What is the mass of NaCl that is present in the \'Unknown NaCl\' solution? Pleas

Question

What is the mass of NaCl that is present in the 'Unknown NaCl' solution? Please provide explination

Below is some information

The Ksp for Silver Chloride is: 1.830e-10.

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Thanks for your help!!

Burent reading AgCl(aq) mL V tot NaCl [Ag+] M 0.5 100.5 6.68E-11 1 101.5 6.75E-11 1.5 103 6.85E-11 2 105 6.98E-11 2.5 107.5 7.14E-11 3 110.5 7.34E-11 3.5 114 7.58E-11 4 118 7.84E-11 4.5 122.5 8.14E-11 5 127.5 8.47E-11 5.5 133 8.84E-11 6 139 9.24E-11 6.5 145.5 9.67E-11

Explanation / Answer

You are allowed to determine the [Ag+] in the solution.
Now consider a saturated solution of AgCl only.
You know that Ksp AgCl = 1.830*10^-10
Ksp = [Ag+][Cl-]
[Ag+] [Cl-] = 1.83*10^-10
[Ag+] = [Cl-] = ?(1.83*10^-10 = 1.35*10^-5 M

From our analysis we found that [Ag+] in solution was 9.67E-11M

But [Ag+] [Cl-] = 1.83*10^-10
If [Ag+] = 9.67E-11M , solve for [Cl-]

[Cl-] = (1.83*10^-10) / ( 9.67E-11M )

[Cl-] = 1.89 M That is the total Cl- in solution

You know that the AgCl is contribution   9.67E-11M as Cl- ( because [Ag+] = [Cl-] from AgCl

Therefore the concentration of Cl- from the NaCl =1.89 M - (9.67E-11M ) =1.89M

And [NaCl] in solution = 1.89M

so mass of NaCl= 1.89 x .1 x 58.5

=11.07 gm ANS

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