Chemistry

Question 1

Strong acids List

Answer 1

HCl (aq), HBr (aq), HI (aq) ((Monoprotic acid)​
H2SO4 (Diprotic acid)​
HNO3 ​
HClO4 (perchloric acid)​
HClO3 (chloric acid)​

Question 2

Strong bases list

Answer 2

all group 1 & 2 metal hydroxides except Mg(OH)2) ​
NaOH ​
KOH ​
Ca(OH)2 ​
Ba(OH)2

Question 3

Moderately strong acid

Answer 3

H3PO4 (Triprotic acid)​

Question 4

Weak Acids List

Answer 4

Usually derived from “Carbon” Acids: CH3COOH Acetic Acid (HAc), CH2O2 formic acid, acetylsalicylic acid (aspirin), protonated bases (drugs)),​ H2CO3

Question 5

Weak Bases List

Answer 5

NH3​

transition metals form weak bases such as Ni(OH)2, Fe(OH)2, Fe(OH)3, Cu(OH)2. Mg(OH)2 ​

Question 6

Arrhenius Definition of Acids/Bases

Answer 6

Acid: Any substance that when put in wate will increase the hydronium ion (H3O+) concentration.

Base: Any substance that when put in water will increase the hydoxide ion (OH-) concentration.

Question 7

Bronsted-Lowry Acid Base Theory

Answer 7

Acid: Any compound that can donate a proton in a proton transfe reaction.
Base: Any compound that can accept a proton in a proton transfer reaction.

Question 8

Lewis Acid Base Theory

Answer 8

Acid: An elelectron pair acceptor (usually metals)
Base: An electron pair donor

Question 9

Avogadro’s Number

Answer 9

6.022x10^23 (# of particles in a mole)

Question 10

Molar Mass

Answer 10

(Grams of a substance/molar mass) = moles of a substance

Question 11

Molarity (M)

Answer 11

Molarity = (Moles of a solute)/(Liters of a solution)

Question 12

Weak acids have a Ka ___ 1

Answer 12

Ka < 1

Question 13

Strong acids have a Ka ___ 1

Answer 13

Ka > 1

Question 14

Bases almost always have a ______ charge than the acid

Answer 14

more negative/ lower

Question 15

What dictates the movement of acid/base drugs across the membrane?

Answer 15

Charge. pH of a solution and the pK of a drug dictates charge. Only uncharged molecules go through the membrane easily.

Question 16

Ka is _____ with a stronger acid and pKa is _____.

Answer 16

Ka is higher, pKa is lower. Means there is more H+ dissociation and that more acid would be required to put the proton (H+) back onto the conjugate base.

Question 17

Ka is _____ with a weaker acid and pKa is _____.

Answer 17

Ka is lower, pKa is higher. Means there is less H+ dissociation and that less acid would be required to put the proton (H+) back onto the conjugate base.

Question 18

Definitions of pKa.

Answer 18

The pKa is the pH at which both the acid (HA or HB+) and the conjugate (A- or B) base are maintained in equal amounts.

10^pH-pK = [A-]/[HA] = 1/1

10^pH-pK = [B]/[HB+] = 1/1

(above is the Henderson-Hasselbach Equation ​ )

pKa is a measure of the hydrogen ion concentration required to put a proton back on the conjugate base of the acid.

Question 19

What is a buffer?

Answer 19

A buffer is essentially a weak base that acts as a protonated acid by adding a weak acid.

Buffers work to compensate when hydrogen ion is added or removed to a solution that was in equilibrium.

They are designed to maintain constant pH by preventing changes in the [H+] by absorbing or providing extra [H+]

Buffers are made from weak acids and their salts.

Question 20

Is pure water buffered?

Answer 20

Pure water is not buffered .
Water is an extremely weak acid and not highly ionized. Any change in the [H+] or [OH-] will cause a change in the pH of the solution.

Question 21

What is a neutralization reaction?

Answer 21

The reaction of a bonsted acid and a bronsted base can yield water and a salt. 1 OH- from the base will react with 1 acidic proton (H+) from the acid.