Bronsted/Lewis Acids
Lewis Acids are ...
Lewis Bases are ...
Electron receivers
Electrons donors
An acid makes a ...
A base makes a ...
Conjugated base
Conjugated acid
whats the constant of Kw=
1 x 10^-14
Suppose a buffer is composed of 0.65M potassium formate (HCOOK) and 0.80 M formic Acid (HCOOH), pKa = 3.70 for HCOOH. Find the pH of the buffer
3.61
The following reaction occur at 500K. Arrange them in order of increasing tendency to proceed to completion (least--> greatest tendency)
1. 2NOCl <--> 2NO + Cl2. Kp= 1.7 x 10^-2
2. 2SO3 <--> 2SO2 + O2. Kp = 1.3 x 10^-5
3. 2NO2 <--> 2NO + O2. Kp=5.9 x 10^-5
(HINT: Smallest Kp to biggest Kp)
2 < 3 < 1
True or False:
All Bronsted- Lowry Acids/bases are Lewis acids/bases but not all Lewis acids/bases are Bronsted- Lowry acids/bases
TRUE
Identify the conjugate acid of HCO3- in the reaction :
HCO3- + HPO42- <---> H2CO3 + PO43-
H2CO3
The OH- concentration in a 1.0 x 10-3 M Ba(OH)2 solution is ...
0.002M
Find the pH of a solution that has 4.0 mol of CH3NH3Cl and 1.5 mol of CH3NH2. The Kb of CH3NH2 is 4.5 x 10^-4. Assume this is a 1L solution
10.22
Find the concentration of [H^+] in a 0.58M of potassium hydrogen phosphate (KH2PO4) solution, given that, for H2PO4, the first Ka= 6.2 x 10^-8, second Ka= 5.0 x 10^-8 (HINT: Ignore the Ka that is the smallest)
1.89 x 10^-4
Bronsted Acids are....
Bronsted Bases are....
proton donos
proton acceptor
In the reaction HSO4- (aq) + OH- (aq) <---> SO42- (aq) + H2O(l) , the conjugate acid base pairs are ...
HSO4^- and SO4^2- ; and H2O and OH^-
What is the pH of 0.15M solution of NaOH?
pH = 13.2
Calculate the pH of 0.4M of H2SO3, given that Ka1= 5.3 x 10^-3 and Ka2= 9.5 x 10^-6
1.34
In which one of the following solutions will acetic acid have the greatest percent ionization?
a) 0.1 M CH3COOH
b)0.1 M CH3COOH dissolved in 1M HCl
c) 0.1 M CH3COOH plus 0.1M CH3COONa
d) 0.1 M CH3COOH plus 0.2 M CH3COONa
a)
Which of these species will act as a Lewis acid?
a) NH3 b) NH4+ c) H2O d) BF3 e) F-
d)
Write the reaction between acetic acid and water and identify the Acid/ Base with its CB/CA.
CH3COOH + H2O <--> CH3COO^- + H3O^+
A B CB CA
Determine the pH of a KOH solution made by mixing 0.251g KOH with enough water to makes 1.00 x 102 mL of solution
12.65
Calculate the pH of a buffer solution that contains 0.25M benzoic acid (C6H5CO2H) and 0.15M sodium benzoate (C6H5COONa) [Ka = 6.5 x 10-5 for benzoic acid]
3.97
Which one of these statements about strong acids is true?
a) All strong Acids have H atoms bonded to electronegative oxygen atoms
b) Strong acids are 100% ionized in water
c) The conjugate base of a strong acid is itselsf a strong base
d) Strong acids are very concentrated acids
e) Strong acids produce solutions with higher pH than weak acids
b)
Water can act as both an acid and a base which is said to be ...
Amphoteric
If the pH of an acid rain storm is approximately 3, how many times greater is the [H+ ] in the rain than in a cup of coffee having a pH of 5.0?
100 times
The pKa values for carbonic acid are 1.81 and 5.98. Write the balance chemical equations corresponding to the pKa's
1. H2CO3<--> HCO3^- + H^+.
2. HCO3 <--> CO3^2- + H^+
Consider the weak acid CH3COOH (acetic acid). If a 0.048 M CH3COOH solution is 5.2% ionized determine the [H3O^+] concentration at equilibrium
2.5 x 20^-3M