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At the equivalence point if pH of HA is 8 and the pH of HB is 9 which is the stronger acid?
At first one has to suppose that the concentrations of HA and HB are the same! 1)
Eq.P. at pH=8: You need less OH- (titrant) to reach this, so the acid donated its last proton easier, so it was stronger. (Eq.P. at pH=7 means it isn't weak at all)
1) It is more accurate to compare pH value's half-the-wayof titration, because pH1/2way is exactly equal to pKa value of the acid concerned AND it is independent of concentration: it is buffered!!!
What else can I help you with?
A 0.361 molar solution of the weak acid HA with a pKa of 4.039 is titrated with a 0.163 molar solution of NaOH. What is the pH of the solution at the equivalence point of this titration?
At the equivalence point of the titration, all the weak acid HA has been neutralized by the strong base NaOH. This results in the formation of the conjugate base A-. The pH at the equivalence point of this titration would be determined by the salt formed by the reaction of the weak acid and strong base, and can be calculated using the Henderson-Hasselbalch equation.
At the equivalence point if pH of HA is 8 and the pH of HB is 9 which is the stronger acid Also which conjugate base would be stronger A or B?
Conjugate base B- is stronger, it has a higher pH at Eq.P.Your first (and also the original) question is answered as follows:At first one has to suppose that the concentrations of HA and HB are the same! 1)Eq.P. at pH=8: You need less OH- (titrant) to reach this, so the acid donated its last proton easier, so it was stronger. (Eq.P. at pH=7 means it isn't weak at all)1) It is more accurate to compare pH value's half-the-wayof titration, because pH1/2way is exactly equal to pKa value of the acid concerned AND it is independent of concentration: it is buffered!!!
What would be the pH at the half-equivalence point in titration of a monoprotic acid with NaOH solution if the acid has Ka equals 5.2x10-6?
At the half-equivalence point, the moles of acid initially present are equal to the moles of base added. This corresponds to half the acid being neutralized, forming a buffer solution. The pH can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the acid.
How do you calculate a dissociation constant?
Determination of the Dissociation Constant and Molar Mass for a Weak AcidAbstract: 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 AcidAbstract: 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 AcidAbstract: 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
What is the acid dissociation constant for an acid at equilibrium H?
The acid dissociation constant (Ka) is a measure of the strength of an acid in solution. It is defined as the ratio of the concentration of the dissociated form of the acid (H+) to the undissociated form (HA) at equilibrium. Mathematically, it is expressed as Ka = [H+][A-] / [HA], where [H+] is the concentration of hydrogen ions, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the undissociated acid.
What is the formula for one acid and one base?
HCl is hydrochloric acid and NaOH is sodium hydroxide a base.
How do you help someone dropping out of school?
no point in trying, their done ha ha ha
How can one calculate the acid dissociation constant (Ka) from the concentration of a solution?
To calculate the acid dissociation constant (Ka) from the concentration of a solution, you can use the formula Ka HA- / HA, where H is the concentration of hydrogen ions, A- is the concentration of the conjugate base, and HA is the concentration of the acid.
Will the combination of the cation of a base and the anion of an acid be a conjugate base?
Each cationic acid HA+, when it donates ONE proton H+, will form its conjugated base A of the acid HA+. (Example: NH4+ ammonium, acid NH3 ammonia, base)Each neutral acid HA, when it donates ONE proton H+, will form its conjugated base A- of the acid HA. (Example: CH3COOH acetic acid CH3COO- acetate, base)Each anionic acid HA-, when it donates ONE proton H+, will form its conjugated base A2- of the acid HA-. (Example: HS- (mono)hydrogen sulfide, acid S2- sulfide, base)Each anionic base HA-, when it adopts ONE proton H+, will form its conjugated acid H2A of the base HA-. (Example: HS- mono-hydrogen sulfide, base H2S di-hydrogen sulfide, acid)Each anionic base A-, when it adopts ONE proton H+, will form its conjugate acid HA of base A-. (Example: CH3COO- acetate, base CH3COOH acetic acid)Each neutral base A, when it adopts ONE proton H+, will form its conjugate acid HA of base A-. (Example: NH3 ammonia, base NH4+ ammonium, acid)
How do i calculate pH given the acid constant?
For a weak acid, HA...HA ==> H^+ + A^- Ka = [H+][A-]/[HA] Plug these values into the Ka equation. You also must know the [HA] that you start with. Solve for [H+] Take -log [H+] = pH
Which grid lines will never meet?
parallel lines intersecting lines will meet at some point (ha ha point! get it?)
How to calculate the Ka of an acid?
To calculate the Ka of an acid, you can use the equation Ka H3OA- / HA, where H3O is the concentration of hydronium ions, A- is the concentration of the conjugate base, and HA is the concentration of the acid. The Ka value represents the acid's strength in donating protons in a solution.
