HA ==> H+ + A-Ka = [H+][A-][HA] and from pH = 2.31, calculated [H+] = 4.89x10^-3 M
Ka = (4.89x10^-3)(4.89x10^-3)/0.012
Ka = 1.99x10^-3
pKa = 2.70
A pKa value is a measurement used for bases and acids. The measurement pH applies to hydronium ion concentrations that are in a solution, whereas pKa only applies to determining the amount of dissociation an acid wants to do in a solution.
the pH of ethanol can be calculated using its pKa value (pKa 15.9) and the Henderson-Hasselbalch equation. pH = pKa - log [AH/A] where [AH/A] the ratio of disassociated versus undisassociated species in solution.
This question does not make very much sense but it will somewhat be answered. PH is the measurement of a concentration of hydronium ions in a solution. PKA is the measurement of how much is available. If the concentration and pka of a substance is known, the pH can be calculated.
pKa= pH - log(A/HA) to clarify -log is subtract log E.g A buffer is prepared by adding .15 M of NaOH and .1 of a weak acid, HA. If the pH of the buffer is 8.15, what is the pKa of the acid? pH= 8.15 - log .15/.1 = 7.97
It is the most effective when it is at pH=pKa of its weak acid component.
HA ==> H+ + A-Ka = [H+][A-][HA] and from pH = 2.31, calculated [H+] = 4.89x10^-3 M Ka = (4.89x10^-3)(4.89x10^-3)/0.012 Ka = 1.99x10^-3 pKa = 2.70
A pKa value is a measurement used for bases and acids. The measurement pH applies to hydronium ion concentrations that are in a solution, whereas pKa only applies to determining the amount of dissociation an acid wants to do in a solution.
the pH of ethanol can be calculated using its pKa value (pKa 15.9) and the Henderson-Hasselbalch equation. pH = pKa - log [AH/A] where [AH/A] the ratio of disassociated versus undisassociated species in solution.
This question does not make very much sense but it will somewhat be answered. PH is the measurement of a concentration of hydronium ions in a solution. PKA is the measurement of how much is available. If the concentration and pka of a substance is known, the pH can be calculated.
pKa= pH - log(A/HA) to clarify -log is subtract log E.g A buffer is prepared by adding .15 M of NaOH and .1 of a weak acid, HA. If the pH of the buffer is 8.15, what is the pKa of the acid? pH= 8.15 - log .15/.1 = 7.97
Its an equation you can use to find the pH of a solution. it is.... --- pH = pKa + log (Base/Acid) --- these may help too Ka = 10^-pKa Kw = Ka*Kb
The buffer capacity increases as the concentration of the buffer solution increases and is a maximum when the pH is equal to the same value as the pKa of the weak acid in the buffer. A buffer solution is a good buffer in the pH range that is + or - 1 pH unit of the pKa. Beyond that, buffering capacity is minimal.
It is the most effective when it is at pH=pKa of its weak acid component.
The ph. for this 1M Na2C4H2O4 solution can be found using the kA and the equation pH = pKa + log([base]/[acid]) This salt Na2C4H2O4 is going to increase the concentration of base in the solution.
How can you calculate pka valve if ph is given?
Ka = [H+][A-] / [HA] Hence [H+] = Ka[HA] / [A-] Remember pH = -log(10)[H+] 'logging' both sides. -log(10)[H+] = - log(10)Ka[HA] / [A-] By algebraic manipulation of log. pH = -log[A-]^-1 - logKa - log[HA] pH = log[A-] - logKa - log[HA] pH = pKa - log[HA]/[A-]
At 'half way' point the pH is equal to the pKa value of the acid: pH = pKa - log[cA/cB] because at that point cA = cB . So pH = pKa = - log(5.2*10-6) = 5.3