Question

1. A common mineral in Earth's crust has the chemical composition of 34.55% Mg, 19.96% Si, and 45.49% 0. What is its empirical formula? 2. How many milliliters of 0.100 MHNO, are needed to neutralize the following solution? Write the balanced molecular equation, complete ionic equation, and net ionic equation 58.5 mL of 0.0100 M Al(OH)3 3. a) Balance the following equations. b) Identify oxidizing and reducing agents. c) Determine the oxidation numbers of the elements involved in the redox reaction. Zn (8) + CuSO4 (aq) - 12 (8) + S0,- (aq) - (aq) + S.O.- (aq) 4. Complete and balance the following equations and write the net ionic equations for each. FeCl2 (aq) + NazS (aq) → MgSO4 (aq) + BaCl2 (aq) -

Answer 1

Mole Sipmplest tio may (11 Element f.4y 74.55 .44 24 74.ST 0.21 Mg 19.9 E0.71 Si ৭.৭८ 0.31 29 45.49 5. 49 : २. १४ । : ५ 2: MISiou AlCNe 3t,0 3HNU AI(OHS mm6 ot Al(oH 5xl = 0.585 Mmg mma ot HNa3 0.585 X3 .755 mme volue- SSt.1 74/5.M.t1 (+2)(-2) CUSC4 (+2+-2) D 0.A = RA n Cusau -- 21 t S,DE +2) 2) (9.5) (-2) R-A S203 D. A= Fectzlo4rt FeSitaaC + Na,S(ae tar:) Net lonic Fes4 +Balzlas) Mgch asey Ba4Souan -

A1(02ar) +3HNO3 (09) AICNO +3H204) AI3+ Cag Nos Car H'crs 3NO3 (4 3,) AI OH + HT
rest part of (2) is in 2nd picture.