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Question

An aqueous solution that has 58.5% (w/v) NaCl and 5 M MgCl2 has a density of 1.949 gm/mL. Mark the option(s) which represent the correct molarity or relation of the specified ion(s). (Assume 100% dissociation of each salt)


A
[Cl]=20 M
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B
[Mg2+]=10 M
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C
[All the cations] = 15 M
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D
[All the anions][All the cations]=43
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Solution

The correct options are
A [Cl]=20 M
C [All the cations] = 15 M
D [All the anions][All the cations]=43
Let's take 1 L of solution.
Mass of NaCl = 585 gm , moles of NaCl = 10 mol
Moles of Na+=10 mol and moles of Cl=10 mol due to NaCl.
Now, in 1 L solution of 5M MgCl2 ,
moles of Mg2+=5 moles and moles of Cl=10 mol
So, [Cl]=10+101 =20 M,[Na+]=101 =10 M,[Mg2+]=51 =5 M
[cations] = 10 + 5 = 15
[All the anions][All the cations]=2010+5=43

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