þ produce h + (as h 3 o + ) ions in water (the hydronium ion is a hydrogen ion attached to a water...
TRANSCRIPT
þ Produce H+ (as H3O+) ions in water (the hydronium
ion is a hydrogen ion attached to a water molecule)
þ Taste sour
þ Corrode metals (react to H2 (g))
þ Are electrolytes (conduct electricity)
þ React with bases to form a salt and water
þ pH is less than 7
þ Turns blue litmus paper to red “Blue to Red A-CID”
Some Properties of Acids
Produce OH- ions in water
Taste bitter, chalky
Are electrolytes (conduct electricity)
Feel soapy, slippery
React with acids to form salts and water
pH greater than 7
Turns red litmus paper to blue “Basic Blue”
Some Properties of Bases
HCl Hydrochloric Acid Stomach acid
HNO3 Nitric Acid Jewelry making
H2SO4 Sulfuric Acid Paper making; Car batteries
H3PO4 Phosphoric Acid Preservative in Coca-Cola
NaOH Sodium hydroxide lye
KOH Potassium hydroxide liquid soap
Ba(OH)2 Barium hydroxide stabilizer for plastics
Mg(OH)2 Magnesium hydroxide “MOM” Milk of magnesia
Al(OH)3 Aluminum hydroxide Maalox (antacid)
Some Common Acids & Bases- (video)
Definition #1: Arrhenius (traditional)
Acids – produce H+ ions (or hydronium ions H3O+)
Bases – produce OH- ions
(problem: some bases don’t have hydroxide ions!)
Acid/Base definitions
Arrhenius acid is a substance that produces H+ (H3O+) in water
Arrhenius base is a substance that produces OH- in water
Strong acid- ionizes completely in aqueous solutionStrong electrolytesHCl, HNO3
Weak acid- releases few hydrogen ions in aqueous solutionHCN and acetic acid (-COOH)
Strong base- ionizes completely in aqueous solutionStrong electrolytes
Weak base- releases few hydroxide ions in aqueous solution
Arrhenius Acids and Bases- (video)
HNO3, HCl, H2SO4 and HClO4 are among the only strong acids.
Strong and Weak Acids/Bases
The strength of an acid (or base) is determined by the amount of IONIZATION. STRONG=100% IONIZED
The strength of an acid (or base) is determined by the amount of IONIZATION. STRONG=100% IONIZED
Weak acids are much less than 100% ionized in water.
One of the best known is acetic acid = CH3COOH
Strong and Weak Acids/Bases
Strong and Weak Acids/Bases
Strong Base: 100% dissociated in water.
NaOH (aq) ---> Na+ (aq) + OH- (aq)
Strong and Weak Acids/Bases
Other common strong bases include KOH and Ca(OH)2.
CaO (lime) + H2O -->
Ca(OH)2 (slaked lime)CaO
Weak base: less than 100% ionized in water
One of the best known weak bases is ammonia
NH3 (aq) + H2O (l) NH4+ (aq) + OH-
(aq)
Strong and Weak Acids/Bases
Strong and Weak Acids/Bases
Acid/Base Definitions- (video)Definition #2: Brønsted
– Lowry
Acids – molecule or ion that is a proton donor
Bases – molecule or ion that is a proton acceptor
A “proton” is really just a hydrogen atom that has lost it’s electron!
A Brønsted-Lowry acid is a proton donorA Brønsted-Lowry base is a proton acceptor
acidconjugate
basebase conjugate
acid
ACID-BASE THEORIESACID-BASE THEORIESThe Brønsted definition means
NH3 is a BASE in water — and water is itself an ACID
BaseAcidAcidBaseNH4
+ + OH-NH3 + H2OBaseAcidAcidBase
NH4+ + OH-NH3 + H2O
Acids & Base Definitions
Lewis acid - a substance that accepts an electron pair
Lewis base - a substance that donates an electron pair
Definition #3 – Lewis Definition #3 – Lewis
Formation of hydronium ion is also an excellent example.
Lewis Acids & Bases
• Electron pair of the new O-H bond originates on the Lewis base.
HH
H
BASE
••••••
O—HO—H
H+
ACID
NO, NO2, CO2, SO2, and SO3 gases from industrial processes can dissolve in atmospheric water to produce acidic solutions.
Burning of fossil fuels by coal-burning power plants, factories, and automobiles
Very acidic rain is known as acid rain.
Acid rain can erode statues and affect
ecosystems.
Acid Rain
example: SO3(g) + H
2O(l) H
2SO
4(aq)
Amphoteric Compounds
Any species that can react as either an acid or a base is described as amphoteric.
example: waterwater can act as a base
H2SO
4(aq) + H
2O(l) H
3O(aq) + HSO
4Ğ(aq)
NH
3(g) + H
2O(l) NH
4(aq) OHĞ(aq)
acid1 base2 acid2 base1
water can act as an acid
base1 acid2 acid1 base2
More About WaterMore About WaterH2O can function as both an ACID and a
BASE.
In pure water there can be AUTOIONIZATION
Equilibrium constant for water = Kw
Kw = [H3O+] [OH-] = 1.00 x 10-14 at 25 oC
In the self-ionization of water, two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton.
Self-ionization or Autoionization of Water
H
2O(l) + H
2O(l) H
3O(aq) + OHĞ(aq)
-
Kw = ionization constant of water
Kw = [H3O+] [OH-] = 1.00 x 10-14 at 25 oC
In a neutral solution [H3O+] = [OH-]
so Kw = [H3O+]2 = [OH-]2
and so [H3O+] = [OH-] = 1.00 x 10-7 M
More About WaterMore About WaterOH-
H3O+
OH-
H3O+
Autoionization
Kw = [H+1][OH-1] = 1E-14
Used to find unknown [H+1] or [OH-1] if the other is known or given
If [H+1] = .0003M, find the [OH-1]
1E-14 = [.0003M] [OH-1]
[OH-1]=3.33E-11M
Kw: the Constant of Water or How to find the missing #
The pH scale is a way of expressing the strength of acids and bases. Instead of using very small numbers, we just use pH
Base 10 logarithms (log)The log of a number is the power to which 10
must be raised to get that numberlog 1000 = 3 because 103 = 1000log 0.1 = -1 because 10-1 = 0.1Use your calculator to solve
log (1.25*10-3) = -2.90-log (3.64*10-12) = 11.44
Logarithms
pH = - log [H+]Example: If [H+] =1E-10
pH = - log( 1E-10)pH = - (- 10)pH = 10
Example: If [H+] = 1.8E-5pH = - log 1.8E-5pH = - (- 4.74)pH = 4.74
Calculating the pH
Find the pH of these:1) A 0.15 M solution of Hydrochloric
acid (answer: .8239)2) A 3.00 X 10-7 M solution of Nitric
acid (answer: 6.5229)
STOP
Try These!
If the pH of Coke is 3.12, [H+] = ???
Because pH = - log [H+] then
- pH = log [H+]
Take antilog (10x) of both sides and get
10-pH = [H+][H+] = 10-3.12 = 7.6 x 10-4 M *** to find antilog on your calculator, look for “Shift” or “2nd
function” and then the log button
pH calculations – Solving for H+pH calculations – Solving for H+
A solution has a pH of 8.5. What is the Molarity of hydrogen ions in the solution?
pH calculations – Solving for H+
pH = - log [H+]
8.5 = - log [H+]
-8.5 = log [H+]
Antilog -8.5 = antilog (log [H+])
10-8.5 = [H+]
3.16E-9 M = [H+]
pH = - log [H+]
8.5 = - log [H+]
-8.5 = log [H+]
Antilog -8.5 = antilog (log [H+])
10-8.5 = [H+]
3.16E-9 M = [H+]
Since acids and bases are opposites, pH and pOH are opposites!
pOH does not really exist, but it is useful for changing bases to pH.
pOH looks at the perspective of a base
pOH = - log [OH-]Since pH and pOH are on
opposite ends,pH + pOH = 14
pOH
[OH-]
[H+] pOH
pH
10 -pOH
10 -pH-Log[H+]
-Log[OH
-]
14 -
pOH
14 -
pH
1.0
x 10-1
4
[OH
- ]
1.0
x 10-1
4
[H
+ ]
The pH of rainwater collected in a certain region of the northeastern United States on a particular day was 4.82. What is the H+ ion concentration of the rainwater? (answer: 1.51E-5M)
The OH- ion concentration of a blood sample is 2.5 x 10-7 M. What is the pH of the blood?(answer: 7.3979)
Calculating [H3O+], pH, [OH-], and pOH
Problem 1: Calculate the [H3O+], pH, [OH-], and pOH of a solution of 0.0024 M hydrochloric acid at 25°C.
[H3O+]= 0.0024 M
pH= 2.62
[OH-]= 4.17 E^-12M
pOH= 11.38
End
Problem 2: What is the [H3O+], [OH-], and pOH of a solution with pH = 3.67? Is this an acid, base, or neutral?
[H3O+]= 10^ -3.67 = 2.14E-4 M
[OH-]= 10^-14 / (2.14E-4) = 4.67E-11 M
pOH= 14 – 3.67 = 10.33
Acid
pH meterTests the voltage of the
electrolyteVoltage changes as
hydronium ion concentration changes
Converts the voltage to pHVery cheap, accurateMust be calibrated with a
buffer solution
pH indicatorsIndicators are compounds that will
change color in the presence of an acid or base.
Indicators are either weak acids or weak bases
Indicators only work in a specific range of pH
Some dyes are natural, like radish skin or red cabbage
Neutralization ReactionsStrong Acid-Strong Base NeutralizationIn aqueous solutions, neutralization is the
reaction of hydronium ions and hydroxide ions to form water molecules.
H3O+(aq) + OH(aq) 2H2O(l)
A salt is an ionic compound composed of a cation from a base and an anion from an acid.
HCl(aq) + NaOH(aq) NaCl(aq) H2O(l)
Titration is the controlled addition and measurement of the amount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentration.
The point at which the two solutions used in a titration are present in chemically equivalent amounts is the equivalence point.
The point in a titration at which an indicator changes color is called the end point of the indicator.
Titration
TitrationTitration1. Add solution from the buret
to the flask.2. Reagent (base) reacts with
compound (acid) in solution in the flask.
3. Indicator shows when exact stoichiometric reaction has occurred. (Acid = Base)
This is called the END POINT where NEUTRALIZATION has occurred.
Titration Math(short version)
M1 • V1 = M2 • V2
Moles H3O+ = Moles OH-
Titration using a pH MeterSet up the buret and the chemicals the same except no
Phenolphthalein is addedSet up the Nova with a pH sensor attached and insert the
probe into the Unknown solution. Proceed with the addition of the base solution until the graph looks like the one attached
The volume where the large
jump takes place is the End
Point, moles Base=moles AcidBegin calculations
Molarity and Titration
1. Start with the balanced equation for the neutralization reaction, and determine the chemically equivalent amounts of the acid and base.
2. Determine the moles of acid (or base) from the known solution used during the titration.
3. Determine the moles of solute of the unknown solution used during the titration using the balanced equation.
4. Determine the molarity of the unknown solution.
Problem: Determine the molarity of an acidic solution, 10 mL HCl, by titration.
(HCl of unknown molarity in the flask, 5.0 x 10-3 M NaOH in the buret)
Titrate the acid with a standard base solution 20.00 mL of 5.0 × 10−3 M NaOH was titrated
1. Write the balanced neutralization reaction equation. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
1 mol HCL reacts with 1 mol NaOH
Determine the chemically equivalent amounts of HCl and NaOH.
3. Calculate the number of moles of NaOH used in the titration. Then calculate the number of moles of HCl initially in the flask.
20.0 mL of 5.0 × 10−3 M NaOH is needed to reach the end point
-3-45.0 10 mol NaOH 1 L
20 mL 1.0 10 mol NaOH used1 L 1000 mL
-4-21.0 10 mol HCl 1000 mL
1.0 10 M HCl10.0 mL 1 L
Amount of HCl = mol NaOH = 1.0 × 10−4 mol
4. Calculate the molarity of the HCl solution
Sample Problem FIn a titration, 27.4 mL of 0.0154 M Ba(OH)2
is added to a 20.0 mL sample of HCl solution of unknown concentration until the equivalence point is reached. What is the molarity of the acid solution?
Sample Problem F SolutionGiven: volume and concentration of known solution
= 27.4 mL of 0.0154 M Ba(OH)2
Unknown: molarity of acid solution
Solution:
1. balanced neutralization equation chemically equivalent amounts
Ba(OH)2 + 2HCl BaCl2 + 2H2O1 mol 2 mol 1 mol 2 mol
Sample Problem F Solution, continued
2. volume of known basic solution used (mL) amount of base used (mol)
mol Ba(OH)2
1 LmL of Ba(OH)
2 solution
1 L
1000 mLmol Ba(OH)
2
3. mole ratio, moles of base used moles of acid used from unknown solution
2 mol HCl
mol Ba(OH)2
mol of Ba(OH)2 in known solution mol HCl
Sample Problem F Solution, continued
4. volume of unknown, moles of solute in unknown molarity of unknown
amount of solute in unknown solution (mol)
volume of unknown solution (mL)
1000 mL
1 L
molarity of unknown solution
Sample Problem F Solution, continued
1. 1 mol Ba(OH)2 for every 2 mol HCl.
2.
3.
0.0154 mol Ba(OH)2
1 L 24.7 mL of Ba(OH)
2 solution
1 L
1000 mL4.22 10-4mol Ba(OH)
2
2 mol HCl
1 mol Ba(OH)2
4.22 10Ğ4 mol of Ba(OH)2
8.44 10Ğ4 mol HCl
3.80
3.80
7.61-4
-4