Chemistry

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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


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