Acid and Bases Chemistry

Question 1

What are the three Acids and bases definition and define them

Answer 1

1. -Arrhenius: an acids releases a proton and a base releases and OH-
2. -Brostedlowry: An acid donates a proton and a base receive protons
3. • Lewis: Acids accept electrons and Bases donare electrons

Question 2

What are three basic rules to identify acid?

Answer 2

1. Hydrogren ions bonded with electophilic non-metals
2. The Hydrogen is usaly positive

Question 3

What are three basic rules to identify a base ?

Answer 3

1. They usually have a hydroxide ions ( OH-)
2. or the hydrogen is attached to a metal
3. hydrogen can have a negative charge

Question 4

How do you create a conjugate base and an conjugate acids

Answer 4

1. -conjugate bases and acids are usually formed in a neutralization equations of acids and basis and are the product of the balance equations of these acids

Question 5

How do you calculate pH and pOH?

Answer 5

1. -pH is the -log of [HO3+]
2. -pOH is the -log [OH +]
3. pH + pOH = 14

Question 6

How to identify a strong acid?

Answer 6

These are ions that separates completely in water, and form strong electrolytes

Question 7

How to identify weak acids?

Answer 7

These partially ionize and create weak electrolytes

Question 8

When dealing with oxy-acids ( acids with oxygen added to it) how do you know whihc one is stronger? What is the exception of oxy-acids?

Answer 8

1. The molecules with most of the oxygen will usually be the strongest
2. HCl- is the exception HCL is stronger than HCLO because the original molecule did not have an O

Question 9

How do you determine a strong base?

Answer 9

These ionize 100% in water and form strong electrolytes

Question 10

How to identify weak acids?

Answer 10

insoluble and do not ionize 100% in water

Question 11

What is a rule of thumb with oxygen and oxygen that can help you remember the strength of a base or acid?

Answer 11

1. the less hydrogen present the more basic the substance
2. the more Oxygen the more acidic the weak acid

Question 12

When reacting with water what type of base does a strong base produce?

Answer 12

weaker bases

Question 13

Analyzing the pH scale

Answer 13

pH log mean that where-ever your start by at the next number up would be increased by X10 -So if your pH is at 8 then it would take you 10X fold the [OH-] to get to a pH of 9 then 10X 10 ( which 100X) of the [OH-] to get to a pH of 10 on the pH scale. that is why we calculate these pH in logs because to get to one pH to another it takes alot of the concentration of either H+ or OH-

Question 14

Define the meaning of pKa and pKb and their relations to the power of an acid or a base.

Answer 14

1. pka or pKb: tells you the pH or the pOH at which you have 50% of both acids and bases to buffer a solution
2. smaller pKa: equals a good acid because a good acid disassociates quickly (technically they don’t even have one but we use it arbitrary)
3. smaller pKb= a good base because a good base disassociates quickly

Question 15

what are amphoteric species?

Answer 15

1. Species that can react with themselves and are use in chemical reactions to drive things such as alcohol and SN1 and SN2 reactions

Question 16

What is the Ka and Kb?

Answer 16

1. This is the rate of making either the acid ( ka) or the base (kb)
2. These properties can be used to find the pH of a solution
3. The higher these numbers the stronger your acid or your base

Question 17

Explain the concept of the hydrolysis of salts

Answer 17

1. It’s when a neutralization reactions went through, and the salt is able to react with water thinking about buffers, you can only have two types of neutralization reations.
   
   1. SA + WB - Acetic salt because the srong acid wins
   2. SB + WA- gives an basic salt because the strong base wins.
2. The salt of the weak molecules are the only ones that can react i.e hydrolyze with water.