completely neutralized by 38.5 mL of 0.150 M NaOH?
3. A 25.0 mL solution of sulfuric acid is completely neutralized by 18 mL of 1.0 M LiOH. What is the concentration of the H2SO4 solution?