Question

A student prepared a 1:1 buffer, for which [hac] = [ac-] = 0.04797 m. using their 1:1 buffer and a 0.10351 m hcl solution, the student prepared solution c in part 3 of the experimental procedure. given this information, how many moles of hac were there in the student's solution c after a reaction took place?

Answer 1

To calculate the moles of acetic acid (HAc) after reacting with HCl in a buffer solution, we must know the volume of Solution C and assume all HCl reacts completely. Without specific volume information, an exact amount cannot be determined, but the initial molar ratio of HAc to Ac- (1:1) and the concentration of HCl would be used for the calculation.

Step-by-step explanation:

To determine how many moles of HAc (acetic acid) were present in the student's Solution C after the reaction with HCl, we need to consider the reaction between HAc and HCl. When HCl is added to the buffer solution, it reacts with the acetate ion (Ac-) to form HAc and Cl-. Since the buffer solution was a 1:1 mixture of HAc and Ac-, initially, the moles of HAc were equal to the moles of Ac-. After the reaction, the moles of HAc increase by the amount of HCl added, assuming that all the HCl reacted completely.

Without the specific volumes used to prepare Solution C, we cannot accurately calculate the exact amount of HAc after the reaction. However, the general approach would be to use the initial concentration ([HAc] = [Ac-] = 0.04797 M) and the amount of HCl added to calculate the new moles of HAc.