A a solution of sodium hydrogen sulfate in water would be basic a a solution of sodium hydrogen sulfate in water would be basic


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A) A solution of sodium hydrogen sulfate in water would be basic.

  • A) A solution of sodium hydrogen sulfate in water would be basic.

  • B) A solution of sulfuric acid and sodium hydrogen sulfate in water would be a buffer.

  • C) A solution of sodium hydrogen sulfate and sodium sulfate in water would be a buffer.

  • D) All of the above.



A) 1/10.

  • A) 1/10.

  • B) 10/1.

  • C) ½.

  • D) 2/1.



A) Hydrochloric acid titrated with barium hydroxide.

  • A) Hydrochloric acid titrated with barium hydroxide.

  • B) Sodium nitrite titrated with hydrochloric acid.

  • C) Ammonium chloride titrated with sodium hydroxide.

  • D) Nitric acid titrated with sodium hydroxide.



A) Tap water



A) basic nitrate ions react with the added acid forming water.

  • A) basic nitrate ions react with the added acid forming water.

  • B) silver iodide precipitates out of the solution leaving the sodium ions dissolved in the solution.

  • C) sodium iodide precipitates out of the solution leaving behind the silver ions.

  • D) the iodide ions from the acid primarily react with the nitrate ions from silver nitrate.



A) True

  • A) True

  • B) False



A) True

  • A) True

  • B) False



A) Copper(II) ion

  • A) Copper(II) ion

  • B) Potassium ion

  • C) Silver ion

  • D) None of the above



A) ammonia with hydrochloric acid.

  • A) ammonia with hydrochloric acid.

  • B) hydrofluoric acid with potassium hydroxide.

  • C) sodium hydrogen sulfate with sodium hydroxide.

  • D) hydrochloric acid with potassium hydroxide.



A) ammonia is a Bronsted base and silver chloride a Bronsted acid.

  • A) ammonia is a Bronsted base and silver chloride a Bronsted acid.

  • B) ammonia is slightly acidic so it reacts with the slightly basic chloride ions.

  • C) ammonia forms a soluble complex ion with the silver.

  • D) the Ksp for the silver chloride changes in the presence of ammonia.



A) Cl-

  • A) Cl-

  • B) NO3-

  • C) HSO4-

  • D) CH3COO-

  • E) OH-



A) [H+] > [OH-]

  • A) [H+] > [OH-]

  • B) [H+] < [OH-]

  • C) pH = 0

  • D) Kw = [H+]/[OH-]

  • E) none of the above



A) water becomes more acidic when heated.

  • A) water becomes more acidic when heated.

  • B) water becomes more basic when heated.

  • C) none of these.



A) HCl

  • A) HCl

  • B) NH4Cl

  • C) NaCH3COO

  • D) CH3COOH

  • E) NH3



A) 8.96 mL

  • A) 8.96 mL

  • B) 9.2 mL

  • C) 9.246 mL

  • D) 0.108 mL

  • E) 9.0 mL



A) 1.26 x 10-5

  • A) 1.26 x 10-5

  • B) 2.015 x 10-3

  • C) 1.9 x 10-3

  • D) 2.7 x 10-8

  • E) none of the above



A) fluoride

  • A) fluoride

  • B) chloride

  • C) bromide

  • D) iodide

  • E) carbonate



A) K+

  • A) K+

  • B) Au+

  • C) Zn2+

  • D) Hg2+

  • E) Hg22+



A) Yes



A) Any OH- ions added will react with a weak acid already in solution.

  • A) Any OH- ions added will react with a weak acid already in solution.

  • B) The solution will not change its pH very much even if a concentrated acid is added.

  • C) The solution will not change its pH very much even if a strong base is added.

  • D) Any H+ ions added will react with a conjugate base of a weak acid already in solution.

  • E) all of the above



C

  • C

  • A

  • B

  • D

  • B

  • B

  • B

  • C

  • A

  • C





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