Test Acids and Bases

1. The pH of a solution is 2 at 25 °C. What is the pOH of this solution?
   (1) 0; (2) 2:(3) 12; (4) 14.
2. In a solution with a pH of 3 the color of (1) litmus is red; (2) litmus is
   blue;(3) phenolphthalein is red; (4) phenolphthalein is blue.
3. What is the total number of moles of H1+ ions that will neutralize 2.0 moles
   of OH1-ions? (1) 1.0; (2) 2.0; (3) 17; (4) 34.
4. Which salt hydrolyzes in water to form a solution that is acidic? (1) KCl;
   ( 2) NH4Cl;(3) NaCl; (4) LiCl.
5. Which particle is amphiprotic? (1) HNO3 ; (2) NO31- ; (3) NH3 ; (4) NH41+ .
6. As 50. milliliters of 0.1 M HCl is added to 100 milliliters of 0.1 M NaOH the
   pH of theNaOH solution (1) decreases; (2) increases; (3) remains the same.
7. Which compound is an electrolyte? (1) C6H12O6 ; (2) C12H22O11; (3) C2H5OH
   (4) CH3COOH.
8. The hydroxide ion concentration is greater than the hydronium ion concentration in a 0.1 M solution of (1) NaOH; (2) CH3OH; (3) HNO3 ; (4) H2SO4.
9. What is the pH of a solution whose hydronium ion concentration is 0.0001 moles per
   liter? (1) 1; (2) 10; (3) 14; (4) 4.
10. The conjugate base of the bisulfite ion is the (1) sulfide ion; (2) sulfite ion;
    (3) bisulfate ion; (4) sulfate ion.
11. A weak acid (HX) has an equilibrium constant of 1.0 X 10-8. What is the pH of a 1.0
    M solution of this acid? (1) 1; (2) 7; (3) 8; (4) 4.
12. If 6 milliliters of 1M HCl is exactly neutralized by 3 milliliters of KOH then the
    molarity of the KOH is (1) 1M; (2) 2M; (3) 3M; (4) 9M.
13. The pH of 0.001M HCl is (1) 1; (2) 2; (3) 3; (4) 4.
14. NH3 + H2O = NH4 1+ + OH1- Given the above reaction the two Bronsted acids are
    (1) NH3 and H2O; (2) NH3 and OH1- ; (3) NH4 1+ and H2O ; (4) NH4 1+ and OH1- .
15. An organic compound whose water solution turns litmus red is (1) CH3OH; (2) C6H12;(3) CH3COOH; (4) C6H12O6 .
16. Which could act as either a Bronsted acid or a Bronsted base? (1) chloride ion;
    (2) sulfide ion; (3) bisulfide ion; (4) carbonate ion.
17. Which solution will be exactly neutralized by 1.0 liter of 1.0M NaOH? (1) 1.0 liter
    of 0.50M HCl; (2) 1.0 liter of 2.0M HCl; (3) 0.50 liter of 0.50M HCl; (4) 0.50 liter
    of 2.0M HCl.
    17. Which solution will be exactly neutralized by 1.0 liter of 1.0M NaOH? (1) 1.0 liter
    of 0.50M HCl; (2) 1.0 liter of 2.0M HCl; (3) 0.50 liter of 0.50M HCl; (4) 0.50 liter
    of 2.0M HCl.
18. Which pH indicates the highest concentration of hydronium ions? (1) 1; (2) 7;
    (3) 10; (4) 14.
19. Which 0.1M aqueous solution is the poorest conducter of electricity? (1) C2H5OH;
    (2) HCl; (3) H2SO4 ; (4) NH3 .
20. Which of the following 0.1 M solutions is the best conductor of electricity? (1) HNO3
    ; (2) HNO2 ; (3) NH3 ; (4) CH3COOH .
21. Which of the following is the weakest Bronsted acid? (1) HBr; (2) HI; (3) HCl;
    (4) HF.
22. When K2CO3 dissolves in water the resulting solution turn litmus paper (1) red
    and is acidic; (2) blue and is acidic; (3) red and is basic; (4) blue and is basic.
23. A 30 milliliter sample of HCl is completely neutralized by 10. milliliters of a 1.5 M
    NaOH solution. What is the molarity of the HCl solution? (1) 0.25; (2) 0.50;
    (3) 1.5; (4) 4.5.
24. Which could be the pH of a solution whose hydronium ion concentration is less than
    the hydroxide ion concentration? (1) 9; (2) 2; (3) 3; (4) 4.
25. A solution of which metallic ion would have an acid pH? (1) sodium; (2) aluminum;
    (3) potassium; (4) lithium.
26. Which compound is the weakest electrolyte? (1) HCl; (2) HNO3 ; (3) H2S;
    (4) H2SO4 .
27. Which hydrogen ion concentration indicates the most acidic solution? (1) 1 x
    10-11M; (2) 1 x 10-9 M; (3) 1 x 10-7 M; (4) 1 x 10-5 M.
28. Which compound is correctly classified as a salt? (1) KNO3 ; (2) HNO3 ; (3) CH3COOH
    ; (4) C2H5OH .
29. How many milliliters of 2.0 M NaOH are needed to exactly neutralize 50 mL of 2.0
    M HCl? (1) 25; (2) 50; (3) 100; (4) 200.
30. In the reaction H2O + H2O ------> H3O1+ + OH1- water is acting as (1) a Bronsted
    acid only; (2) a Bronsted base only; (3) neither a Bronsted acid nor base; (4) both
    a Bronsted acid and base.
31. Which of the following combinations when dissolved in water would produce an
    acidic buffer? (1) KCl and NaCl; (2) NaOH and HOH; (3) NaCl and HCl;
    (4) CH3COOH and NaCH3COO .
32. When titrating a strong acid and a weak base the stoichiometric point may have a
    pH of (1) 0; (2) 7; (3) 5; (4) 9.
33. Which 0.1 molar aqueous solution contains the highest concentration of OH1- ions?
    (1) CH3OH ; (2) NaOH ; (3) C2H5OH ; (4) NH3 .
34. Red litmus will turn blue when placed in an aqueous solution of (1) HCl; (2) CH3COOH;
    (3) KOH; (4) CH3OH.
35. Which ion is amphiprotic? (1) Cl1- ; (2) HSO41- ; (3) O2- ; (4) NH41+ .
36. A solution at 25 degrees Celsius with a pH of 7 contains (1) more hydronium ions
    than hydroxide ions; (2) fewer hydronium ions than hydroxide ions; (3) an equal
    number of hydronium ions and hydroxide ions; (4) no hydronium ions or hydroxide
    ions.
37. Which acid is almost completely ionized in a dilute solution at 25 °C? (1) CH3COOH;
    (2) H2S; (3) H3PO4 ; (4) HNO3 .
38. A solution of potassium carbonate would have a pH closest to (1) 1; (2) 5; (3) 3;(4) 8.
39. How many liters of 2.5 M HCl are required to exactly neutralize 1.5 liters of 5.0 M
    NaOH? (1) 1.0; (2) 2.0; (3) 3.0; (4) 4.0.
40. What are the Bronsted-Lowry bases in the following reaction:
    H2S + H2O ------> H3O1+ + HS1- ? (1) H2S and H2O; (2) H 2S and H3O1+ ; (3) HS1-and H2O; (4) HS1- and H3O1+ .
41. When additional solid NaCl dissolves in a solution of NaCl in water the pH of the
    solution (1) decreases; (2) increases; (3) remains the same.
42. When hydrochloric acid is neutralized by sodium hydroxide then the salt formed is
    sodium (1) hydrochlorate; (2) chlorate; (3) chloride; (4) perchloride.
43. The ionization constant of 1.8 x 10-5 is for a weak acid. A reasonable pH for a 0.1 M
    solution of this acid would be (1) 1; (2) 9; (3) 3; (4) 14.
44. A 1 molal solution of magnesium chloride has a higher boiling point than a 1 molal
    solution of solution of (1) FeCl3 ; (2) CaCl2 ; (3) BaCl2 ; (4) NaCl.
45. A water solution of which gas contains more hydroxide ions than hydronium ions?
    (1) HCl; (2) NH3 ; (3) CO2 ; (4) SO2 .
46. The following are hydrogen ion concentrations. Which hydrogen ion concentration
    indicates the strongest acid? (1) 1.0 x 10-4; (2) 2.0 x 10-5; (3) 3.0 x 10-6; (4) 4.0 x
    10-7.
47. How many milliliters of 0.200 molar NaOH are needed to neutralize 100 milliliters
    of 0.100 molar HCl? (1) 40.0; (2) 50.0; (3) 100.; (4) 200.
48. Given the following reaction: H2SO4 + H2O ======> HSO41- + H3O1+ . The two
    Bronsted-Lowry acids are (1) H2SO4 and H2O; (2) H2SO4 and H3O1+ ; (3) H2O and
    H3O1+ ; (4) HSO4 1- and H3O1+ .
49. Neutralization of 15 milliliters of a 1.0-molar solution of KOH requires 5 milliliters
    of hydrochloric acid. What is the molarity of the HCl solution? (1) 1.0; (2) 2.0;
    (3) 3.0; (4) 6.0.
50. Which solution is the best conductor of electricity? (1) 1.0 M boric acid; (2) 1.0 M
    carbonic acid; (3) 1.0 M acetic acid; (4) 1.0 M hydrochloric acid.