AQA A Level Chemistry 3.1.12 - Acids and Bases
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1. Bronsted-Lowry acid Proton donor
2. Bronsted-Lowry base Proton acceptor
3. pH Measure of acidity by measuring concentration of H⁺ ions.
4. Low pH means Acidity
5. High pH means Alkalinity
6. Calculating pH pH = -log [H⁺]
7. Calculating [H⁺] -pH
[H⁺] = 10
8. What does an Transfer of the H⁺ from the acid to the base.
acid/base reaction in-
volve?
9. Strong acid Fully dissociates in water.
10. Weak acid Only very slightly dissociates in water.
11. Ka weak acid dissoci- Ka = [H⁺] [A⁻]
ation constant [HA]
12. The more a weak acid The more H⁺ are formed.
dissociates... The stronger the acid.
The larger the Ka value.
13. Calculating pKa pKa = -log (Ka)
14. Calculating Ka from -pKa
pKa Ka = 10
1/4
Study online at https://quizlet.com/_3hpqpr
1. Bronsted-Lowry acid Proton donor
2. Bronsted-Lowry base Proton acceptor
3. pH Measure of acidity by measuring concentration of H⁺ ions.
4. Low pH means Acidity
5. High pH means Alkalinity
6. Calculating pH pH = -log [H⁺]
7. Calculating [H⁺] -pH
[H⁺] = 10
8. What does an Transfer of the H⁺ from the acid to the base.
acid/base reaction in-
volve?
9. Strong acid Fully dissociates in water.
10. Weak acid Only very slightly dissociates in water.
11. Ka weak acid dissoci- Ka = [H⁺] [A⁻]
ation constant [HA]
12. The more a weak acid The more H⁺ are formed.
dissociates... The stronger the acid.
The larger the Ka value.
13. Calculating pKa pKa = -log (Ka)
14. Calculating Ka from -pKa
pKa Ka = 10
1/4
