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What is the acid dissociation constant for an acid at equilibrium H?
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What is the acid dissociation constant for an acid at equilibrium HX H X?
The dissociation constant is:k = [H][X]/[HX]
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).
What indicates the ionization constant for an acid?
An acid dissociation constant, Ka, (also known as acidity constant, or acid-ionization constant) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction known as dissociation in the context of acid-base reactions. The equilibrium can be written symbolically as: HA A− + H+,
What is the acid dissociation constant for an acid at equilibrium HX ----- H (spuare Plus) plus x -?
HX ---> H+ + X- Keq = [H+][X-]/[HX]
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 acid dissociation constant for an acid at equilibrium HX - H X-?
The dissociation constant is:k = [H][X]/[HX]
What is the acid dissociation constant for an acid at equilibrium HX H X?
The dissociation constant is:k = [H][X]/[HX]
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).
What indicates the ionization constant for an acid?
An acid dissociation constant, Ka, (also known as acidity constant, or acid-ionization constant) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction known as dissociation in the context of acid-base reactions. The equilibrium can be written symbolically as: HA A− + H+,
What is the acid dissociation constant for an acid at equilibrium HX ----- H (spuare Plus) plus x -?
HX ---> H+ + X- Keq = [H+][X-]/[HX]
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.
How do you derive pH values for weak acids?
Every acid has a constant, called the acid dissociation constant(or Ka), which shows how much the acid dissociates to form ions in water.For an acid, the general dissociation equation is:HA -------> H+ + A-Ka = (concentration of H+) times (concentration of A-) divided by (concentration of HA)The values for concentrations are the values AT EQUILIBRIUM, where the concentrations of all three substances remain the same.If HA was a strong acid, it would completely(or almost completely) ionize in water to form its ions. Therefore, you can say that the concentration of H+ ions in the solution equal the concentration of HA. From this, you can calculate the pH by using the formula pH = - log (H+).If HA was a weak acid, however, things would be different. The acid only partially ionize in water, so you cannot say that the concentration of H+ is equal to the concentration of HA.If you know the value of the acid dissociation constant, you can easily find the concentration of H+ in the solution, and in turn calculate the pH.You know that the amounts of H+ and A- are equal. If you know the concentration of the acid HA you put in, you can calculate the H+ .
Why formic acid is more acidic than acetic acid?
Because it has a greater/higher Ka (dissociation constant). This is related to the ease with which the H+ can be released from the COOH group.
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.
What is the hydrogen-ion concentration if the acid dissociation constant is 0.000 001 and the acid concentration is 0.01 M?
The concentration in such case is calculated including the H ion concentration contributede by water, So the [H] is .00000001+.0000001
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
