Suppose you let x represent the number of moles of acetic acid dissolved in 1 liter of solution. After the acetic acid ionizes 11%, in terms of x, how many moles of acetic acid are left. How many moles of CH3CO2- are formed, and how many moles of H3O is formed? What are the new molar concentrations of these three species? Using Ka, what is the value of x?Teemo said:Homework Statement
In a particular solution, acetic acid is 11% ionized at 25 degrees Celsius. Calculate the pH of the solution and the mass of acetic acid dissolved to yield 1.00 L of solution.
Ka of CH3CO2H: 1.8x10^(-5)
Homework Equations
Ka=([CH3CO2-][H3O+])/[CH3CO2H]
pH=-log[H3O+]
The Attempt at a Solution
I'm not sure how exactly I should begin, as I do not know the concentration of the acetic acid, so I don't know how to solve for [H+]
Chestermiller said:Suppose you let x represent the number of moles of acetic acid dissolved in 1 liter of solution. After the acetic acid ionizes 11%, in terms of x, how many moles of acetic acid are left. How many moles of CH3CO2- are formed, and how many moles of H3O is formed? What are the new molar concentrations of these three species? Using Ka, what is the value of x?
Yes.Teemo said:How exactly would this work? Would it be ([.11x][.11x])/[.89x], where x is original concentration of acetic acid?
Teemo said:Right, I have the answer key which writes that the formula is C=Ka/(degree dissociation)^2, however I'm not sure what this formula is called and why the degree of dissociation is squared.
The percent dissociation of acetic acid refers to the percentage of acetic acid molecules in a solution that have dissociated into hydrogen ions (H+) and acetate ions (CH3COO-). It is a measure of the strength of an acid and is typically expressed as a decimal or percentage.
The percent dissociation of acetic acid can be calculated by taking the concentration of hydrogen ions (H+) in the solution and dividing it by the initial concentration of acetic acid. This value is then multiplied by 100 to get the percentage.
The percent dissociation of acetic acid can be affected by factors such as temperature, concentration of the acid, and the presence of other substances in the solution. Higher temperatures and lower concentrations can increase the percent dissociation, while the presence of certain substances, such as strong bases, can decrease it.
The percent dissociation of acetic acid is important in chemistry because it can help determine the strength of an acid and its behavior in a solution. It is also a key factor in understanding acid-base reactions and their equilibrium constants.
The percent dissociation of acetic acid has many practical applications, such as in the production of vinegar and other food products. It is also used in industries such as pharmaceuticals and cosmetics to control the acidity of products. In addition, it is an important concept in environmental chemistry, as it can affect the pH of natural water sources and the behavior of pollutants.