A solution is prepared by mixing 150.0 ml of 1.0010^-2 m mg(no3)2 and 250.0 ml of 1.0010^-1m naf calculate the concentrations

Question

larisa [96]

3 years ago

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A solution is prepared by mixing 150.0 ml of 1.0010^-2 m mg(no3)2 and 250.0 ml of 1.0010^-1m naf calculate the concentrations

of mg2+ and f at equilibrium with solid mgf2 ksp= 6.4*10^-9

Chemistry

1 answer:

Andreas93 [3] · Answer 1 · 2022-07-18T04:50:23+03:00

First, we have to get moles of Mg2+ = molarity * volume

= 1 x 10^-2 * 0.15 L

= 0.0015 mol

initial [Mg2+] = 0.0015 / 0.4 L(total volume)

= 0.00375 M

then, moles of F- = molarity * volume

= 1 x 10^-1 * 0.25

= 0.025 Mol

initial [F-] = 0.025 / 0.4 = 0.0625 M

by using ICE table:

MgF2(s) → Mg2 + 2F-

initial 0.00375 0.0625

change + X +2 X

Equ 0.00375+X 0.0625+2X

when Ksp = [Mg2+][F-]^2

by substitution:

6.4 x 10^-9 = (0.00375+X)( 0.0625 +2X)^2 by solving for X

∴X= 0.00024 M

∴[Mg2+] = 0.00375 + X

= 0.00375 + 0.00024

= 0.004 M

and [F-] = 0.0625 + 2X

= 0.0625 + 2* 0.00024

= 0.06 M

A solution is prepared by mixing 150.0 ml of 1.00*10^-2 m mg(no3)2 and 250.0 ml of 1.00*10^-1m naf calculate the concentrations

A solution is prepared by mixing 150.0 ml of 1.0010^-2 m mg(no3)2 and 250.0 ml of 1.0010^-1m naf calculate the concentrations