The total volume required to reach the endpoint of a titration required more than the 50 ml total volume of the buret. an initial volume of 49.16±0.06 ml was delivered, the buret was refilled, and an additional 1.69±0.04 ml was delivered before the endpoint was reached. the titration of a blank solution without the analyte required 0.33±0.04 ml . calculate the endpoint volume corrected for the blank and its absolute uncertainty. note: significant figures are graded for this problem. to avoid rounding errors, do not round your answers until the very end of your calculations.

The endpoint volume is 50.52 ±  0.14 mL

Explanation:

In a titration always is necessary to subtract the blank volume to the titrant volume to obtain the real volume of the titrant. Thus in this case, the total endpoint volume is the sum of the initial volume delivered and the second volume delivered, minus the blank volume:

V = (49.16±0.06 mL) + (1.69±0.04 mL) - (0.33±0.04 mL)

V = (49.16 + 1.69 - 0.33) ± (0.06+0.04+0.04) mL

V = 50.52 ±  0.14 mL

It is necessary to consider the sum of the errors too.

a force of 500                  

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !