Rank The Following Solutions From The Highest $ \left[ H_3O^+ \right] $ (1) To The Lowest $ \left[ H_3O^+ \right] $ (5).1. $ \left[ H_3O^+ \right] = 3.16 \times 10^{-4} , M $2. $ [OH^-] = 4.35 \times 10^{-2} , M
Understanding pH and Hydrogen Ion Concentration
In chemistry, the concentration of hydrogen ions (H+) in a solution is a crucial factor in determining its acidity or basicity. The pH scale is a measure of the concentration of hydrogen ions in a solution, with lower pH values indicating higher concentrations of hydrogen ions. In this article, we will rank five different solutions based on their hydrogen ion concentrations, from highest to lowest.
Solution 1: $ \left[ H_3O^+ \right] = 3.16 \times 10^{-4} , M $
The first solution has a hydrogen ion concentration of . This solution is considered acidic, as the concentration of hydrogen ions is higher than that of a neutral solution (which has a pH of 7). To determine the pH of this solution, we can use the formula:
pH = -log[H+]
Substituting the value of [H+] into the formula, we get:
pH = -log(3.16 \times 10^{-4}) pH ≈ 3.5
This solution has a pH of approximately 3.5, indicating that it is acidic.
Solution 2: $ [OH^-] = 4.35 \times 10^{-2} , M $
The second solution has a hydroxide ion concentration of . This solution is considered basic, as the concentration of hydroxide ions is higher than that of a neutral solution. To determine the pH of this solution, we can use the formula:
pH = -log[OH-]
Substituting the value of [OH-] into the formula, we get:
pH = -log(4.35 \times 10^{-2}) pH ≈ 1.4
This solution has a pH of approximately 1.4, indicating that it is strongly basic.
Solution 3: $ \left[ H_3O^+ \right] = 1.23 \times 10^{-5} , M $
The third solution has a hydrogen ion concentration of . This solution is considered weakly acidic, as the concentration of hydrogen ions is lower than that of a neutral solution. To determine the pH of this solution, we can use the formula:
pH = -log[H+]
Substituting the value of [H+] into the formula, we get:
pH = -log(1.23 \times 10^{-5}) pH ≈ 4.9
This solution has a pH of approximately 4.9, indicating that it is weakly acidic.
Solution 4: $ [OH^-] = 1.02 \times 10^{-6} , M $
The fourth solution has a hydroxide ion concentration of . This solution is considered weakly basic, as the concentration of hydroxide ions is lower than that of a neutral solution. To determine the pH of this solution, we can use the formula:
pH = -log[OH-]
Substituting the value of [OH-] into the formula, we get:
pH = -log(1.02 \times 10^{-6}) pH ≈ 5.9
This solution has a pH of approximately 5.9, indicating that it is weakly basic.
Solution 5: $ \left[ H_3O^+ \right] = 6.21 \times 10^{-7} , M $
The fifth solution has a hydrogen ion concentration of . This solution is considered neutral, as the concentration of hydrogen ions is equal to that of a neutral solution. To determine the pH of this solution, we can use the formula:
pH = -log[H+]
Substituting the value of [H+] into the formula, we get:
pH = -log(6.21 \times 10^{-7}) pH ≈ 6.2
This solution has a pH of approximately 6.2, indicating that it is neutral.
Ranking the Solutions
Based on the pH values calculated above, we can rank the solutions from highest to lowest hydrogen ion concentration as follows:
- Solution 2: $ [OH^-] = 4.35 \times 10^{-2} , M $ (pH ≈ 1.4)
- Solution 1: $ \left[ H_3O^+ \right] = 3.16 \times 10^{-4} , M $ (pH ≈ 3.5)
- Solution 3: $ \left[ H_3O^+ \right] = 1.23 \times 10^{-5} , M $ (pH ≈ 4.9)
- Solution 4: $ [OH^-] = 1.02 \times 10^{-6} , M $ (pH ≈ 5.9)
- Solution 5: $ \left[ H_3O^+ \right] = 6.21 \times 10^{-7} , M $ (pH ≈ 6.2)
Q: What is the pH scale?
A: The pH scale is a measure of the concentration of hydrogen ions (H+) in a solution. It ranges from 0 to 14, with lower pH values indicating higher concentrations of hydrogen ions and higher pH values indicating lower concentrations of hydrogen ions.
Q: What is the difference between acidic and basic solutions?
A: Acidic solutions have a higher concentration of hydrogen ions (H+) than basic solutions. Basic solutions have a higher concentration of hydroxide ions (OH-) than acidic solutions.
Q: How do I determine the pH of a solution?
A: To determine the pH of a solution, you can use the formula:
pH = -log[H+]
where [H+] is the concentration of hydrogen ions in the solution.
Q: What is the pH of a neutral solution?
A: The pH of a neutral solution is 7. This is because the concentration of hydrogen ions (H+) is equal to the concentration of hydroxide ions (OH-).
Q: Can a solution have a pH greater than 14?
A: No, a solution cannot have a pH greater than 14. The pH scale only ranges from 0 to 14.
Q: What is the relationship between pH and hydrogen ion concentration?
A: The pH of a solution is inversely proportional to the concentration of hydrogen ions (H+). This means that as the concentration of hydrogen ions increases, the pH of the solution decreases.
Q: Can a solution be both acidic and basic at the same time?
A: No, a solution cannot be both acidic and basic at the same time. A solution can either be acidic or basic, but not both.
Q: How do I determine the type of solution (acidic or basic) based on its pH?
A: If the pH of a solution is less than 7, it is acidic. If the pH of a solution is greater than 7, it is basic. If the pH of a solution is equal to 7, it is neutral.
Q: Can a solution have a pH of exactly 7?
A: Yes, a solution can have a pH of exactly 7. This is because the concentration of hydrogen ions (H+) is equal to the concentration of hydroxide ions (OH-).
Q: What is the significance of pH in everyday life?
A: pH is an important concept in everyday life, as it affects the taste, texture, and safety of many substances. For example, a low pH can make a substance taste sour, while a high pH can make a substance taste bitter. Additionally, pH can affect the safety of substances, as high or low pH values can indicate the presence of harmful substances.
Q: Can pH be used to determine the quality of water?
A: Yes, pH can be used to determine the quality of water. Water with a pH that is too high or too low can indicate the presence of harmful substances, such as heavy metals or bacteria.
Q: How do I measure pH in a solution?
A: There are several ways to measure pH in a solution, including using pH paper, pH meters, and pH probes. Each of these methods has its own advantages and disadvantages, and the choice of method will depend on the specific needs of the experiment.
Q: What is the difference between pH and pOH?
A: pH and pOH are two related but distinct concepts. 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-). The relationship between pH and pOH is given by the equation:
pH + pOH = 14
This equation shows that as the pH of a solution increases, the pOH of the solution decreases, and vice versa.