How can I calculate a pH of hypochlorite buffer into LiCLO with only initial concentrations and no Ka value?

[CLO-]=.1M
[LiCLO]=.1M

Are you allowed to look up the value for Ka for HClO? If so that makes it easy. If not that presents a problem but I would do it this way.

pH = pKa + log(base)/(acid)
pH = pKa + log 0.1/0.1
pH = pKa + log 1
pH = pKa + 0
pH = pKa.
I may not have understood the question; you may wish to post the entire problem.

Yes, I can use the Ka of HClO. (hypochlorite ion from hypochlorous)

HClO is a weak acid with a Ka of 2.9*10-8
The pKa = 7.54 (-log of the Ka)
Since the concentration ratio is equal to 1 and the log of 1 is zero, the pH would equal the pKa.

Please verify

right.

To calculate the pH of a hypochlorite buffer containing LiCLO, we first need to determine the concentration of H+ ions in the solution. Since you only have the initial concentrations of [CLO-] and [LiCLO], and no Ka value, we can use the assumption that the hypochlorite buffer dissociates completely.

The chemical reaction for the dissociation of hypochlorite buffer is:
CLO- + H2O ⇌ H+ + CLO2-

Given:
[CLO-] = 0.1 M
[LiCLO] = 0.1 M

Since LiCLO is a salt, it completely dissociates into its ions in water. Therefore, [Li+] = [CLO-] = 0.1 M.

Now, let's focus on the [CLO-] concentration, as it will directly affect the pH.

To determine the concentration of H+ ions, we need to consider the equilibrium expression for the dissociation of the hypochlorite buffer. However, since you don't have the Ka value, we need to find another way to calculate the pH.

One way to estimate the pH is to use the Henderson-Hasselbalch equation, which is applicable to weak acid-buffer systems. The equation is:

pH = pKa + log ([A-] / [HA])

In this case, we will assume CLO- to be the conjugate base (A-) and HClO to be the weak acid (HA).

Since hypochlorous acid (HClO) is the conjugate acid of hypochlorite (CLO-), we can write the following equilibrium equation for their dissociation:

HClO ⇌ H+ + CLO-

From the stoichiometry of the reaction, we can say that the initial concentration of [HA] (HClO) is equal to the initial concentration of [CLO-].

Therefore, [HA] = [CLO-] = 0.1 M.

Now, we need to determine the pKa value of HClO in order to use the Henderson-Hasselbalch equation. The pKa value is a measure of acid strength and can vary depending on temperature and other factors. If you don't have the pKa value, you can look it up in reference books or online databases.

Assuming a pKa value of 7.5 for HClO, we can proceed with the calculation.

pKa = 7.5
[HA] = [CLO-] = 0.1 M

Using the Henderson-Hasselbalch equation:
pH = pKa + log ([A-] / [HA])

pH = 7.5 + log (0.1 / 0.1) = 7.5 + log (1) = 7.5

Therefore, the pH of the hypochlorite buffer containing LiCLO with the given initial concentrations is 7.5.