<p> Practice Problems Chpt. 10-13 (Bauer)</p><p>1. Calculate the amount of heat energy required to transform 7.50 g of ice (H2O (s)) O O at 0 C to steam (H2O (g)) at 100.0 C.</p><p>2. Rank the following in order of increasing melting point.</p><p>HF , MgO, H2 , HBr , KBr, </p><p>3. Give the concentrations of all ions in each of the following solutions.</p><p>(a) 0.50 M Co(NO3)2</p><p>(b) 1.0 M FeCl3 </p><p>4. Calculate the number of moles of each ion present in each of the following solutions.</p><p>+ (a) Na ion in 1.00 L of a 0.251 M Na2SO4 solution.</p><p>- (b) Cl ion in 5.50 L of a 0.10 M FeCl3 solution.</p><p>- (c) NO3 ion in 100.0 mL of a 0.55 M barium nitrate solution.</p><p>+ (d) NH4 ion in 250.0 mL of a 0.350 ammonium sulfate solution.</p><p>5. What volume of 3.0 M H2SO4 can be prepared from 100.0 mL of 18.0 M H2SO4?</p><p>6. What volume of 12 M HCl must be used in order to prepare 750 mL of 0.25 M HCl? </p><p>7. When 5.0 L of water is addd to 1.0 L of 6.0 M HCl what is the concentration of the resulting solution? 8. What volume of 0.25 M Na2SO4 is needed to precipitate all of the barium, as barium sulfate, from 12.5 mL of 0.15 M Ba(NO3)2?</p><p>9. Calculate the mass of CaCO3 precipitate produced when 37.5 mL of 0.149 M Na2CO3 is mixed with 36.2 mL of 0.158 M CaCl2.</p><p>10. Molarity is defined as,</p><p>(a) grams of solute per liter of water.</p><p>(b) grams of solute per liter of solution.</p><p>(c) moles of solute per liter of water.</p><p>(d) moles of solute per liter of solution.</p><p>2 11. What mass of K2CrO4 is needed to prepare 5.00 x 10 mL of 0.250 M K2CrO4?</p><p>12. Consider the following reaction.</p><p>PCl5 (g) ⇄ PCl3 (g) + Cl2 (g)</p><p>Suppose that 0.90 mol of PCl5 is placed in a 2.0 L container. Calculate the equilibrium concentrations of all species once equilibrium is attained assuming that K=2.0 x 10-4.</p><p>-6 13. For barium fluoride, Ksp = 1.0 x 10 . Calculate the concentration of fluoride ion in a saturated solution of barium fluoride. Calculate the solubility of barium fluoride in mol/L and in g/L.</p><p>14. In a saturated solution of zinc hydroxide the concentration of zinc ion is -9 7.2 x 10 M. Calculate Ksp for zinc hydroxide. 15. Consider the following reaction.</p><p>N2 (g) + O2 (g)  2 NO (g)</p><p>Suppose that 6.0 mol of N2 and 6.0 mol of O2 are placed in 2.00 L container. Calculate the equilibrium concentrations of all species assuming that K=2.5 x 10-3.</p><p>16. What volume of 1.00 M NaOH is required to titrate 25.0 mL of 0.154 M acetic acid?</p><p>17. Calculate the pH of each of the following solutions.</p><p>-3 (a) 1.00 x 10 M Ba(OH)2</p><p>(b) 3.50 x 10-2 M HCl</p><p>(c) 6.00 M HCl</p><p>-2 18. Calculate the pH of a 1.00 x 10 M HC2H3O2 solution. For acetic acid -5 Ka = 1.8 x 10 .</p><p>19. The pH of a 0.10 M solution of a weak acid is 3.57. Calculate Ka for the acid. </p>