Acids and Bases
Buffers
Titrations
Thermo and Electro
Miscellaneous
100
Acid strength decreases in the series HI > HSO4– > HF > HCN. Which of these species is the weakest base?
A) I–
B) SO4 2–
C) F–
D) CN–
E) H2SO4
A) I–
100
Which of the following species could you combine with HF to form a buffer system?
A. NaCl
B. HCl
C. NaF
D. HF₂
C. NaF
100
Calculate the pH of a 40mL .2M HCOOH solution before .1M of NaOH is added and with a ka of 1.8*10^-4??
2.22
100
Calculate the equilibrium constant for the decomposition of water 2H2O (l)
2H2 (g) + O2 (g) at 25°C, given that ΔG°f (H2O(l)) = –237.2 kJ/mol.
3.8 x 10^41
100
If pka=-log(ka), pkb=-log(kb), then pDiddy=?
-log(diddy)
200
Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87.
1.3*10^-3 M
200
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 itself a strong base.
D) Strong acids are very concentrated acids.
E) Strong acids produce solutions with a higher pH than weak acids
B) Strong acids are 100% ionized in water.
200
What is the pH when 30.0 mL of 0.10 M acetic acid (CH₃COOH) is titrated with 45.0 mL of 0.067 M NaOH? Ka=1.8 x 10^-5
10.30
200
Which response includes all of the following processes that are accompanied by a decrease in entropy?
2 SO2(g) + O2(g)
C2H2(g) + 5/2O2(g)
Br2(l)
H2O2(l)
2 SO2(g) + O2(g)
C2H2(g) + 5/2O2(g)
200
Who created the national anthem
Lana Del Rey
(Half points if u say Francis Scott Keys)
300
Which of the following yields an acidic solution when dissolved in water?
A) HNO2 B) LiOH C) KClO2 D) NaCl E) Ca(OH)2
A) HNO2
300
You dissolve the salt NaF in water. What is the pH of the resulting solution?
Basic
300
What is the pH at the midpoint of a solution containing 40 mL of .2M HCOOC and .1M NaOH with a ka of 1.8*10^-4?
3.7
300
What is the value of Gibbs free energy when the equilibrium constant is less than 1?
ΔG < 0
ΔG > 0
ΔG = K
ΔG = 0
Cannot be determined
ΔG > 0
300
Who was in Paris?
The peer leader Georgina
400
Identify the conjugate base of HPO42– in the reaction
HCO3– + HPO42– -> H2CO3 + PO43–
A) H2O B) HCO3 – C) H2CO3 D) PO4 3– E) None of these.
D) PO4 3–
400
What is the OH– ion concentration in a 5.2 x 10–4 M HNO3 solution?
1.9 x 10–11 M
400
What is the pH of a solution containing 40 mL of .2M HCOOH and 90mL of .1M NaOH?
11.9
400
A certain electrochemical cell has for its cell reaction:
Zn + HgO → ZnO + Hg
Which is the half-reaction occurring at the anode?
A) HgO + 2e– → Hg + O2– C) Zn → Zn2+ + 2e–
B) Zn2+ + 2e– → Zn D) ZnO + 2e– → Zn
Zn → Zn2+ + 2e–
400
The following reaction pulls up uninvited and turns the whole lab into O’Block.
Hint: Group 1 + H2O
Na + H2O
500
Halogens bonded to a hydrogen are considered strong acids (HCl, HBr, HI). Except HF, why?
The bond length between H and F is too small to allow the compound to completely dissociate.
500
What makes an acid acidic?
Potential of hydrogen.
500
If 100mL of .30 sodium hydrogen carbonate is mixed thoroughly with 100 mL of .10M sodium hydroxide, and the pka of carbonic acid is 10.3, what is the pH?
10
500
Given the following two half-reactions, determine which overall reaction is spontaneous and calculate its standard cell potential.
Cd2+(aq) + 2 e- → Cd(s) E° = -1.21 V
Sn2+(aq) + 2 e- → Sn(s) E° = -0.14 V
a. Cd2+(aq) + Sn(s) → Cd(s) + Sn2+(aq) = +1.07 V
b. Cd2+(aq) + Sn(s) → Cd(s) + Sn2+(aq) = -1.35 V
c. Cd(s) + Sn2+(aq) → Cd2+(aq) + Sn(s) = +1.07 V
d. Cd(s) + Sn2+(aq) → Cd2+(aq) + Sn(s) = -1.07 V
e. Cd(s) + Sn2+(aq) → Cd2+(aq) + Sn(s) = +1.35 V
Cd(s) + Sn2+(aq) → Cd2+(aq) + Sn(s) = +1.07 V
500
Fav white girl song?
Hint: Song has been playing throughout class time
Hint: Yearning Level 100
The one that got away - Katy Perry (500)
Wildest Dreams - Taylor Swift (250)
Cinnamon Girl - Lana (1000)