How many grams of NaCl are required to precipitate most of the Ag ions from 250

# How many grams of nacl are required to precipitate

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8.How many grams of NaCl are required to precipitate most of the Ag+ions from 2.50 × 102mL of 0.0113 M AgNO3solution? Write the net ionic equation for the reaction. (5 points) 9. What volume of 0.416M Mg(NO 3 ) 2 should be added to 255 mL of 0.102 M KNO 3 to produce a solution with a concentration of 0.278 M NO 3 ions? Assume volumes are additive. (4 points) M1V1 +M2V2= M3V3 (Reference: Chang 4.69) (.832 mol/L)(x) + (.102mol/L)(255 mL)=b(.278mol/L) (255+x) 0.832x + 26.01 = 70.89 + 0.278x .554x = 44.88 X= 81.0L 3 Copyright © 2017 by Thomas Edison State University . All rights reserved. 10.Describe how to prepare 1.00 L of 0.646 MHCl solution, starting with 2.00 MHCl 11. Calculate the volume in mL of a 1.420 M NaOH solution required to titrate the following solutions: (9 points) a. 25.00 mL of a 2.430 M HCl solution Moles HCl = 0.02500 x 2.430 = 0.06075 NaOH= 0.06075 mol / 1.420 M =0.04278 L = 42.78 ml b. 25.00 mL of a 4.500 M H 2 SO 4 solution Moles H2SO4 = 0.02500 x 4.500 = 0.1125 When balanced 2 moles to 1 NaOH. 2 x .1125 = .2250 .2250/1.42 = .1585L = 158.8 ml c. 25.00 mL of a 1.500 M H 3 PO 4 solution Moles H3PO4 = 0.02500 x 1.500 = 0.03750 3 to 1 ratio so, .03750 x 3 = .1125 0.1125 / 1.420 = 0.07923 L = 79.23 mL (Reference: Chang 4.91) 12. A 325 mL sample of solution contains 25.3 g of CaCl 2 . (4 points) a. Calculate the molar concentration of Cl in the solution. 25.3g x (1 mol CaCl2/110.9g CaCl2) x (2 mol Cl-/1 mol CaCl2)=.456 mol Cl- Molarity = mol of sol/ L of sol .456 mol Cl / .325 L = 1.4M Cl b. How many grams of Cl are in 0.100 L of this solution? 1.40m x 35.45g Cl = 49.63g Cl 49.63g Cl x .100 L = 4.96g in .100 L of solution (Reference: Chang 4.148) 13. A student mixes 100.0 mL of 0.500 M AgNO 3 with 100.0 mL of 0.500 M CaCl 2 . (8 points) a. Write the balanced molecular equation for the reaction.  • • • 