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2 years ago

_____ occurs when the product of the ion concentrations exceeds the Ksp.

Chemistry

2 answers:

arlik [135]2 years ago

4 0

Precipitation occurs when the product of the ion concentration exceeds the Ksp.

serious [3.7K]2 years ago

4 0

Answer : Precipitation occurs when the product of the ion concentrations exceeds the $K__{sp}$ .

Explanation :

Ionic product : It is the product of the concentrations of the ions in solution raised to the same power by its stoichiometric coefficient in a solution of a salt. This takes place at any concentration. The ionic product is represented as, Q.

Solubility product constant : It is defined as the product of the concentration of the ions present in a solution raised to the power by its stoichiometric coefficient in a solution of a salt. This takes place at equilibrium only. The solubility product constant is represented as, $K__{sp}$ .

There are three cases for the solubility :

When $Q$ this means that the solution is unsaturated solution and more solid will be dissolve.
When $Q=k_{sp}$ this means that the solution is saturated solution.
When $Q>k_{sp}$ this means that the solution is supersaturated solution and solid will be precipitate.

Hence, the precipitation occurs when the product of the ion concentrations exceeds the $K__{sp}$ .

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For the reaction N2(g) + 2H2(g) → N2H4(l), if the percent yield for this reaction is 100.0%, what is the actual mass of hydrazin

barxatty [35]

Answer:

53.6 g of N₂H₄

Explanation:

The begining is in the reaction:

N₂(g) + 2H₂(g) → N₂H₄(l)

We determine the moles of each reactant:

59.20 g / 28.01 g/mol = 2.11 moles of nitrogen

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1 mol of N₂ react to 2 moles of H₂

Our 2.11 moles of N₂ may react to (2.11 . 2) /1 = 4.22 moles of H₂, but we only have 3.35 moles. The hydrogen is the limiting reactant.

2 moles of H₂ produce at 100 % yield, 1 mol of hydrazine

Then, 3.35 moles, may produce (3.35 . 1)/2 = 1.67 moles of N₂H₄

Let's convert the moles to mass:

1.67 mol . 32.05 g/mol = 53.6 g

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3 years ago

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Explanation:

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Answer:

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3 years ago

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Answer:

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2 years ago

Read 2 more answers

A. At STP, what is the volume of 708 mol of nitrogen gas? 708 mol = 708 mol X L B. A sample of hydrogen gas occupies 14.1 L at S

elena-14-01-66 [18.8K]

Answer:

A. 15859.2 L or 15900 L

B. 0.629 mol

Explanation:

At STP, one mole is equal to approximately 22.4 L

L or mL is volume, so you are attempting to solve for L or mL.

708 mol x (22.4 L/1 mol) = 15859.2 L (w/ significant figures included - 15900 L)

(14.1 L) x (1 mole/ 22.4 L) = 0.629 mol.

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2 years ago