4- Acids and bases

Question 1

What happens to an acid when added to water?

Answer 1

Acids have the ability to produce H+ ions when added to water

(The strength of an acid is measured by how many of these ions it produces)

Question 2

What happens to a base when added to water?

Answer 2

bases produce OH- ions when added to water

Question 3

5 acids in everyday life

Answer 3

HCl: Hydrochloric acid​
H2CO3: Carbonic acid​
CH3COOH: Acetic acid/Acetate​
Lactic acid​
Citric acid

Question 4

3 bases in everyday life

Answer 4

Sodium bicarbonate (NaHCO3)​
Aluminium hydroxide (Al(OH)3) ​
Magnesium hydroxide (Mg(OH)2)

Question 5

what is the Arrhenius Acid-Base Theory?

Answer 5

acids have the following properties:

Produces H+ ion in water​
Are electrolytes, because they produce hydrogen ions (H+ = protons) in water​
Have a sour taste and turn litmus indicator paper red​
HCl (aq) → H+ (aq) + Cl- (aq)

Question 6

bases according to arrhenius acid-base theory

Answer 6

bases have the following properties:

Produce hydroxide ions (OH−) in water​
Are electrolytes, because they produce hydroxide ions (OH−) in water​
Taste bitter or chalky​
Feel soapy and slippery, turn litmus indicator paper blue
KOH (aq) → K+ (aq) + OH- (aq)

Question 7

What is an acid?

Answer 7

an acid is a substance that donates H+

Question 8

what is a base?

Answer 8

A base is a substance that accepts H+

Question 9

equilibrium of hydrogen ion transfer

Answer 9

HF (aq) + H2O (l) ⇋ H3O+ (aq) + F- (aq)

only strong acids or strong bases go to completion

Question 10

What is a conjugate acid-base pair?

Answer 10

Conjugate acid-base pair is when an acid and a base that differ from each other through the loss or gain of a proton (H+).

Question 11

strength of acid and conjugate base rule?

Answer 11

The stronger the acid the weaker the conjugate base​

The weaker the acid the stronger the conjugate base​

Question 12

strength of base and conjugate acid rule?

Answer 12

The stronger the base the weaker the conjugate acid​

The weaker the base the stronger the conjugate acid

Question 13

strong base/acid lies far to the left or right of an equation?

Answer 13

right

Question 14

what is a neutralisation reaction?

Answer 14

the chemical reaction between an acid and a hydroxide base in which salt and water are the products.

Question 15

The salt formed in a neutralisation reaction is the combination of…?

Answer 15

..the anion (e.g. Cl-) from the acid and the cation (e.g. Na+) from the base​.

Acid + Base → Salt + Water​

HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) ​

Question 16

equation for solutions

Answer 16

Acidic solution: [H3O+] > [OH–]​
Basic solution: [H3O+] < [OH–]​
Neutral solution: [H3O+] = [OH–]

Question 17

the levels of H3O+ and OH- determine if a solution is more acidic or alkaline

Answer 17

The more H3O+ present the more acidic the solution​ — Many of H+ available to donate​
The less H3O+ present the more alkaline the solution​ — Not many of H+ available to donate​
The less OH- present the more acidic the solution​ — Not many OH- available to accept H+​
The more OH- present the more alkaline the solution​ — Many OH- available to accept H+

Question 18

What is the range of a pH test?

Answer 18

0-14

7 = neutral
7> =acidic
7< = alkaline (basic)

Question 19

what is a buffer?

Answer 19

A buffer is made up of a weak acid and its conjugate base

When there is a buffer in a solution, the pH is maintained.
This means that the pH does not change when acids or bases are added.

Question 20

normal blood pH?

Answer 20

7.35-7.45​

Question 21

what is acidosis?

Answer 21

a lowering of the pH of the blood

H2CO3 is a weak acid that will release a small amount of H+ into the blood, which increases the amount of H3O+ in the blood​.

Question 22

what is alkalosis?

Answer 22

A raising of the pH of the blood

A lowering of the CO2 level due to hyperventilation leads to a high blood pH

Question 23

what does pH mean?

Answer 23

potential of hydrogen

Question 24

2 blood buffers?

Answer 24

bicarbonate and phosphate buffers

Question 25

what are electrolytes?

Answer 25

Electrolytes are compounds that are able to conduct electricity when in aqueous solutions.

acids, bases and salts can all form electrolytes

Question 26

how do buffers work?

Answer 26

buffers neutralise H3O+ or OH− from foods and cellular processes to maintain pH.