Determination of the Dissociation Constant and Molar Mass for a Weak Acid
Abstract: We will determine Ka and the molar mass for an unknown weak acid by using a pH meter to record the pH at intervals during the titration with sodium hydroxide. The titration curve and its first derivative will be plotted to establish the equivalence point. Introduction The strength of an acid is defined by its ability to donate a proton to a base. For many common acids, we can quantify acid strength by expressing it as the equilibrium constant for the reaction in which the acid donates a proton to the standard base, water, as shown in the equations below: HA + H2O Û H3O+ + A-, for H3CCOOH: H3CCOOH + H2O Û H3O+ + H3CCOO - The equilibrium constant for a reaction of this type is called the Acid Dissociation Constant, "Ka", for the acid HA Determination of the Dissociation Constant and Molar Mass for a Weak Acid
Abstract: We will determine Ka and the molar mass for an unknown weak acid by using a pH meter to record the pH at intervals during the titration with sodium hydroxide. The titration curve and its first derivative will be plotted to establish the equivalence point. Introduction The strength of an acid is defined by its ability to donate a proton to a base. For many common acids, we can quantify acid strength by expressing it as the equilibrium constant for the reaction in which the acid donates a proton to the standard base, water, as shown in the equations below: HA + H2O Û H3O+ + A-, for H3CCOOH: H3CCOOH + H2O Û H3O+ + H3CCOO - The equilibrium constant for a reaction of this type is called the Acid Dissociation Constant, "Ka", for the acid HA Determination of the Dissociation Constant and Molar Mass for a Weak Acid
Abstract: We will determine Ka and the molar mass for an unknown weak acid by using a pH meter to record the pH at intervals during the titration with sodium hydroxide. The titration curve and its first derivative will be plotted to establish the equivalence point. Introduction The strength of an acid is defined by its ability to donate a proton to a base. For many common acids, we can quantify acid strength by expressing it as the equilibrium constant for the reaction in which the acid donates a proton to the standard base, water, as shown in the equations below: HA + H2O Û H3O+ + A-, for H3CCOOH: H3CCOOH + H2O Û H3O+ + H3CCOO - The equilibrium constant for a reaction of this type is called the Acid Dissociation Constant, "Ka", for the acid HA
equilibrium constant
Any circle will work!
pi is a constant = 3.141592654 . . . . circle area = pi * ( ( diameter/2 )2 )
If the direction of motion is constant then the velocity is the same as the speed in that direction. If the direction is not constant, the information given is nowhere near sufficient to calculate the velocity.
wavelength since frequency =hc/lambda h=plancks constant and c=velocity of light
The strength of an acid or the measure of its tendency to release proton ions (H+) can be indicated from its dissociation constant which is called Ka. The acid dissociation constant, pKa , is the negative logarithm of dissociation constant (Ka).
Alkaline, but you need to know the concentration and the dissociation constant to calculate pH
The dissociation constant of pure water is 1.9E-5.
An acid dissociation constant is the equilibrium constant for the disassociation of an acid, ultimately a measure of the acid's strength.
The dissociation constant is:k = [H][X]/[HX]
The dissociation constant is:k = [H][X]/[HX]
equilibrium constant
the pKs is 18.
The dissociation constant is 3.715 x 10-5 for the first step and 3.89 x 10-6 for the second step.
acid dissociation constant
Temperature
Acid dissociation constant