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3 years ago

The ksp of tin(ii) hydroxide, sn(oh)2, is 5.45 × 10-27. calculate the molar solubility of this compound.

1 answer:

5 0

Let x be mol/l of Sn(OH)2 that dissolve
Therefore, this will give x mol/l Sn2+ and 2x mol/l OH-
Ksp= (Sn2+)(OH-)^2
= (x)(2x)^2
= 4x^3
4x^3 = 5.45 × 10^-27
x = 1.11 × 10^-9
x = molar solubility = 1.11×10^-9 M

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Answer:

C. Moon, Earth, Jupiter, Sun

Explanation:

Well, the moon is smaller than the Earth so, C is the only logical explanation

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2 years ago

What mass of silver chloride can be produced from 1.65 l of a 0.240 m solution of silver nitrate?

Liono4ka [1.6K]

Check table T and use the concentration equation. Molarity= moles of solute/ liters of solution.

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3 years ago

A 1.00 L sample of a gas at a pressure of 1.000atm is compressed to 0.25 L at a constanttemperature. What is the new pressure of

lord [1]

Answer:

<h3>The answer is 4 atm </h3>

Explanation:

The new pressure can be found by using the formula for Boyle's law which is

$P_1V_1 = P_2V_2$

Since we are finding the new pressure

$P_2 = \frac{P_1V_1}{V_2} \\$

From the question we have

$P_2 = \frac{1 \times 1}{0.25} = \frac{1}{0.25} \\$

We have the final answer as

Hope this helps you

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3 years ago

Please answer the following on the picture<br>ASAP PLZZZ

maxonik [38]

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4 years ago

What is the final volume (L) of a 1.00 L system at 315 K and 1.10 atm if STP conditions are established?

LenaWriter [7]

Answer:

0.95L

Explanation:

Data obtained from the question include:

V1 (initial volume) = 1L

T1 (initial temperature) = 315K

P1 (initial pressure) = 1.10 atm

T2 (final temperature) = stp = 273K

P2 (final pressure) = stp = 1atm

V2 (final volume) =?

Using the general gas equation P1V1/T1 = P2V2/T2, the final volume of the system can be obtained as follow:

P1V1/T1 = P2V2/T2

1.1 x 1/315 = 1 x V2/273

Cross multiply to express in linear form.

315 x V2 = 1.1 x 273

Divide both side by 315

V2 = (1.1 x 273) /315

V2 = 0.95L

Therefore, the final volume of the system if STP conditions are established is 0.95L

5 0

3 years ago