Question

1. Which of the following compounds in an aqueous solution is a weak acid? A) H2S B) HI C) HBr D) H2SO4 E) HCIO 2. Identify the major ionic species present in an aqueous solution of H2SO4. A) S6, 036-(plus H2O as a neutral species) B) H', OH, 56,302- C) 2H, 56, 402- D) H', HS04 E) 24*, SO42- 3. Which of the following represents an acid-base neutralization reaction? A) 2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g) B) SO2(g) + H2O(l) → H2SO3 (9) C) LiOH(aq) + HNO3(aq) → LINO3(aq) + H2O(1) D) 2KBr(aq) + Cl2(g) → 2Cl(aq) + Brz(1) E) CaBrz(aq) + H2SO4(aq) → CaSO4(s) + 2HBr(g) 4. 34.62 mL of 0.1510 M NaOH was needed to completely neutralize 50.0 mL of H2SO4 solution. What was the concentration of the original sulfuric acid solution? A) 0.0229 M B) 0.218 M C) 0.0523 M D) 0.209 M E) 0.105 M

Answer 1

(1) (A) H₂S weak acid. (B) HI strong acid (c) HBO strong acid D H₂ Soy strong acid E HClOy strong acid O (2) H₂SO4 (aq) → 2H+ + 5042- ( 2H+, sou2- (3) Acid-base neutralization reaction. Acid and a base react to form salt and water. C) LiOH (ag) + HNO3(aq) → Lino, (aq) + H2O16) Base Acid salt --- walls (4) 2 Na Oh Cage) + H2SO4 (aq) + Nasou laq) + 2400 Millimales of NaOH = 2x millimales of H₂SO4 34.62 ml x 0.1510M = 2x M x 50 mL Mr, soy = 34.62 mL X 0.1510M. 2 X 50.0 mL = 0.0523M © 0.0523 Mi