1. (9) An impure 18.540g sample of a weak base of a metal hydroxide, M(OH)), is 62.08% M(OH), by mass. The sample is added to 625.0mL of 0.2800M sulfuric acid (H. SO.). The resulting solution is acidic is then neutralized
with 238.2mL of 0.1130M NaOH.
a) What is the mass of M(OH), in the original sample? (1 pt)
b) Assuming that the M(OH), is the only substance that reacts with the acid, determine the moles of M(OH),
present in the original sample (5 pts).
c) Determine the identity of the metal (3 pts).

b) Assuming that the M(OH), is the only substance that reacts with the acid, determine the moles of M(OH),

present in the original sample (5 pts).

Explanation:

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.