Question

7. Determine the final concentrations of the following diluted solutions: a 92.76 mL of 0.1382 M HCl solution diluted to 250.0 mL 0.1382(92.76)= 250.0(X) 12.819132 = 250.0X 250.0 250.0 (X=0.05128 b. 125 mL of 2.265 M NaOH solution diluted to 0.500 L V2 Vg C 125(2.265)=0.500 (X) 283,925 = asoox X=566.25 8. How much water must be added to 336,0 mL of 0.109 M NaCl solution to obtain a solution that is exactly 0.1000 M? 9. How much water must be added to 0.550 L of 0.109 M MgCl2 solution to obtain a solution that is exactly 0.1000 M? M. Rosen

I’m stuck on how to go about setting up my equations on these two problems. I’ve been looking over my notes and I just keep double guessing myself. I’d be happy with either help on problem 8 or on problem 9.

Answer 1

Solution : 7) a. from relation, M, V = My Va given, M, = Molavity of solution before dilution 0.1282M) VE Volume u n v (92.76 m2) Mz = Molarity of sclation after dilution=? Vzi volumen 12 250.0 mL. Hencs, My = mayo 20:13 82 92.76 My = 0.0512 M 250.0 6. From relation, M, V = My Vz given, M, - Melarity of Nqoh sestation before dilection (2-265m) V = Volume n u = 125 m2 M = Molarity of Maou after dilution = 2 Vze volumen 120.B00L = 500 ML Hence, My M Vi % My = 2.265 x 125 500 M = 0.56625 M