Acids and Bases

Question 1

What is the equation for strong acids and strong Bases?

Answer 1

Kw= [H⁺][OH⁻]=10⁻¹⁴ at 298K

Question 2

What is a Brønsted-Lowry Lowry Acid and what is a Brønsted-Lowry Lowry Base?

Answer 2

A Brønsted Lowry acid is a proton donor and a Brønsted Lowry base is a proton acceptor.

Question 3

Why when forming the equation for Kw can you cancel the concentration of the water?

Answer 3

The equilibrium shifts so far to the left that it is very close to 0 and it is then incorporated as a constant within Kw.

Question 4

What is a conjugate base and conjugate acid?

Answer 4

Acid→conjugate base
Base→conjugate acid

Question 5

What is the equation for weak acids and weak bases?

Answer 5

Ka=[H⁺][A⁻]/[HA]

Question 6

What is the definition of pH?

Answer 6

-log[H⁺]

Question 7

How many decimal places for pH?

Answer 7

2!!

Question 8

When calculating the PH of a weak acid from the concentration of the acid what do you need to remember?

Answer 8

[A⁻]=[H⁺]

Question 9

How to calculate pH from pKa?

Answer 9

10^-pKa= pH

Question 10

What is my thought process for a reaction between a strong acid and a strong base?

Answer 10

Find the moles of both the acid and the base
find which one is in excess
plug the moles extra into Kw equation

Question 11

What is the relative strength of the acid if the Ka is high?

Answer 11

Strong

Question 12

Why does water remain neutral at different temperatures even though the pH increases and decreases?

Answer 12

[H+]=[OH-]

Question 13

What is the definition of a weak acid?

Answer 13

Acid partially dissociates

Question 14

What is the definition of a strong acid?

Answer 14

Acid fully dissociates

Question 15

What is a buffer solution?

Answer 15

A solution which keeps pH constant and can withstand small additions of acids and alkalis. It is a mixture of a weak acid and its salt.