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12 Dec 2019

What is the cobalt (II) ion concentration in a solution prepared by mixing 385 mL of 0.380 M cobalt (II) nitrate with 417 mL of 0.279 M sodium hydroxide? The Ksp of cobalt (II) hydroxide is 1.3 × 10-15

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Irving Heathcote
Irving HeathcoteLv2
13 Dec 2019

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Related questions

A solution contains 1.13×10-2 M sodium carbonate and 1.18×10-2 M ammonium sulfide.
Solid cobalt(II) nitrate is added slowly to this mixture.

A. What is the formula of the substance that precipitates first?

formula =




B. What is the concentration of cobalt(II) ion when this precipitation first begins?
[Co2+] = ______ M

1.An aqueous solution of cobalt(II) nitrate has a concentration of 0.322 molal.

The percent by mass of cobalt(II) nitrate in the solution is ___ %.

2.
An aqueous solution of sodium sulfide has a concentration of 0.417 molal.

The percent by mass of sodium sulfide in the solution is _____ %.

3.
An aqueous solution is 40.0% by mass silver nitrate, AgNO3, and has a density of 1.47 g/mL.

The molality of silver nitrate in the solution is ____m.

I did the following two calculations:

Calculation of concentration (M) of 1 mL of cobalt (II) in diluted solution with 9 mL of deionized water

C1*V1 = C2*V2 (I)
0.1 M cobalt * 0.001 L cobalt = C2 * 0.01 L
C2 = (0.1 M * 0.001 L)/0.01 L = 0.01 M

Calculation of concentration (M) of unknown sample
Y = mx + b = 3.43x - 0.0094 (II)
X = (y-b)/m = (0.22+0.0094)/3.43 = 0.067 M

And I cannot figure out the final calculation:

Calculation of mg of cobalt in 1 kg of soil
M = moles/volume

I've attached a picture that could provide further context.

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