30 ml of 0. 00138 m cl- solution is titrated with 0. 00057 m ag+. calculate the pag half-way to the equivalence point when the added titrant volume is 30ml. (hint!: use the ksp value for agcl)

The pAg halfway to the equivalence point when the added titrant volume is 30 ml is 7.45.

The pAg halfway to the equivalence point can be calculated using the concept of stoichiometry and the equilibrium constant expression for the formation of silver chloride (AgCl).

First, we need to determine the number of moles of Cl- present in the initial solution. The initial concentration of Cl- is 0.00138 M, and the volume of the solution is 30 ml. Therefore, the moles of Cl- can be calculated as follows:

Moles of Cl- = Concentration of Cl- × Volume of Solution

            = 0.00138 M × 0.030 L

            = 0.0000414 moles

Since the stoichiometry between Ag+ and Cl- is 1:1, the moles of Ag+ required to react with the moles of Cl- can be assumed to be the same.

Next, we calculate the concentration of Ag+ required to react with the moles of Cl-. The moles of Ag+ can be determined as follows:

Moles of Ag+ = Concentration of Ag+ × Volume of Titrant Added

            = 0.00057 M × 0.030 L

            = 0.0000171 moles

At the halfway point, the moles of Ag+ reacted with the moles of Cl- are equal. Therefore, the moles of Ag+ remaining in solution are:

Moles of Ag+ remaining = Moles of Ag+ initial - Moles of Ag+ reacted

                     = 0.0000171 moles - 0.0000414 moles

                     = -0.0000243 moles

Since the moles of Ag+ cannot be negative, we assume that all the Cl- ions have reacted, and the excess Ag+ ions have formed a precipitate of AgCl.

Using the equilibrium constant expression for AgCl, Ksp = [Ag+][Cl-], we can calculate the concentration of Ag+ at the halfway point.

Ksp = [Ag+][Cl-]

[Ag+] = Ksp / [Cl-]

      = (1.77 × 10^-10) / (0.00138 M)

      ≈ 1.285 × 10^-7 M

Finally, we can calculate the pAg halfway to the equivalence point using the formula:

pAg = -log10([Ag+])

    = -log10(1.285 × 10^-7)

    ≈ 7.45

Step 3: At the halfway point, all the Cl- ions have reacted with Ag+ ions to form AgCl. The remaining Ag+ ions in solution will be in equilibrium with the AgCl precipitate. The concentration of Ag+ at this point can be calculated using the equilibrium constant expression for AgCl.

The pAg halfway to the equivalence point is 7.45. This means that the concentration of Ag+ ions in the solution is approximately 1.285 × 10^-7 M. At this concentration, the solution is close to the solubility product constant (Ksp) for AgCl, which is 1.77 × 10^-10.

The pAg value represents the negative logarithm of the Ag+ concentration in the solution. By calculating the concentration of Ag+ at the halfway point, we can determine the pAg value.

The result indicates that halfway to the equivalence point, the concentration of Ag+ ions in the solution is relatively high, indicating that a significant portion of the AgCl precipitate has formed. This corresponds to the formation of a visible white precip

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