A 10.00-mL sample of 0.254 M H2So4 reacts with 15.00-mL of 0.385 M NaOH according to the reaction H2SO4(aq) + 2NaOH --> 2H20 (l) + Na2SO4 (aq). Which of the following statements is correct? A) There is an excess of 3.24 x 10^ -3 mol of NaOH, B) There is an excess of 3.24 x 10 ^-3 mol of H2SO4, C) There is an excess of 2.19 x 10^-3 mol of H2SO4, D) Neither NaOH nor H2SO4 is present in excess or E) Ther is an excess of 6.95 x 10^-4 mol of NaOH
According to the answer key for my exam, the correct answer is choice E. I put choice A. Where did I mess up?
2006-09-28 14:03:23 · 1 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
Moles of H2SO4 = 0.01L * 0.254 Moles/L = 0.00254
Moles of NaOH = 0.015L * 0.385 Moles/L = 0.005775
2X moles of H2SO4 = 0.00508
Answer = 0.005775 - 0.00508 = 0.000695 moles of NaOH extra
2006-09-28 14:14:27 · answer #1 · answered by feanor 7 · 0⤊ 0⤋