Equation for ph values at different volumes in weak acid and strong babse tutration
Answers
Answered by
3
Helllooo!
When calculating pH, remember that [] refers to molarity, M. Molarity is expressed in units of moles of solute per liter of solution (not solvent). Using the concentration of hydrogen and hydroxide ions, the following relationship results:
Kw = [H+][OH-] = 1x10-14 at 25°C
for pure water [H+] = [OH-] = 1x10-7
Acidic Solution: [H+] > 1x10-7
Basic Solution: [H+] < 1x10-7
HOW TO CALCULATE PH AND [H+]
The equilibrium equation yields the following equation for pH:
pH = -log10[H+]
[H+] = 10-pH
Example:
Calculate the pH for a specific [H+]. Calculate pH given [H+] = 1.4 x 10-5 M
pH = -log10[H+]
pH = -log10(1.4 x 10-5)
pH = 4.85
hope this helps you!!
When calculating pH, remember that [] refers to molarity, M. Molarity is expressed in units of moles of solute per liter of solution (not solvent). Using the concentration of hydrogen and hydroxide ions, the following relationship results:
Kw = [H+][OH-] = 1x10-14 at 25°C
for pure water [H+] = [OH-] = 1x10-7
Acidic Solution: [H+] > 1x10-7
Basic Solution: [H+] < 1x10-7
HOW TO CALCULATE PH AND [H+]
The equilibrium equation yields the following equation for pH:
pH = -log10[H+]
[H+] = 10-pH
Example:
Calculate the pH for a specific [H+]. Calculate pH given [H+] = 1.4 x 10-5 M
pH = -log10[H+]
pH = -log10(1.4 x 10-5)
pH = 4.85
hope this helps you!!
Similar questions