How many moles of Mg*2 in 6.00 mL of a 6.0 N Mg3(PO4)2 solution ?First we have to convert moles into equivalentsMg3(PO4)23 Mg*22 PO43+1 mol =equivalents1 mol MP =mol Mg*2eqmol(6.00 x 10-3 L)(-%3Deq MP-) =eqmol Mg*2mol MP)(--) =mol Mg*2mol MPа. 250.b. 100.0С. 2d. 30.00е. 6f. 24g. 3h. 36i. 18.0j. 1k. 6.00 x 10-3I. 3.60 x 10-2m. 6.00 x 10-2n. 5О. 3.0 х 102p. 1.80 x 10-2q. 7.65 x 10-10r. 2.63S. 7.89t. 5.26и. 1012v. 109w. 106Х. 103у. 95.21z. 10

Given, Normality of Mg3(PO4)2 = 6.0 N Volume of Mg3(PO4)2 = 6.00 mL Find number of moles of Mg2+…

How many moles of Mg*2 in 6.00 mL of a 6.0N Mg3(PO4)2 Solution ? First we have to convert moles into equivalents Mg3(PO4)2 3 Mg*2 + 2 PO43 1 mol = equivalents 1 mol MP = mol Mg*2 eq mol (6.00 x 10-3 L)(- eq MP (- eq mol Mg*2 mol MP)(- -) = mol Mg*2 mol MP а. 250. b. 100.0 с. 2 d. 30.00 е. 6 f. 24 g. 3 h. 36 i. 18.0 j. 1 k. 6.00 x 10-3 I. 3.60 x 10-2 m. 6.00 x 10-2 n. 5 o. 3.0 x 10-2 p. 1.80 x 10-2 q. 7.65 x 10-10 r. 2.63 S. 7.89 t. 5.26 u. 1012 V. 109 w. 106 х. 103 у. 95.21 z. 10

How many moles of Mg2 in 6.00 mL of a 6.0N Mg3(PO4)2 Solution ? First we have to convert moles into equivalents Mg3(PO4)2 3 Mg2 + 2 PO43 1 mol = equivalents 1 mol MP = mol Mg2 eq mol (6.00 x 10-3 L)(- eq MP (- eq mol Mg2 mol MP)(- -) = mol Mg*2 mol MP а. 250. b. 100.0 с. 2 d. 30.00 е. 6 f. 24 g. 3 h. 36 i. 18.0 j. 1 k. 6.00 x 10-3 I. 3.60 x 10-2 m. 6.00 x 10-2 n. 5 o. 3.0 x 10-2 p. 1.80 x 10-2 q. 7.65 x 10-10 r. 2.63 S. 7.89 t. 5.26 u. 1012 V. 109 w. 106 х. 103 у. 95.21 z. 10

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 112AP

See similar textbooks

Similar questions

What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.
6-21 Are mixtures of gases true solutions or heterogeneous mixtures? Explain.
D5W is a solution used as an intravenous fluid. It is a 5.0% by mass solution of dextrose (C6H12O6) in water. If the density of D5W is 1.029 g/mL, calculate the molarity of dextrose in the solution.
You want to prepare a 1.0 mol/kg solution of ethyleneglycol, C2H4(OH)2, in water. Calculate the mass of ethylene glycol you would need to mix with 950. g water.
34. For each of the following solutions, the number of moles of solute is given, followed by the total volume of the solution prepared. Calculate the molarity of each solution. a. 0.754 mol KNO; 225 mL b. 0.0105 in of CaCl; 10.2 mL c. 3.15 mol NaCl; 5.00 L d. 0.499 mol NaBr; 100. mL
A solution labeled “0.25 M AICl3” would contain _________ le(s) of Al3+ and mole(s) of Cl- in each liter of e solution.