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Afina-wow [57]
3 years ago
5

The student placed 10 mL of PbCl2 (saturated solution) in the test tube and added a pinch of NaCl. A white precipitate of PbCl2

formed. How will this affect the concentration of Pb2+?
Chemistry
1 answer:
zysi [14]3 years ago
6 0

Answer:

Adding NaCl to a saturated PbCl2 solution will decrease the Pb2+ concentration.

Explanation:

If a solution is saturated this means it cannot dissolve more material.  

PbCl2 ⇆ Pb2+ + 2Cl-

Adding more Cl- in the solution is the same thing as trying to dissolve more of the material. In the solution, the concentration of Cl- will increase.

In order for the Ksp to maintain a constant value, the concentration of Pb2+ must decrease if the concentration of Cl- is increased.

Adding NaCl to a saturated PbCl2 solution will decrease the Pb2+ concentration.

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What volume of 0.08892 M HNO3 is required to react completetly with 0.2352 g of potassium hydrogen phosphate?
galina1969 [7]

Answer:

0.0303 Liters

Explanation:

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From the reaction it can be observed that 1 mol of potassium hydrogen phosphate reacts with 2 mol of HNO₃

The number of moles of 0.2352 g of potassium hydrogen phosphate

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