General Chemistry - Acids and Bases
17 important questions on General Chemistry - Acids and Bases
Bronsted-Lowry Acids/Bases
Base - Accepts a H+
**Always occur in conjugate acid-base pairs
Lewis Acids/Bases
Base - electron pair donor
Arrhenius nomenclature - anions with the suffix ide
Ex: F = fluoride ==> hydrofluoric acid
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Arrhenius nomenclature - oxyanions -> oxyacids
oxyanions with the suffix ate, gain the suffix ic acid
Kw dissociation constant of water
Kw = [H+][OH-] = 10^-14
rearrange to : pH + pOH = 14
Estimating pH/ pKa from a alue with a power of 10, if [H+] = 1x10^x, pH =?
Estimating pH/ pKa from a value that is not base 10
-log[H+] = m - log(n)
We can estimate that log(n) is between 0 and 1, the larger the value of n, the closer log(n) is to 1, so you can estimate based on that value where it will fall
What determines the strength of an acid/base?
When an acid/ base is strong, its conjugate is____
This occurs in proportion, the stronger the acid, the weaker its conjugate is
When can we ignore the common ion effect in our pH calculations?
List of 4 common strong acids
HNO3 - Nitric acid
H2SO4 - Sulfuric acid
HCl - Hydrochloric acid
List of 4 common strong bases
KOH - potassium hydroxide
Ca(OH)2 - calcium hydroxide
Soluble hydroxides of group IA and IIA metals
Acid dissociation constant
Ka = [H3O+][A] / [HA]
Weaker the acid, smaller the Ka
**pure liquids, including water, are not included**
Base dissociation constant
Kb = [B+][OH-] / [BOH]
Determining Ka from Kb (and vice versa)
** shows inverse proportionality of strength af acids/bases and their conjugates
4 combinations of strong/ weak acids/ bases and their products
- Strong Acid/ Strong Base
- Yields a salt and water, conjugate acids/ bases are inert. pH =7
2. Strong Acid/ Weak Base
- Yields a salt with no water. anion of strong acid is inert, cation of weak base is not inert, contributes to pH making solution slightly acidic
3. Weak Acid/ Strong Base
- cation of strong base is inert, anion of weak acid is not inert, contributes to pH making solution slightl alkaline
4. Weak acid/ weak base
- pH depends on relative strength of reactants
- If Ka is larger than Kb, solution is acidic and vice versa
- yields salt, no water
Titration of a polyprotic acid/ base
* 1/2 to 1st eq. pt: pH = pKa1
*1st eq. pt, all of original base is consumed
*1/2 to 2nd eq. pt: pH = pKa2
*2nd eq. pt, only the 2nd acid remains
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