What Is The PH Of A Solution With $\left[ H^{+} \right] = 2.3 \times 10^{-6}$?A. 6.00 B. -5.64 C. -0.36 D. 5.64

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Introduction to pH

pH is a measure of the concentration of hydrogen ions (H+) in a solution. It is a crucial concept in chemistry, as it helps us understand the acidity or basicity of a solution. The pH scale ranges from 0 to 14, with 7 being the neutral point. A pH less than 7 indicates an acidic solution, while a pH greater than 7 indicates a basic solution.

The pH Formula

The pH of a solution can be calculated using the formula:

pH = -log[H+]

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

Calculating pH from Hydrogen Ion Concentration

To calculate the pH of a solution with a given hydrogen ion concentration, we can use the formula above. Let's consider the given problem:

What is the pH of a solution with [H+] = 2.3 × 10^(-6)?

Step 1: Understand the Given Concentration

The given concentration of hydrogen ions is 2.3 × 10^(-6) M. This means that there are 2.3 × 10^(-6) moles of hydrogen ions per liter of solution.

Step 2: Apply the pH Formula

Now, we can apply the pH formula to calculate the pH of the solution:

pH = -log(2.3 × 10^(-6))

Step 3: Calculate the Logarithm

To calculate the logarithm, we can use a calculator or a logarithmic table. The logarithm of 2.3 × 10^(-6) is approximately -5.64.

Step 4: Calculate the pH

Now, we can calculate the pH by multiplying the logarithm by -1:

pH = -(-5.64) = 5.64

Conclusion

Therefore, the pH of a solution with [H+] = 2.3 × 10^(-6) is 5.64.

Significance of pH in Chemistry

pH is a crucial concept in chemistry, as it helps us understand the acidity or basicity of a solution. It is used in various applications, such as:

  • Water Treatment: pH is used to determine the acidity or basicity of water, which is essential for water treatment processes.
  • Soil Science: pH is used to determine the acidity or basicity of soil, which affects plant growth and nutrient availability.
  • Biology: pH is used to determine the acidity or basicity of biological systems, such as blood and tissues.

Common pH Values

Here are some common pH values and their corresponding acidity or basicity:

  • Acidic Solutions: pH < 7 (e.g., stomach acid, pH = 1.5-3.5)
  • Neutral Solutions: pH = 7 (e.g., pure water, pH = 7)
  • Basic Solutions: pH > 7 (e.g., baking soda, pH = 8-9)

Conclusion

In conclusion, pH is a measure of the concentration of hydrogen ions in a solution. It is a crucial concept in chemistry, as it helps us understand the acidity or basicity of a solution. The pH formula is pH = -log[H+], where [H+] is the concentration of hydrogen ions in moles per liter (M). By applying this formula, we can calculate the pH of a solution with a given hydrogen ion concentration.

Frequently Asked Questions

  • What is the pH of a solution with [H+] = 1.0 × 10^(-7)? Answer: pH = 6.99
  • What is the pH of a solution with [H+] = 5.0 × 10^(-5)? Answer: pH = 4.30
  • What is the pH of a solution with [H+] = 1.0 × 10^(-3)? Answer: pH = 3.00

References

  • CRC Handbook of Chemistry and Physics: This reference book provides a comprehensive table of pH values for various substances.
  • Chemical Engineering Handbook: This reference book provides a comprehensive discussion of pH and its applications in chemical engineering.
  • Biology Textbooks: This reference book provides a comprehensive discussion of pH and its applications in biology.

Understanding pH and Its Significance

pH is a measure of the concentration of hydrogen ions (H+) in a solution. It is a crucial concept in chemistry, as it helps us understand the acidity or basicity of a solution. The pH scale ranges from 0 to 14, with 7 being the neutral point. A pH less than 7 indicates an acidic solution, while a pH greater than 7 indicates a basic solution.

Q&A: pH and Its Applications

Q: What is the pH of a solution with [H+] = 1.0 × 10^(-7)?

A: The pH of a solution with [H+] = 1.0 × 10^(-7) is 7.00.

Q: What is the pH of a solution with [H+] = 5.0 × 10^(-5)?

A: The pH of a solution with [H+] = 5.0 × 10^(-5) is 4.30.

Q: What is the pH of a solution with [H+] = 1.0 × 10^(-3)?

A: The pH of a solution with [H+] = 1.0 × 10^(-3) is 3.00.

Q: What is the pH of a solution with [H+] = 2.3 × 10^(-6)?

A: The pH of a solution with [H+] = 2.3 × 10^(-6) is 5.64.

Q: What is the pH of a solution with [H+] = 1.0 × 10^(-4)?

A: The pH of a solution with [H+] = 1.0 × 10^(-4) is 4.00.

Q: What is the pH of a solution with [H+] = 5.0 × 10^(-6)?

A: The pH of a solution with [H+] = 5.0 × 10^(-6) is 5.30.

Q: What is the pH of a solution with [H+] = 1.0 × 10^(-5)?

A: The pH of a solution with [H+] = 1.0 × 10^(-5) is 5.00.

Q: What is the pH of a solution with [H+] = 2.0 × 10^(-5)?

A: The pH of a solution with [H+] = 2.0 × 10^(-5) is 4.70.

Q: What is the pH of a solution with [H+] = 1.0 × 10^(-6)?

A: The pH of a solution with [H+] = 1.0 × 10^(-6) is 6.00.

Q: What is the pH of a solution with [H+] = 5.0 × 10^(-7)?

A: The pH of a solution with [H+] = 5.0 × 10^(-7) is 6.30.

Q: What is the pH of a solution with [H+] = 1.0 × 10^(-8)?

A: The pH of a solution with [H+] = 1.0 × 10^(-8) is 8.00.

Conclusion

In conclusion, pH is a measure of the concentration of hydrogen ions in a solution. It is a crucial concept in chemistry, as it helps us understand the acidity or basicity of a solution. The pH formula is pH = -log[H+], where [H+] is the concentration of hydrogen ions in moles per liter (M). By applying this formula, we can calculate the pH of a solution with a given hydrogen ion concentration.

Frequently Asked Questions (FAQs)

  • What is the pH of a solution with [H+] = 1.0 × 10^(-9)? Answer: pH = 9.00
  • What is the pH of a solution with [H+] = 5.0 × 10^(-9)? Answer: pH = 8.30
  • What is the pH of a solution with [H+] = 1.0 × 10^(-10)? Answer: pH = 10.00

References

  • CRC Handbook of Chemistry and Physics: This reference book provides a comprehensive table of pH values for various substances.
  • Chemical Engineering Handbook: This reference book provides a comprehensive discussion of pH and its applications in chemical engineering.
  • Biology Textbooks: This reference book provides a comprehensive discussion of pH and its applications in biology.