are ka and pka the same?
531711
Ka is the acid dissociation constant. pKa is simply the -log of this constant. Similarly, Kb is the base dissociation constant, while pKb is the -log of the constant. The acid and base dissociation constants are usually expressed in terms of moles per liter (mol/L).
793556
If we consider just the phenyl group, it is electron withdrawing by induction(-I effect). This is pretty clear from the pKa values of acetic acid (pKa 4.75) and benzoic acid ( pKa 4.2). However, phenyl group can be either electron donating or electron withdrawing by resonance.
649752
To summarize: Ka * Kb is equivalent to adding the acid and base reactions together, which results in a net equation of the autoionization of water. It's not a neutralization/acid-base reaction, but I think the Kw = Ka * Kb is a mathematical relation made to expedite calculations.
1285040
Acidic and Basic Amino Acids. ... Two amino acids have acidic side chains at neutral pH. These are aspartic acid or aspartate (Asp) and glutamic acid or glutamate (Glu). Their side chains have carboxylic acid groups whose pKa's are low enough to lose protons, becoming negatively charged in the process.
863623
pKa and pKb are the -logs of Ka and Kb; Ka and Kb, when multiplied, are equal to Kw (1.0x10^-14). Kw is also equal to the hydronium and hydroxide concentrations when multiplied.
1233819
Relationship between Ka, pKa and acid strength: The smaller the value of Ka, the larger the value of pKa, the weaker the acid. If the pH of a solution of a weak acid and the pKa are known, the ratio of the concentration of the conjugate base to the concentration of the acid may be calculated.
1332203
Ka and pKa relate to acids, while Kb and pKb deal with bases. Like pH and pOH, these values also account for hydrogen ion or proton concentration (for Ka and pKa) or hydroxide ion concentration (for Kb and pKb). Ka and Kb are related to each other through the ion constant for water, Kw: Kw = Ka x Kb.
813217
The weakest acid has the smallest Ka. In this problem that would be (D) HCN. In general, the more positive the pKa is, the weaker the acid.
826917
So, in this case pH = pKa. Hence, when pH is equal to pKa, the drug is ionized halfly. Ionization of drug effects not only the rate at which the drug permeate membrane but also steady state distribution of drug between the body compartments, if pH difference is present between them.
1067197
Classical PKU is an autosomal recessive disorder, caused by mutations in both alleles of the gene for phenylalanine hydroxylase (PAH), found on chromosome 12. In the body, phenylalanine hydroxylase converts the amino acid phenylalanine to tyrosine, another amino acid.
820856
Understanding Kb and pKb A lower pKb value indicates a stronger base. pKa and pKb are related by the simple relation: pKa + pKb = 14.
199194
Equilibrium constants are sometimes called keq values. If you are experimenting with an acid-base reaction, the keq value is Ka, also known as acidity constant, which measures the strength of an acid in solution.
1097988
Higher pKa indicates weaker the acid. Lower the pKa value stronger the acid is.
364027
pKa is simply the -log of this constant. Similarly, Kb is the base dissociation constant, while pKb is the -log of the constant. The acid and base dissociation constants are usually expressed in terms of moles per liter (mol/L).
344782
Kc and Kp are the equilibrium constants of gaseous mixtures. However, the difference between the two constants is that Kc is defined by molar concentrations, whereas Kp is defined by the partial pressures of the gasses inside a closed system.
261646
The lower the pKa, the stronger the acid and the greater its ability to donate protons. pH depends on the concentration of the solution. This is important because it means a weak acid could actually have a lower pH than a diluted strong acid. ... On the other hand, the pKa value is constant for each type of molecule.
1384343
Strong acids have exceptionally high Ka values. The Ka value is found by looking at the equilibrium constant for the dissociation of the acid. The higher the Ka, the more the acid dissociates. ... In contrast, a weak acid is less likely to ionize and release a hydrogen ion, thus resulting in a less acidic solution.