Match the acid and base to it's definition
| Draggable item | arrow_right_alt | Corresponding Item |
|---|---|---|
Arrhenius Base | arrow_right_alt | proton donor |
Arrhenius Acid | arrow_right_alt | proton acceptor |
Lewis Base | arrow_right_alt | forms H+ in water |
Bronsted Lowry Base | arrow_right_alt | forms OH- in water |
Bronsted Lowry Acid | arrow_right_alt | electron pair acceptor |
Lewis Acid | arrow_right_alt | electron pair donor |
Below is a Bronsted acid-base reaction.
HF is a Bronsted Lowry acid which means it is a proton donor.
PO4-3 is a Bronsted Lowry base which means it is a proton acceptor.
The reactants are given to you. What do you predict that the products will be? Remember: a proton is also known as H+
Look at the equation below.
On the equation below, fill in the blank on the red lines on which reactant you think is the bronsted lowry acid and which reactant you think is the bronsted lowry base.
What is the conjugate acid of H2O?
What is the conjugate base of H2O?
Why can water be considered a conjugate acid or conjugate base?
For the Equation:
HClO4(aq) + H2O(l) ⇄ H3O+(aq) + ClO4–(aq)
What is the Acid?
For the equation
H2SO3(aq) + H2O(l) ⇄ H3O+(aq) + HSO3–(aq)
What is the base?
For the equation
HC2H3O2(aq) + H2O(l) ⇄ H3O+(aq) + C2H3O2–(aq)
What is the Acid conjugate base pair?
For the equation
H2S(g) + H2O(l) ⇄ H3O+(aq) + HS–(aq)
What is the Base Conjugate Acid pair?
For the Below equations underline:
Acids in RED
Bases in Blue
Conjugate acids in ORANGE
Conjugate bases in GREEN
Look at the equation below.
On the equation below, fill in the blank on the blue lines on which product you think is the conjugate acid and which product you think is the conjugate base.
Solution A: pH= 3.3
Solution B: pOH= 11.8
Solution C: pH= 5.5
Solution D: pOH= 10
Which solution is the most acidic? Explain your answer.
Organize the following solutions with most acidic at the top and most basic at the bottom.
Solution A: pH= 3.3
Solution B: pOH= 11.8
Solution C: pH= 5.5
Solution D: pOH= 10
C
D
A
B