100 ml solution of ph=6 is diluted to 1000ml.resulting solution has ph

To determine the pH of a solution after dilution, we need to understand how pH and concentration relate to each other. When you dilute a solution, you are essentially reducing the concentration of hydrogen ions (H⁺) in that solution. Let's break this down step by step.

Understanding pH and Dilution

The pH scale measures the acidity or basicity of a solution, with lower values indicating higher acidity (more H⁺ ions) and higher values indicating higher basicity (fewer H⁺ ions). The formula for pH is:

pH = -log[H⁺]

In your case, you have a solution with a pH of 6. This means that the concentration of hydrogen ions in the original 100 ml solution can be calculated as follows:

[H⁺] = 10^(-pH)

So, for a pH of 6:

[H⁺] = 10^(-6) = 1 x 10^(-6) moles per liter

Calculating the Effect of Dilution

When you dilute this solution from 100 ml to 1000 ml, you are increasing the volume by a factor of 10. This dilution affects the concentration of hydrogen ions. The new concentration after dilution can be calculated using the dilution formula:

C1V1 = C2V2

Where:

• C1 = initial concentration of H⁺ ions
• V1 = initial volume (100 ml)
• C2 = final concentration of H⁺ ions
• V2 = final volume (1000 ml)

Rearranging the formula to find C2 gives us:

C2 = (C1 * V1) / V2

Substituting the known values:

C2 = (1 x 10^(-6) moles/L * 0.1 L) / 1 L

C2 = 1 x 10^(-7) moles/L

Finding the New pH

Now that we have the new concentration of hydrogen ions, we can find the new pH:

pH = -log[H⁺]

Substituting the new concentration:

pH = -log(1 x 10^(-7)) = 7

Final Thoughts

After diluting the original 100 ml solution with a pH of 6 to a total volume of 1000 ml, the resulting solution will have a pH of 7. This indicates that the solution has become neutral due to the dilution effect, as the concentration of hydrogen ions has decreased significantly. This example illustrates how dilution can shift the pH of a solution, moving it closer to neutrality as the concentration of acidic ions decreases.