pH = pKa + log([A-]/[HA])
pH = pKa+log([conjugate base]/[undissociated acid])
The actual meaning of pKa: the negative log of the dissociation constant, which is a measure of strength of an acid/base
when pKa = pH, there is equal concentration of acid and its conjugate base. pKa helps to understand the nature of acid and base like pH:
pKa 2 but 7 but < 10 -- weak base pKa >10 --strong base
pH is a measure of the concentration of hydronium ions in solution. pKa is a measure of how much an acid wants to dissociate in a solution.
pH has almost no effect on how much a strong acid dissociates. A strong acid added to a mixture drives the pH down by 1 for every 10 times the strong acid concentration goes up (because pH is a log scale--every unit on a log scale represents another power of 10). pH does however have an impact on how much a weak acid dissociates. Of course the pH drops when an acid does dissociate, and weak acids dissociate some, so they are interrelated. An equilibrium is reached. pKa tells you where that equilibrium will be reached and what the final pH will be:
pH = pKa + log([A-]/[HA])
Notice that the only time pH = pKa is when the acid is exactly half dissociated; when [A-] = [HA]. That is the exact point that you want buffer solutions to be. But that's another story.
For buffer solutions the pH and pKa functions are correlated by the following relationship:
pH=pKa+Log([A-]/[HA], in which the second term is defined as conjugated acid [A-] over undissociated acid [HA].
In general , the Henderson- Hasselbach equation is given by:
pH= pKa + log [base]/ [acid]
since the ratio is 1 to 1 : pH = pKa + log 1 , log 1= 0
pH = pKa when the ratio is 1 to 1
one is the concentration of H+, the other is the constant that dictate the ability of a substance to release proton to water
look up relationship of pKa to pH. (Hasselbach equation). Then convert pKb to pKa by the following relationship: 14-pKb=pKa
A simple relation is: pOH = 14 - pH
I will assume you are asking about the pH of pure water if pKw is 14.26. The relationship between pH, pOH, and pKw is as follows: pH + pOH = pKw. If it is pure, neutral water (no acids or bases present), then pH = pOH, so: pH + pOH = 14.26 2(pH) = 14.26 pH = pOH = 7.13
The pOH is 6,4.
The pOH is 6,4.
pOH +pH=14 pOH+7.6=14 pOH=(14-7.6)=6.4
pH and pOH are a measure of the concentration of the hydronium ions and hydroxyl ions respectively in the solution. pH = -log[H+] pOH = -log[OH-] and they are related: pH + pOH = 14
I will assume you are asking about the pH of pure water if pKw is 14.26. The relationship between pH, pOH, and pKw is as follows: pH + pOH = pKw. If it is pure, neutral water (no acids or bases present), then pH = pOH, so: pH + pOH = 14.26 2(pH) = 14.26 pH = pOH = 7.13
We can subtract pOH from 14, using the formula pH + pOH = 14. This is only true at 14 degrees Celsius.
pH + pOH =14
The pOH is 6,4.
The pOH is 6,4.
It will have a pOH of 12. Because pH+pOH=14
pH is -log[H(subscript 3)O+] pOH is the [OH-] pOH = 14 - pH apex
pH + pOH =14
pOH +pH=14 pOH+7.6=14 pOH=(14-7.6)=6.4
pH and pOH are a measure of the concentration of the hydronium ions and hydroxyl ions respectively in the solution. pH = -log[H+] pOH = -log[OH-] and they are related: pH + pOH = 14
1.8
pOH is the negative log of the OH- concentration. It is also related to pH by pH + pOH = 14.