acids and bases Flashcards
Name the first strongest Acid
what is its formula
what is its conjugate base formula
ka?
Perchloric acid (aqueous Hydrogen perchlorate)
HCLO4 (aq)
CLO4^- (aq)
very large
Name the second strongest Acid
what is its formula
what is its conjugate base formula
ka?
Hydroiodic acid ( aqueous hydrogen iodide)
HI (aq)
I^- (aq)
very large
Name the third strongest Acid
what is its formula
what is its conjugate base formula
ka?
hydrobromic acid (aqueous hydrogen bromide)
HBr (aq)
Br^- (aq)
very large
Name the fourth strongest Acid
what is its formula
what is its conjugate base formula
ka?
hydrochloric acid (aq hydrogen chloride)
HCl(aq)
Cl^-
very large
Name the fifth strongest Acid
what is its formula
what is its conjugate base formula
ka?
sulfuric acid (aqueous hydrogen sulfate)
H2SO4 (aq)
HSO4 ^-(aq)
very large
Name the sixth strongest Acid
what is its formula
what is its congugate base
ka?
Nitric acid (aqueous hydrogen nitrate)
HNO3 (aq)
NO3^- (aq)
very large
What are the physical properties of Acids
- Taste sour
- Acidic
- Have a PH less than 7
4.(H30+)>(OH-)
Ex. citrus fruits such as oranges
What are the Physical Properties of Bases
- Taste bitter
2.. Feel slippery
3.Basic - Have a PH greater than 7
- (H30+)<(OH-)
Ex. Soap
Explain the Reaction of Acids
- React with certain metals to produce hydrogen gas
- React with carbonates and bicarbonates to produce carbon dioxide gas
What is acid base neutralization
acid-base neutralization is a chemical reaction in which an acid reacts with a base to form water and a salt. During this process, the acid’s hydrogen ions (H⁺) combine with the base’s hydroxide ions (OH⁻), neutralizing each other. For example:
HCl + NaOH →NaCl + H2O
This reaction typically results in a pH closer to 7, which is neutral.
(H3O+)=(OH-)
What is the Arrhenius acid-base theory
- Arrhenius acid is any substance that produces H+ or (H3O+) in water
- Arrhenius base is any substance that produces OH- in water
What is the Brønsted-Lowry acid-base theory.
- Acids are proton (H+) donors.
- Bases are proton (H+) acceptors.
- acid + base ⇌ conjugate base + conjugate acid
what is Autoionization of water
what is the formula
- A proton is transferred from one water molecule to another to produce a hydronium ion (H₃O⁺) and a hydroxide ion (OH⁻).
- H2O(l) + H2O(l) → H3O+(aq) + OH-(aq)
acid base congugate base congugate acid
What is the formula for the Ion Product of water
what does KW represent
- Kw = [H3O+][OH-]
- The ion-product constant (Kw) is the product of the molar
concentrations of H3O+ and OH- ions at a particular
temperature.
What is the concentration of OH- ions in a HCl solution
whose hydronium ion concentration is 1.3 M?
Kw = [H3O+][OH-] = 1.0 x 10-14 @ 25^.C
[H3O+] = 1.3 M
[OH-] = Kw/[H3O +]
=1 x 10 x 10 ^ -14/1.3
= 7.7 x 10-15 M
What is Ph
what are the formulas to calculate it
- The measure of acidity
- pH = -log [H3O1+]
- pH + pOH = 14.00
- pH = pKa + log [A1-] / [HA]
what is percent acid dissociation
Percent acid dissociation formula
- Percent acid dissociation refers to the percentage of acid molecules that dissociate (break apart) into ions in a solution compared to the total amount of acid present. It is a measure of the strength of the acid, indicating how much of it has ionized.
- % dissociation = ionized acid concentration at equilibrium x initial concentration of acid x 100%
What are acid- base indicators and how do they work?
An acid-base indicator is a weak acid or weak base that changes colour in response to changes in hydrogen (H+) or hydroxide (OH-) ion concentrations. These indicators are commonly used in titrations to determine the endpoint of an acid-base reaction, as well as to measure pH levels
what are electrolytes
- An electrolyte is a substance that conducts electricity when dissolved in water or melted, due to the movement of ions. Examples include salts like sodium chloride (NaCl) and potassium chloride (KCl).
rong electrolytes vs weak electrolytes
- Strong Electrolyte – 100% dissociation
NaCl (s) Na+ (aq) + Cl- (aq)
- Weak Electrolyte – not completely dissociated
CH3COOH(aq) CH3COO- (aq) + H+ (aq)
Strong acids vs weak acids
- Strong Acids are strong electrolytes
HCl (aq) + H2O (l) → H3O+ (aq) + Cl- (aq)
- Weak Acids are weak electrolytes
NaOH (s) ⇌ Na+ (aq) + OH- (aq)
Weak bases?
Weak Bases are weak electrolytes
F- (aq) + H2O (l) ⇌ OH- (aq) + HF (aq)
Conjugate acid-base pairs?
- The conjugate base of a strong acid has no measurable
strength (a.k.a. it’s extremely weak). - The OH- ion is the strongest base that can exist in aqueous
solution.
Weak Acids (HA) and Acid Ionization Constants
HA (aq) + H2O (l) → H3O+ (aq) + A- (aq)
Ka = [H3O+][A-]/[HA]
Ka is the acid ionization constant
the larger the Ka value the stronger the acid
What is a buffer solution
- A weak acid and a salt of its conjugate base, or
- A weak base and a salt of its conjugate acid.
- A buffer solution has the ability to resist changes in pH upon
the addition of small amounts of either acid or base.
what are the 2 types of buffers
- An acidic buffer solution has a pH less than 7.
A solution of a mixture of a weak acid and a salt of its
conjugate base.
CH3COOH + NaCH3COO
(weak acid) + (conjugate base salt)
- An basic buffer solution has a pH greater than 7.
A solution of a mixture of a weak base and a salt of its
conjugate acid.
NH3 + NH4Cl
(weak base) + (conjugate acid salt)
how do buffers work?
- If more acid (H3O+) is added to this solution, the equilibrium
will shift to the left, absorbing the excess acid, so the
[H3O+] (and pH) remains unchanged. - If acid (H3O+) is removed (by adding OH-) then the
equilibrium will shift to the right, releasing H3O+ so as to
keep the pH constant.
The pH of rainwater collected in a certain region of Nova
Scotia on a particular day was 4.82. What is the H3O+ ion
concentration of the rainwater?
pH = -log [H3O+]
[H3O+] = 10^-pH = 10^-4.82
= 1.5 x 10^-5 M
The OH- ion concentration of a blood sample is 2.5 x 10-7 M.
What is the pH of the blood?
pH + pOH = 14.00
pOH = -log [OH-]
-log (2.5 x 10^-7) = 6.60
pH = 14.00 – pOH = 14.00 – 6.60 = 7.40
What is the pH of a 2 x 10-3 M HNO3 solution?
Start 0.002 M 0.0. 0.0
HNO3 (aq) + H2O (l) = H3O+ (aq) + NO3- (aq)
End 0.0 0. 0020.002 M
pH = -log [H3O+] = -log(0.002) = 2.7
What is the pH of a 1.8 x 10-2 M Ba(OH)2 solution?
Ba(OH)2 is a strong base – 100% dissociation.
Ba(OH)2 (s) Ba2+ (aq) + 2OH- (aq)
Start 0.018 M 0.0 M 0.0 M
End 0.0 M 0.018 M 0.036 M
pH = 14.00 – pOH = 14.00 + log(0.036) = 12.6
