Question

ASAP

1) Determine the molarity of a solution fomed by dissolving 97.7 g LiBr in enough e the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution. E) 1.18 M C) 0.768 NM aker contains 0.50 mol of potassium bromide in 600 ml. of water. An additional 600 mI, of C) 0.42 mol A) 0.130 NM B) 2.30 M D) 150 M 2) A beaker contains 0.50 mol of potassium bromide in 600 ml. of water. An addi water is added. The number of moles of potassium bromide in the beaker is A) 0.25 mol B) 0.50 mol D) 0.83 mol E) 1.2 mol 3) If 4.89 g of ZnCl2 is dissolved in enough water to give a total volume of 500 mL, what is the molarity of the solution? A) 1.33 MM B) 0.0717 M C) 0.849 NM D) 0.0179 M E 0.217 M 4) According to the following reaction, how many moles of Fe(OH)2 can form from 175.0 ml. of 0.227 M LiOH solution? Assume that there is excess FeCl2. FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq) A) 5.03 x10-2 moles B) 6.49 x 10-2 moles C) 3.97 x 10-2 moles D) 2.5210-2 moles E) 1.99 x 10-2 moles 5) According to the following reaction, what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution? 2 KCl(aq) + Pb(NO3)2(aq) - PbCl2(s) + 2 KNO3(aq) A) 97.4 mL B) 58.1 ml C) 86.1 mlL D) 43.0 mL E) 116 ml 6) What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 solution? Hint: You will want to write a balanced reaction. A) 345 ml B) 581 ml C) 278 ml. D) 173 ml E) 139 mL 7) The titration of 25.0 ml of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M):? A) 0.36 M B) 0.40 M C) 0.25 M D) 0.20 M E) 0.10 M 8) Determine the oxidation state of P in PO33-. C) 0 D) +3 E) +2 9) Determine the oxidation state of C in CO3-4. A) +2 10) Determine the oxidation state of nitrogen in NO A)+5 D) +3

Answer 1