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Ka = [H+].[Br-] / [HBr]
However the value of this expression is very high, because HBr is a STRONG acid, meaning that much more than 99.9% of the HBr molecules in water are protolized (ionized), making [H+] and [Br-] equal to the original (added) HBr amount, and the [HBr]-value nearly zero.
Wiki User
∙ 12y ago
Wiki User
∙ 13y agoKa={ [H+] [Br-] }/ [HBr]
Which turns into
Ka= x2/ ([HBr] - x)
[HBr] = initial concentration of HBr
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The acid dissociation constant for an acid dissolved in water is equal to?
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).
Prove that Kw equals product of Ka and Kb for an acid-base pair in water?
dissociation of acid in water: A + H2O <-> A- + H3O+ with dissociation constant Ka = [A-][H3O+]/[A][H2O] = [A-][H3O+]/[A]. dissociation of base in water: B + H2O <-> HB+ + OH- with dissociation constant Kb = [HB+][OH-]/[B][H2O] = [HB+][OH-]/[B] dissociation of water in itself: 2H2O <-> H3O+ + OH- with dissociation constant Kw = [H3O+][OH-]/[H2O]^2 = [H3O+][OH-] where [H2O] has been ommitted because it is a pure liquid. substituting relations for Ka and Kb into Kw gives: Kw = [H3O+][OH-] = (Ka[A]/[A-])(Kb[B]/[HB+]) = KaKb where [A] = [HB+] and [B] = [A-].
Why does a larger Ka mean a stronger acid?
A larger Ka indicates that the acid will more readily react as the molecular bonds are relatively weak. The Ka is known as the dissociation constant.
What is the dissociation constant for benzoic acid?
Ka for benzoic acid is 6.46 x 10-5.
What is the concentration of undissociated acid if the hydrogen-ion concentration is 0.0001 M and the acid dissociation constant is 0.0000001?
The equation is acid + water equalizes into hydronium and conjugate base, and Ka (acid dissociation constant) is products divided by reactants. If the Acid = (H+)(base)/Ka, then the acid concentration is (H+)(H+)/Ka, or (0.0001)(0.0001)/0.0000001, which equals 1M.
The abbreviation Ka represents?
acid dissociation constant
What does the abbreviation Ka represent?
Acid dissociation constant
The acid dissociation constant for an acid dissolved in water is equal to?
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).
Prove that Kw equals product of Ka and Kb for an acid-base pair in water?
dissociation of acid in water: A + H2O <-> A- + H3O+ with dissociation constant Ka = [A-][H3O+]/[A][H2O] = [A-][H3O+]/[A]. dissociation of base in water: B + H2O <-> HB+ + OH- with dissociation constant Kb = [HB+][OH-]/[B][H2O] = [HB+][OH-]/[B] dissociation of water in itself: 2H2O <-> H3O+ + OH- with dissociation constant Kw = [H3O+][OH-]/[H2O]^2 = [H3O+][OH-] where [H2O] has been ommitted because it is a pure liquid. substituting relations for Ka and Kb into Kw gives: Kw = [H3O+][OH-] = (Ka[A]/[A-])(Kb[B]/[HB+]) = KaKb where [A] = [HB+] and [B] = [A-].
Why does a larger Ka mean a stronger acid?
A larger Ka indicates that the acid will more readily react as the molecular bonds are relatively weak. The Ka is known as the dissociation constant.
What is the dissociation constant for benzoic acid?
Ka for benzoic acid is 6.46 x 10-5.
What is the equation for the acid dissociation constant Ka of carbonic acid?
H2CO3---------- 2 H+ + (CO3)2-
What is the concentration of undissociated acid if the hydrogen-ion concentration is 0.0001 M and the acid dissociation constant is 0.0000001?
The equation is acid + water equalizes into hydronium and conjugate base, and Ka (acid dissociation constant) is products divided by reactants. If the Acid = (H+)(base)/Ka, then the acid concentration is (H+)(H+)/Ka, or (0.0001)(0.0001)/0.0000001, which equals 1M.
What is the pH of fluorosulfuric acid?
The pKa of the fluorosulfuric acid is -10; HSO3F is a very strong acid, a so-called superacid. Ka is the dissociation constant; pKa is the decimal logarithm of Ka.
Why is acetic weaker than hydrochloric acid?
The strength of the acid depends on the amount of hydrogen ions which come from the dissociation of the acid. Hydrochloric acid (HCl) splits entirely into ions: H+ and Cl-, due to a large acid dissociation constant (Ka). Ka of an acetic acid is relatively small (10-4.8). That means that lots of molecules stays undissociated and do not produce H+ ions.
How do you write sets?
kpay ka
What is the Henderson-Hasselbalch equation?
Note- See the related link for the complete derivation belowSUMMARY OF ACID-DISSOCIATION CONSTANT (pKa) (from Rhoades and Pflanzer Human Physiology)HA ßà H+ + A-1) Reaction to the right à dissociation reaction2) Reaction to left à association reactionThe rate of the dissociation reaction = [HA] x dissociation rate constant k1 (which is a specific value for this reaction).The rate of the association reaction = [H+] x [A-] x association rate constant k2At equilibrium à rates of association and dissociation are =. Thereforek1 x [HA] = k2 x [H+] x [A-]Hence à [H+] x [A-] /[HA] = k1/k2A NEW CONSTANT à is defined for k1/k2 à we call it Ka (equilibrium constant for the reaction and dissociation constant for the acid)A HIGHER Ka à more completely an acid is dissociated à stronger acid à lower pHA LOWER Ka à not as much dissociation à weak acid à higher pHThe Ka is often small in difficult to manipulate à so we present the number in a logarithmic form à pKa (which is the log10 of the INVERSE of KapKa = log10(1/Ka) = --log10(Ka)LOW pKaà high dissociation constant à STRONG ACIDHIGH pKa à low dissociation constant à WEAK ACIDTHE HENDERSON HASSELBALCH EQUATION[H+] x [A-] /[HA] = Ka à therefore[H+] = Ka x [HA] / [A-]Take log of both sidelog[H+] = logKa + log([HA]/[A-]) à multiple both sides by -1-- log[H+] = --logKa + log([A-]/[HA])And because pH = --log[H+] and pKa = log(1/Ka) = --log(Ka)pH = pKa + log([A-]/[HA])HENCE à WHEN [A-] = [HA] à the pH of solution = it's pKa (because the log1 is 0)Conversely à the pKa is the pH at which there are as many molecules of weak acid as there are conjugate base in solution.For the bicarbonate buffer system à (pK = 6.1)Cheers
