Question

3. Given a H+ concentration of a solution is 6.6 × 10-4 M at 25°C, calculate I. the pH of the solution II. the concentration of hydroxide ion of solution III. the concentration of hydrogen ion in a solution with pOH of 3.9 (Kw = 1.0 × 10-14 mol2 dm-6) 4. Determine the [H3O+] and pH of a 0.1 M solution of benzoic acid. The dissociation constant for benzoic acid is 6.5 × 10-5. 5. Calculate the pH and degree of dissociation for 0.25 M ethylamine solution. The dissociation constant for ethylamine is 5.6 × 10-4. 6. Given that the ionization constant, Ka for HNO2 solution is 4.6 × 10-4 at 25°C. Write the ionization equation of HNO2 solution. Find the pH value and percent ionization of a 2.5 M HNO2 solution. 7. Consider the list of bases and their respective Kb values: Aniline (C6H5NH2); Kb = 3.9 × 10-10 Ethylamine (C2H5NH2); Kb = 5.6 × 10-4 Ammonia (NH3); Kb = 1.8 × 10-5 Arrange the following base in order of decreasing of base strength.

          3.
Given a H<sup>+</sup> concentration of a solution is 6.6 × 10<sup>-4</sup> M at 25°C, calculate
I. the pH of the solution
II. the concentration of hydroxide ion of solution
III. the concentration of hydrogen ion in a solution with pOH of 3.9
(K<sub>w</sub> = 1.0 × 10<sup>-14</sup> mol<sup>2</sup> dm<sup>-6</sup>)
4.
Determine the [H<sub>3</sub>O<sup>+</sup>] and pH of a 0.1 M solution of benzoic acid. The dissociation
constant for benzoic acid is 6.5 × 10<sup>-5</sup>.
5.
Calculate the pH and degree of dissociation for 0.25 M ethylamine solution. The
dissociation constant for ethylamine is 5.6 × 10<sup>-4</sup>.
6.
Given that the ionization constant, K<sub>a</sub> for HNO<sub>2</sub> solution is 4.6 × 10<sup>-4</sup> at 25°C. Write the
ionization equation of HNO<sub>2</sub> solution. Find the pH value and percent ionization of a 2.5 M
HNO<sub>2</sub> solution.
7.
Consider the list of bases and their respective K<sub>b</sub> values:
Aniline (C<sub>6</sub>H<sub>5</sub>NH<sub>2</sub>);     K<sub>b</sub> = 3.9 × 10<sup>-10</sup>
Ethylamine (C<sub>2</sub>H<sub>5</sub>NH<sub>2</sub>); K<sub>b</sub> = 5.6 × 10<sup>-4</sup>
Ammonia (NH<sub>3</sub>);           K<sub>b</sub> = 1.8 × 10<sup>-5</sup>
Arrange the following base in order of decreasing of base strength.

3.
Given a H<sup>+</sup> concentration of a solution is 6.6 × 10<sup>-4</sup> M at 25°C, calculate
I. the pH of the solution
II. the concentration of hydroxide ion of solution
III. the concentration of hydrogen ion in a solution with pOH of 3.9
(K<sub>w</sub> = 1.0 × 10<sup>-14</sup> mol<sup>2</sup> dm<sup>-6</sup>)
4.
Determine the [H<sub>3</sub>O<sup>+</sup>] and pH of a 0.1 M solution of benzoic acid. The dissociation
constant for benzoic acid is 6.5 × 10<sup>-5</sup>.
5.
Calculate the pH and degree of dissociation for 0.25 M ethylamine solution. The
dissociation constant for ethylamine is 5.6 × 10<sup>-4</sup>.
6.
Given that the ionization constant, K<sub>a</sub> for HNO<sub>2</sub> solution is 4.6 × 10<sup>-4</sup> at 25°C. Write the
ionization equation of HNO<sub>2</sub> solution. Find the pH value and percent ionization of a 2.5 M
HNO<sub>2</sub> solution.
7.
Consider the list of bases and their respective K<sub>b</sub> values:
Aniline (C<sub>6</sub>H<sub>5</sub>NH<sub>2</sub>); K<sub>b</sub> = 3.9 × 10<sup>-10</sup>
Ethylamine (C<sub>2</sub>H<sub>5</sub>NH<sub>2</sub>); K<sub>b</sub> = 5.6 × 10<sup>-4</sup>
Ammonia (NH<sub>3</sub>); K<sub>b</sub> = 1.8 × 10<sup>-5</sup>
Arrange the following base in order of decreasing of base strength.

Added by Jeffery C.

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