Rank The Following Solutions From The Highest { H _3 O ^{+} $}$ To The Lowest { H _3 O ^{+} $}$.1. { [ H _3 O ^{+} ]=3.16 \times 10^{-4} M$}$2. { [ OH ^{-} ]=4.35 \times 10^{-2} M$} 3. \[ 3. \[ 3. \[ PH

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Ranking Solutions from Highest to Lowest [H3O+]: A Comprehensive Guide

Understanding pH and [H3O+]

In chemistry, pH is a measure of the concentration of hydrogen ions (H+) in a solution. It is an important concept in understanding the acidity or basicity of a solution. The pH scale ranges from 0 to 14, with a pH of 7 being neutral. A pH less than 7 is considered acidic, while a pH greater than 7 is considered basic.

The concentration of hydrogen ions in a solution is denoted by [H3O+], which is the concentration of hydronium ions (H3O+) in moles per liter (M). The relationship between pH and [H3O+] is given by the equation:

pH = -log[H3O+]

This equation shows that the pH of a solution is inversely proportional to the concentration of hydrogen ions.

Ranking Solutions from Highest to Lowest [H3O+]

To rank the solutions from highest to lowest [H3O+], we need to calculate the pH of each solution using the equation above.

Solution 1: [H3O+] = 3.16 × 10^-4 M

To calculate the pH of this solution, we can use the equation:

pH = -log(3.16 × 10^-4)

pH ≈ 3.5

This solution has a pH of approximately 3.5, which means it is acidic.

Solution 2: [OH^-] = 4.35 × 10^-2 M

To calculate the pH of this solution, we need to first calculate the concentration of hydrogen ions using the equation:

[H3O+] = 10^(-pH)

We can then rearrange this equation to solve for pH:

pH = -log([H3O+])

However, we are given the concentration of hydroxide ions ([OH^-]) instead of hydrogen ions. We can use the equation:

pH + pOH = 14

where pOH is the concentration of hydroxide ions in moles per liter (M).

pOH = -log([OH^-])

pOH = -log(4.35 × 10^-2)

pOH ≈ 1.36

Now, we can calculate the pH of the solution:

pH = 14 - pOH pH ≈ 14 - 1.36 pH ≈ 12.64

This solution has a pH of approximately 12.64, which means it is basic.

Solution 3: pH = 5.5

To calculate the concentration of hydrogen ions in this solution, we can use the equation:

[H3O+] = 10^(-pH)

[H3O+] = 10^(-5.5)

[H3O+] ≈ 3.16 × 10^-6 M

This solution has a concentration of hydrogen ions of approximately 3.16 × 10^-6 M.

Solution 4: pH = 7.2

To calculate the concentration of hydrogen ions in this solution, we can use the equation:

[H3O+] = 10^(-pH)

[H3O+] = 10^(-7.2)

[H3O+] ≈ 6.31 × 10^-8 M

This solution has a concentration of hydrogen ions of approximately 6.31 × 10^-8 M.

Solution 5: pH = 9.1

To calculate the concentration of hydrogen ions in this solution, we can use the equation:

[H3O+] = 10^(-pH)

[H3O+] = 10^(-9.1)

[H3O+] ≈ 1.26 × 10^-10 M

This solution has a concentration of hydrogen ions of approximately 1.26 × 10^-10 M.

Ranking the Solutions from Highest to Lowest [H3O+]

Based on the calculations above, the solutions can be ranked from highest to lowest [H3O+] as follows:

  1. Solution 2: [OH^-] = 4.35 × 10^-2 M with a pH of approximately 12.64 and a concentration of hydrogen ions of approximately 1.26 × 10^-13 M.
  2. Solution 1: [H3O+] = 3.16 × 10^-4 M with a pH of approximately 3.5 and a concentration of hydrogen ions of approximately 3.16 × 10^-4 M.
  3. Solution 3: pH = 5.5 with a concentration of hydrogen ions of approximately 3.16 × 10^-6 M.
  4. Solution 4: pH = 7.2 with a concentration of hydrogen ions of approximately 6.31 × 10^-8 M.
  5. Solution 5: pH = 9.1 with a concentration of hydrogen ions of approximately 1.26 × 10^-10 M.

Therefore, the solutions can be ranked from highest to lowest [H3O+] as follows:

  1. Solution 2: [OH^-] = 4.35 × 10^-2 M
  2. Solution 1: [H3O+] = 3.16 × 10^-4 M
  3. Solution 3: pH = 5.5
  4. Solution 4: pH = 7.2
  5. Solution 5: pH = 9.1
    Frequently Asked Questions (FAQs) about Ranking Solutions from Highest to Lowest [H3O+]

Q: What is the pH scale and how is it related to [H3O+]?

A: The pH scale is a measure of the concentration of hydrogen ions (H+) in a solution. It ranges from 0 to 14, with a pH of 7 being neutral. The concentration of hydrogen ions in a solution is denoted by [H3O+], which is the concentration of hydronium ions (H3O+) in moles per liter (M). The relationship between pH and [H3O+] is given by the equation:

pH = -log[H3O+]

Q: How do I calculate the pH of a solution given the concentration of hydrogen ions?

A: To calculate the pH of a solution, you can use the equation:

pH = -log[H3O+]

where [H3O+] is the concentration of hydrogen ions in moles per liter (M).

Q: How do I calculate the concentration of hydrogen ions in a solution given the pH?

A: To calculate the concentration of hydrogen ions in a solution, you can use the equation:

[H3O+] = 10^(-pH)

Q: What is the difference between pH and pOH?

A: pH is a measure of the concentration of hydrogen ions (H+) in a solution, while pOH is a measure of the concentration of hydroxide ions (OH-) in a solution. The two are related by the equation:

pH + pOH = 14

Q: How do I calculate the pH of a solution given the concentration of hydroxide ions?

A: To calculate the pH of a solution given the concentration of hydroxide ions, you can use the equation:

pH = 14 - pOH

where pOH is the concentration of hydroxide ions in moles per liter (M).

Q: What is the significance of the pH scale in everyday life?

A: The pH scale is important in many areas of everyday life, including:

  • Food and drink: pH is used to determine the acidity or basicity of food and drink, which can affect their taste and nutritional value.
  • Water quality: pH is used to determine the quality of water, which can affect its safety for drinking and other uses.
  • Medicine: pH is used to determine the acidity or basicity of medications, which can affect their effectiveness and safety.
  • Environmental science: pH is used to determine the acidity or basicity of soil and water, which can affect the health of plants and animals.

Q: How do I determine the pH of a solution using a pH meter?

A: To determine the pH of a solution using a pH meter, you can follow these steps:

  1. Calibrate the pH meter using a standard solution of known pH.
  2. Dip the pH meter probe into the solution to be measured.
  3. Read the pH value displayed on the pH meter.

Q: What are some common sources of error when measuring pH?

A: Some common sources of error when measuring pH include:

  • Contamination of the solution with impurities or other substances that can affect the pH.
  • Inaccurate calibration of the pH meter.
  • Incorrect handling or storage of the pH meter.
  • Inadequate training or experience in using the pH meter.

Q: How do I troubleshoot common problems with pH measurement?

A: Some common problems with pH measurement and their solutions include:

  • Inaccurate pH readings: Check the calibration of the pH meter and ensure that it is properly maintained.
  • pH meter not responding: Check the pH meter probe for damage or contamination and ensure that it is properly connected to the pH meter.
  • pH meter giving inconsistent readings: Check the pH meter calibration and ensure that it is properly maintained.
  • pH meter not giving any readings: Check the pH meter probe for damage or contamination and ensure that it is properly connected to the pH meter.