Observing the Solubility of Sodium Chloride 1.) Write the dissolution reaction a

Question

Observing the Solubility of Sodium Chloride

1.) Write the dissolution reaction and solubility product expression (Ksp equation) for each of the following solids:

a. BaCl2

Ksp equation:

dissolution reaction:

b. Na3PO4

Ksp equation:

dissolution reaction:

2.) The reported solubility of NaCl is 359 g/L in water. Convert this to moles/L.

3.) What is the solubility product constant expression (the Ksp equation) for NaCl?

4.) Using the solubility of NaCl (see question 2), calculate the Ksp for sodium chloride. You will need this for your post-lab – be sure to write it there before turning this in!

5.) Is the solubility of the salt in each of the following systems greater, less, or unaffected by the indicated change? To obtain credit, you must also explain your answer.

a. Dissolving calcium chloride in a solution containing 1.0 M calcium nitrate:

b. Dissolving calcium chloride in a solution containing 1.0 M barium nitrate:

c. Dissolving calcium chloride in a solution containing 1.0 M barium chloride:

Explanation / Answer

1.) Write the dissolution reaction and solubility product expression (Ksp equation) for each of the following solids:

a. BaCl2

Ksp equation:

Ksp = [Ba+2][Cl-]^2

dissolution reaction:

BaCl2(s) <--> Ba+2(aq) + 2Cl-(aq)

b. Na3PO4

Ksp equation:

Ksp = [Na+]^3[PO4-3]

dissolution reaction:

Na3PO4 <--> 3Na+(aq) + PO4-3(aq)

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