Chemistry
In order for a solution to be acidic: A) ph=pOH B) [H3O+]>[OH-] C) [H3O+]<[OH-] D) [H3O+]=[OH-] E) None of these
B) [H3O+]>[OH-]
What molarity of pyridine, C5H5N, is required to produce an aqueous solution with pH= 9.35? (Kb= 1.7 x 10-9) A) 1.3 x 10 4 B) 2.2 x 10-5 C) 2.97 D) 0.29 E) 3.6 x 10-5
D) 0.29
A 4.08 g sample of phenol, C6H5OH, is dissolved in 0.250 L of water at 25 C, and it's pH is found to be 5.38. What is the Ka of phenol? A) 2.5 x 10-10 B) 2.5 x 10-9 C) 1.8 x 10-5 D) 1.0 x 10-10 E) 5.8 x 10-5
D) 1.0 x 10-10
What is the concentration of the hydronium ions in a neutral solution? A) 1.0 x 10-14 M B) 0.0 M C) < 1.0 x 10-7 M D) 1.0 x 10-7 M E) > 1.0 x 10-7 M
D) 1.0 x 10-7 M
Calculate the concentration of H3O+ in a solution that contains 5.5 x 10-5 M OH- at 25 C. Identify the solution as acidic, basic, or neutral. A) 1.8 x 10-10 M, acidic B) 5.5 x 10-10 M, neutral C) 9.2 x 10-1 M, acidic D) 1.8 x 10-10 M, basic E) 9.2 x 10-1 M, basic
D) 1.8 x 10-10 M, basic
What is the pH of a solution prepared by dissolving 0.025 mol Ba(OH)2 in water to give 455 mL of solution? A) 12.40 B) 1.26 C) 1.60 D) 13.04 E) 12.74
D) 13.04
Determine the pH of a 0.00598 M HCIO4 solution A) 11.777 B) 3.558 C) 7.566 D) 2.223 E) 6.434
D) 2.223
Which of the following is TRUE? A) An neutral solution does not contain any H30+ or OH- B) A neutral solution contains [H2O] = [H3O+] C) A basic solution does not contain H3O+ D) An acidic solution has [H3O+]> [OH-] E) None of these above are true
D) An acidic solution has [H3O+]>[OH-]
Given the following Ka values, HC2H3O2. 1.8 x 10-5 HCN 6.2 x 10-10 HOCl. 2.9 x 10-8 HClO3. 5.0 x 10 2 HF. 6.6 x 10-4 Which of the following is the weakest base? A) OCl- B) C2H3O2- C) F- D) ClO3- E) CN-
D) ClO3-
True or false: The ion product constant for water (Kw) is best stated as Kw=[H2O][H+]
False
True or false: The pH of a 0.0001 M NaOH solution is 4
False
True or false: Water always acts as an acid in reactions
False
Which of the following bases is the STRONGEST? The base is followed by its Kb? A) CH3NH2, 4.4 x 10-4 B) (CH3CH2)2NH, 8.6 x 10-4 C) C6H5NH2, 4.0 x 10-10 D) C5H5N, 1.7 x 10-9 E) NH3, 1.76 x 10-5
B) (CH3CH2)2NH, 8.6 x 10-4
The conjugate base of NH3 is...... A) -NH3 B) -NH2 C) +NH4 D) -NH4 E) +NH2
B) -NH2
The pH of acid rain may be as low as 2.80. What is the [H3O+] in such acidic rain? A) 6.3 x 10-12 B) 1.6 x 10-3 C) 9.7 x 10-2 D) 630 E) 1.6
B) 1.6 x 10-3
The pH of a 0.10 M solution of hydrazoic acid, HN3, is 2.86. Calculate the Ka value for hydrazoic acid A) 1.4 x 10-4 B) 1.9 x 10-5 C) 2.6 x 10-8 D) 1.9 x 10-6 E) 1.4 x 10-3
B) 1.9 x 10-5
Calculate the pH of a 0.0015 M HCl solution A) 3.84 B) 2.82 C) 1.5 D) 11.17 E) 1.5 x 10-3
B) 2.82
Which of the following is the strongest acid? A) H2S B) HCl C) PH3 D) CH4 E) SiH4
B) HCl
Which is the weakest acid? A) HOClO3 B) HOCl C) HOClO2 D) HOClO
B) HOCl
Which of the following species is not amphiprotic? A) H2O B) SO4-2 C) HC2O4- D) HCO3- E) H2PO4-
B) SO4-2
True or false: The conjugate acid of OH- is H3O+
False
The pH of a 0.30 M solution of HCN is 5.20. Calculate the. Ka value for HCN A) 1.3 x 10-10 B) 8.4 x 10-18 C) 2.1 x 10-5 D) 6.3 x 10-6 E) 4.8 x 10-2
A) 1.3 x 10-10
Calculate the pOH of a 3.5 x 10-2 M NaOH solution A) 1.46 B) 0.46 C) 11.46 D) 12.54 E) 2.46
A) 1.46
Calculate the pH of 0.50 M NaCN. (Ka (HCN) = 6.2 x 10-10) A) 11.45 B) 2.55 C) 9.51 D) 9.21 E) 4.49
A) 11.45
Which species act as bases in the following reaction? H2SO4 + HNO3 <-> H2NO3 + HSO4 A) 2 and 4 B) 1 and 3 C) 1 and 2 D) 2 and 3 E) 3 and 4
A) 2 and 4
What is the [OH-] in an aqueous solution of orange juice with [H3O+] = 3.4 x 10-4 M? A) 2.9 x 10-11 B) 1.00 x 10-14 C) 3.47 D) 10.53 E) 3.4 x 10-4
A) 2.9 x 10-11
The pKb for aniline is 9.13. What is the value of the base ionization constant fro aniline? A) 7.4 x 10-10 B) 9.13 C) 1.35 x 10-5 D) 4.87 E) 1.3 x 10-9
A) 7.4 x 10-10
Arrange the following carboxylic acids in the order in which you would expect their Ka values to increase A) CH3CH2CH2COOH, B) CH3CH2ClCOOH, C) ClCH2CH2CH2COOH, D) CH3CHClCHClCOOH A) A > C > B > D B) D > B > C > A C) A > B > C > D D) C > B > D > A E) D > C > A > B
A) A > C > B > D
For the following reaction, define each of the species as acid, base, conjugate acid, and conjugate base H2SO4 + H2O -> H3O+ + HSO4- A) Acid + Base -> Conjugate Acid + Conjugate Base B) Base + Acid -> Conjugate Base + Conjugate Acid C) Acid + Base -> Conjugate Base + Conjugate Acid D) Base + Acid -> Conjugate Acid + Conjugate Base E) These aren't acids and bases
A) Acid + Base -> Conjugate Acid + Conjugate Base
Determine the pH of 0.35 M HOCl. The Ka of HOCl is 2.9 x 10-8 A) 4.00 B) 1.00 x 10-4 C) 3.12 D) 7.53 E) 8.00
As 4.00
True or false: In the reaction BF3 + F- -> BF4- BF3 acts as a Bronsted-Lowry acid
False
What molarity of a CH3COONa solution has a pH = 9.35? (Ka (CH3COOH) = 1.8 x 10-5) A) 0.75 B) 0.90 C) 2.68 D) 0.37 E) 1.10
Bj 0.90
Calculate the pH of a 0.25 M ethylammonium chloride (C2H5NH3Cl) solution (Kb (C2H5NH2) = 4.3 x 10-4) A) 11.24 B) 4.72 C) 5.62 D) 8.38 E) 2.76
C) 5.62
Which is the strongest base? A) Cl- B) I- C) F- D) Br- E) none of these are bases
C) F-
What is the strongest acid? A) HOBr B) HOI C) HOCI
C) HOCI
The Bronsted-Lowry definition of a base is: A) produces H+ in solution B) produces OH- in solution C) a proton acceptor D) a proton donor E) none of these
C) a proton acceptor
Identify the acid and base on each side of the following equation HSO3- + HPO4 2 <-> SO3-2 + H2PO4- A) base + acid <-> acid + base B) base + acid <-> base + acid C) acid + base <-> base + acid D) acid + base <-> acid + base E) not an acid-base reaction
C) acid + base <-> base + acid
"Milk of magnesia" antacid has a pH of 10.25. What is the [OH-] in this solution? A) 5.6 x 10-11 B) 1.8 C) 3.75 D) 1.8 x 10 10 E) 1.I x 10-4
E) 1.1 x 10-4
A sample of milk is found to have a pH of 6.25. What is the [OH-] in this milk? A) 7.75 B) 5.6 x 10-7 C) 1.8 x 10 6 D) 1.00 x 10-14 E) 1.6
E) 1.6
Determine the Kb for CN- at 25 C. The Ka for HCN is 4.9 x 10-10 A) 1.4 x 10-5 B) 4.9 x 10-14 C) 2.3 x 10-9 D) 3.7 x 10-7 E) 2.0 x 10-5
E) 2.0 x 10-5
What is the [H3O+] in a 0.020 M Ca(OH)2? A) 12.60 B) 1.0 x 10-7 C) 5 x 10-13 D) 0 E)2.5 x 10-13
E) 2.5 x 10-13
A pH meter reads 4.48. What is the [H3O+] in the solution? A) 7.00 B) 9.52 C) 3.0 x 10-10 D) 3.0 x 10 4 E) 3.3 x 10-5
E) 3.3 x 10-5
Which one of the following pairs of species are conjugate acid base pairs? A) H3PO4, PO4-3 B) HCl, HBr C) H3O+, OH+ D) HI, NaOH E) H2SO4, HSO4-
E) H2SO4, HSO4-
What is the conjugate base of H2PO4-? A) H3O+ B) OH- C) H3PO4 D) PO4-3 E) HPO4-2
E) HPO4-2
Which one of the following salts will have a water solution with a pH less than 7? A) KCN B) K2CO3 C) NaC2H3O2 D) NaBr E) NH4Cl
E) NH4Cl
The Ka of nicotinic acid is 1.4 x 10-5. What is the % ionization of nicotinic acid in a 2.30 M solution? A) 1.52 B) 100 C) 0.250 D) 0 E) 0.570
Ej 0.570
True or false: A neutral solution does not contain any H+ or OH-
False
True or false: A weak acid is a dilute acid that is not very powerful
False
True or false: According to Brønsted-Lowry acid-base theory, an acid is any substance that can donate an electron pair
False
True or false: Acids have a bitter taste
False
True or false: An Arrhenius base is a proton acceptor
False
True or false: An acid containing the COOH group is called a carbo-oxy acid
False
True or false: H+ is called the hydronium ion
False
True or false: H2SO3 and H2SO4 are considered conjugate acid-base pair
False
True or false: In any water solution, [H3O+][OH-] = 1x10-7
False
The conjugate acid of HPO4 2- is
H2PO4-
True or false: A 1.0 M [H3O+] solution of a strong acid would have a pH equal to zero
True
True or false: A Brønsted-Lowry acid is a proton donor
True
True or false: A Lewis acid is an electron-pair acceptor, and a Lewis base is an electron-pair donor
True
True or false: A conjugate acid-base pair are two substances related to each other by the transfer of a proton
True
True or false: A solution of pH 2 contains ten times more H3O+ than a solution of pH 3
True
True or false: A solution that has a pH of 10 would also have a pOH of 4
True
True or false: A solution with a pH of 10.00 is basic
True
True or false: A strong acid is one that completely dissociates into ions in solution
True
True or false: A strong acid must also be a strong electrolyte
True
True or false: Acids produce H+ ions in solution
True
True or false: An acid-base reaction is favored in the direction from the acid with the larger Ka toward the acid with the smaller Ka
True
True or false: Arrhenius acid-base theory is limited to applications involving only aqueous solutions
True
True or false: Bases feel slippery
True
True or false: Bases have a bitter taste
True
True or false: NH4+ and NH3 are considered a conjugate acid-base conjugate pair
True
True or false: The common name of CH3COOH is acetic acid
True
True or false: The conjugate base of HF is F-
True
True or false: The conjugate base to HSO4- is SO4 2-
True
True or false: The pH of 0.001 M HCl is 3.0
True
