Complete the table. (The first row is completed for you.)

[H3O+] |
[OH−] |
pOH |
pH |
Acidic or Basic |

1.0 × 10−4 |
1.0 × 10−10 |
10.00 |
4.00 |
Acidic |

5.5 × 10−3 |
________ |
________ |
________ |
________ |

________ |
3.2 × 10−6 |
________ |
________ |
________ |

4.8 × 10−9 |
________ |
________ |
________ |
________ |

________ |
________ |
________ |
7.55 |
________ |

Solution 101P: Here, we are going to complete the given table.

Step1:

pH is the negative logarithm to base 10 of hydrogen ion concentration whereas pOH is the negative logarithm to base 10 of hydroxyl ion concentration, i.e.,

pOH = - log[OH- ] and pH = - log[H+ ]

And pH + pOH =14

We can distinguish acidic, neutral and basic aqueous solutions by the relative values of their pH

Acidic: pH < 7

Neutral: pH = 7

Basic: pH > 7

Step2:

[H3O+] | [OH-] | pOH | pH | Acidic or Basic |

1.0 x 10-4 | 1.0 x 10-10 | 10.00 | 4.00 | Acidic |

5.5 x 10-3 | 1.82 x 10-12 | 11.74 | 2.26 | Acidic |

3.13 x 10-9 | 3.2 x 10-6 | 5.495 | 8.505 | Basic |

4.8 x 10-9 | 2.08 x 10-6 | 5.681 | 8.319 | Basic |

2.82 x 10-8 | 3.55 x 10-7 | 6.45 | 7.55 | Basic |

Therefore, pH = - log[H3O+ ]

= - log (5.5 x 10-3)

= - log 5.5 - log 10-3

= - 0.740 + 3

= 2.26

Therefore,...