A 9.11-g piece of zinc metal is dissolved in 75-mL of 3.5 HCL and hydrogen gas is evolved. The exact amount of 5.0 NaOH needed to neutralize the remaining H+ ions and to precipitate out the Zn 2+ ions as Zn(OH)2 is then added. State the balanced equations for each reaction involved in this process. Discover each equation as an acid/base, a precipitation, or a redox reaction.