Question

A 25.00 mL solution of 0.03210 M Na2CO3 is titrated with 0.02680

M Ba(NO3)2. Calculate pBa2+ following the addition of the given
volumes of Ba(NO3)2. The Ksp for BaCO3 is 5.0×10^−9.
A 25.00 mL solution of 0.03210 M Na CO2 is titrated with 0.02680 M Ba(NO3)2. Calculate pBa2+ following the addition of the given volumes of Ba(NO3)2. The Ksp for Baco, is 5.0 x 10-9. 11.60 mL pBa2+ =

Answer 1

FiFinal answer:

In order to calculate pBa2+ following the addition of Ba(NO3)2, we need to calculate the moles of BaCO3, square the result to find Qsp, and compare Qsp to Ksp at 25°C.

Step-by-step explanation:

In this scenario, we are presented with a 25.00 mL solution containing 0.03210 M Na2CO3 and 0.02680 M Ba(NO3)2.

The objective is to compute pBa2+ subsequent to the addition of the specified volumes of Ba(NO3)2, considering the given Ksp for BaCO3 as 5.0×10^-9 at 25°C.

To achieve this, the calculation involves determining the moles of BaCO3, squaring the outcome to obtain Qsp, and subsequently comparing Qsp with the given Ksp.

The concentration of Ba2+ ions in solution is pivotal, and the equilibrium constant (Ksp) provides insights into the solubility of BaCO3.

By evaluating the relationship between the calculated Qsp and the established Ksp, one can assess the likelihood of precipitation and gain a quantitative understanding of the system's chemical equilibrium at the specified temperature.

This analytical approach facilitates the prediction of the solution's behavior and the potential formation of solid BaCO3 under the given conditions.

Answer 2

To calculate the pBa2+, you need to determine the concentration of Ba2+ and then take the negative logarithm.

Step-by-step explanation:

In this titration, a solution of Ba(NO3)2 is being added to a solution of Na2CO3. The reaction that occurs is:

Ba2+ + CO32- -> BaCO3

Since the stoichiometric coefficients are equal, the moles of BaCO3 that dissolve will be equal to the moles of Ba2+ formed. To calculate the pBa2+, you need to determine the concentration of Ba2+ and then take the negative logarithm.