Final answer:
Based on the given 250 ml of a 0.15M CAPS buffer in the basic form, you would need to get 50 ml of 1M HCl from chemical stores to complete the neutralization reaction.
Step-by-step explanation:
Based on the given question, you already have 250 ml of a 0.15M CAPS buffer in the basic form. To determine if you need to get 50 ml of 1M HCl from chemical stores, we need to calculate the reaction between the CAPS buffer and the HCl. Since CAPS is a weak acid, it can react with HCl, which is a strong acid. The reaction will involve the neutralization of the basic form of CAPS (CAPS-) with the protons from HCl.
To calculate if 50 ml of 1M HCl is needed, we need to determine the moles of CAPS buffer present and compare it to the moles of HCl needed for complete neutralization. We can use the equation moles = concentration x volume (in liters) to calculate the moles of each solution.
Let's first calculate the moles of the 0.15M CAPS buffer:
moles of CAPS buffer = 0.15 mol/L x 0.250 L = 0.0375 mol
Next, let's calculate the moles of HCl needed for complete neutralization:
moles of HCl = 1 mol/L x 0.050 L = 0.050 mol
Comparing the moles of CAPS buffer (0.0375 mol) to the moles of HCl needed (0.050 mol), we can see that we don't have enough CAPS buffer to completely neutralize the HCl. Therefore, you would need to get 50 ml of 1M HCl from chemical stores.