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| 1 |
In the reaction,
HNO3(aq) + H2O(l) = H3O+ + NO3-
the water is a: |
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Brönsted acid |
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Brönsted base |
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conjugate acid |
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conjugate base |
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None of the previous answers. |
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| 2 |
In the reaction,
HNO3(aq) + H2O(l) = H3O+ + NO3-
the nitrate is the: |
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Brönsted acid |
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Brönsted base |
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conjugate acid |
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conjugate base |
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None of the previous answers. |
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| 3 |
In the reaction,
NH3(aq) + H2O(l) = NH4+ + OH-
the water is a: |
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Brönsted acid |
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Brönsted base |
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conjugate acid |
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conjugate base |
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None of the previous answers. |
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| 4 |
In the reaction,
NH3(aq) + H2O(l) = NH4+ + OH-
the ammonium ion is the: |
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Brönsted acid |
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Brönsted base |
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conjugate acid |
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conjugate base |
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None of the previous answers. |
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| 5 |
In the reaction,
CO32- + H2O(l) = HCO3- + OH-
water is a: |
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Brönsted acid |
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Brönsted base |
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conjugate acid |
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conjugate base |
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None of the previous answers. |
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| 6 |
In the reaction,
CO32- + H2O(l) = HCO3- + OH-
the bicarbonate ion is the: |
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Brönsted acid |
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Brönsted base |
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conjugate acid |
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conjugate base |
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None of the previous answers. |
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| 7 |
In the reaction,
H2PO4- + H2O(l) = H3O+ + HPO42-
the dihydrogen phosphate ion is a: |
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Brönsted acid |
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Brönsted base |
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conjugate acid |
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conjugate base |
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None of the previous answers. |
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| 8 |
In the reaction,
H2PO4- + H2O(l) = H3O+ + HPO42-
the hydrogen phosphate ion is the: |
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Brönsted acid |
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Brönsted base |
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conjugate acid |
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conjugate base |
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None of the previous answers. |
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| 9 |
For the next several questions, remember that p = -log10 thus pH = -log10[H+] where [H+] is the hydrogen ion concentration. Also in aqueous solution [H+][OH-] = 1x10-14 and derivable from the last equation pH + pOH = 14.
What is the approximate pH of a 1x10-4 M HCl solution? |
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1 |
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4 |
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10 |
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7 |
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None of the previous answers. |
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| 10 |
What is the approximate pH of a solution that has a 1x10-8 M H+ concentration? |
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8 |
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6 |
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7 |
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1x10-8 |
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None of the previous answers. |
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| 11 |
What is the approximate pH of a 1x10-3 M NaOH solution? |
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3 |
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11 |
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7 |
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1x10-11 |
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None of the previous answers. |
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| 12 |
What is the approximate [H+] in a solution with pH = 2? |
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1x10-12 M |
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12 M |
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1x10-7 M |
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1x10-2 M |
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None of the previous answers. |
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| 13 |
What is the approximate [OH-] in a solution with pH = 9? |
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1x10-9 M |
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5 |
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1x10-5 M |
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1x10-7 M |
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None of the previous answers. |
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| 14 |
A solution with pH = 2 has how many times more hydrogen ion concentration than one with pH = 4? |
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2 |
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100 |
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20 |
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1/100 |
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None of the previous answers. |
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| 15 |
What is the approximate pH of a 5x10-3 M HCl solution? |
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2.3 |
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3.3 |
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11.7 |
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None of the previous answers. |
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| 16 |
What is the approximate [H+] in a solution with pH = 4.7? |
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5x104 M |
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5x10-10 M |
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2x10-5 M |
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None of the previous answers. |
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| 17 |
0.7120 grams of a primary standard acid (potassium hydrogen phthalate, molecular mass = 204.23 g/mol) requres 21.68 mL of a sodium hydroxide solution of unknown concentration to reach the end point. What is the molarity of the sodium hydroxide solution? |
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32.84 M |
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0.1608 M |
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1.608x10-4 M |
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13.23 M |
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None of the previous answers. |
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| 18 |
If 17.0 mL of a 0.123 M barium hydroxide solution are required to neutralize 25.0 mL of a hydrochloric acid solution, what is the concentration of the hydrochloric acid solution? |
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0.167 M |
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0.0836 M |
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0.0418 M |
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0.362 M |
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None of the previous answers. |
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| 19 |
If 24.7 mL of a 0.120 M sodium hydroxide solution are required to neutralize 0.462 grams of an unknown monoprotic acid, what is the molecular mass of the acid? |
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6.42x10-3 g/mol |
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2.24 g/mol |
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6.42 g/mol |
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156 g/mol |
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None of the previous answers. |
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| 20 |
Write the net ionic equation for the reaction of sodium hydroxide with hydrochloric acid. |
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Na+ + Cl- = NaCl |
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Na+ + Cl- + H+ + OH- = NaCl + H2O(l) |
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H+ + OH- = H2O(l) |
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None of the previous answers. |
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