Using your results from the titration what mass of antacid is required to neutralized 25 ml of HCl.

RESULTS: titration: mass of antacid:V of Hcl neutralized :
1:0.31.25.60
2:0.295.32.20
3:0.300.33.20

To determine the mass of antacid required to neutralize 25 mL of HCl, we need to use the mass and volume data from the titration.

From the given results of the titrations, we have the following information:

Titration 1:
Mass of antacid = 0.31 g
Volume of HCl neutralized = 1.25 mL

Titration 2:
Mass of antacid = 0.295 g
Volume of HCl neutralized = 2.20 mL

Titration 3:
Mass of antacid = 0.300 g
Volume of HCl neutralized = 3.20 mL

To find the mass of antacid required to neutralize 25 mL of HCl, we can use proportionality. We can assume that the ratio of mass of antacid to volume of HCl neutralized is constant. So, we can set up a proportion to find the mass of antacid for 25 mL of HCl:

(Mass of antacid 1 / Volume of HCl neutralized 1) = (Mass of antacid 2 / Volume of HCl neutralized 2) = (Mass of antacid 3 / Volume of HCl neutralized 3)

Using the second and third sets of data from the titration:

(0.295 g / 2.20 mL) = (0.300 g / 3.20 mL)

We can solve this proportion to find the constant ratio:

0.295 g * 3.20 mL = 0.300 g * 2.20 mL

0.944 g * mL = 0.660 g * mL

Now, we can set up another proportion to find the mass of antacid required for 25 mL of HCl, using the constant ratio:

(Mass of antacid 2 / Volume of HCl neutralized 2) = (Mass of antacid for 25 mL / 25 mL)

0.295 g / 2.20 mL = (Mass of antacid for 25 mL) / 25 mL

Rearranging the equation to solve for the mass of antacid required:

Mass of antacid for 25 mL = (0.295 g / 2.20 mL) * 25 mL

Mass of antacid for 25 mL = 0.335 g

Therefore, the mass of antacid required to neutralize 25 mL of HCl is approximately 0.335 grams.