Your lab group forgot to record the initial volume measurement on the buret and assumed later that it started at 0.00 mL when the actual starting buret reading was 2.00 mL. Would your final calculated molarity of the unknown acid be higher, lower or equal to the actual concentration

Calculated molarity of acid is higher than the actual concentration.

Explanation:

For an acid-base titration, the following equation is obeyed for calculation-

where, C represents concentration and V represents volume.

So,

Here, and are constants.

Actual volume of base added from burette is lesser than the volume used (based on assumption) for calculation of concentration of acid.

So, actual value of is lesser. Hence calculated concentration or molarity of acid is higher than the actual concentration.

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 !

explanation: