The Ka value for acetic acid, CH3COOH(aq), is 1.8x10^-5. Calculate the ph of a 2.80 M acetic acid solution.
PH=
Calculate the ph of the resulting solution when 3.00 mL of the 2.80 M acetic acid is diluted to make a 250.0 mL solution.
PH=
Answers are not 4.6 or 3.8
Power of hydrogen ions (pH)
The pH is defined as the negative logarithmic function of the concentration of hydrogen () ion in an aqueous solution.
Molar concentration:
The molar concentration is the number of moles of a solute that will dissolve in a liter of solution. It is expressed as mol/L or M (molarity).
Molar concentration:
Dilution equation:
Acid dissociation constant:
Equation for the pH of the solution:
Henderson–Hasseslbalch Equation:
An ICE table is used to find the concentrations or moles of individual reactants or products at equilibrium.
The expansion of an ICE table is as follows:
All quantities are expressed in terms of concentrations or moles.
(1)
Given data:
Initial concentration of acetic acid, = 2.80 M
At equilibrium: The change in concentration is x.
(2)
Given:
Concentration of acetic acid, = 0.0336 M
At equilibrium: The change in concentration is x.
Ans: Part 1
The pH of a 2.80 M acetic acid solution is
Part 2
The pH of the resulting solution is
The Ka value for acetic acid, CH3COOH(aq), is 1.8x10^-5. Calculate the ph of a 2.80 M...
The Ka value for acetic acid, CH3COOH(aq) , is 1.8×10-5 M . Calculate the pH of a 2.80 M acetic acid solution.Calculate the pH of the resulting solution when 2.50 mL of the 2.80 M acetic acid is diluted to make a 250.0 mL solution.
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