Which animal resembles their parents already after being born or hatched?

(2 pts) The solubility of InF3 is 4.0 x 10-2 g/100 mL. a) What is the Ksp? Include the chemical equation and Ksp expression. MW

Aleonysh [2.5K]

Answer:

a) Ksp = 7.9x10⁻¹⁰

b) Solubility is 6.31x10⁻⁶M

Explanation:

a) InF₃ in water produce:

InF₃ ⇄ In⁺³ + 3F⁻

And Ksp is defined as:

Ksp = [In⁺³] [F⁻]³

4.0x10⁻²g / 100mL of InF₃ are:

4.0x10⁻²g / 100mL ₓ (1mol / 172g) ₓ (100mL / 0.1L) = 2.3x10⁻³M InF₃. Thus:

[In⁺³] = 2.3x10⁻³M InF₃ × (1 mol In⁺³ / mol InF₃) = 2.3x10⁻³M In⁺³

[F⁻] = 2.3x10⁻³M InF₃ × (3 mol F⁻ / mol InF₃) = 7.0x10⁻³M F⁻

Replacing these values in Ksp formula:

Ksp = [2.3x10⁻³M In⁺³] × [7.0x10⁻³M F⁻]³ = 7.9x10⁻¹⁰

b) 0.05 moles of F⁻ produce solubility of InF₃ decrease to:

7.9x10⁻¹⁰ = [x] [0.05 + 3x]³

Where x are moles of In⁺³ produced from solid InF₃ and 3x are moles of F⁻ produced from the same source. That means x is solubility in mol / L

Solving from x:

x = -0.018 → False solution, there is no negative concentrations.

x = 6.31x10⁻⁶M → Right answer.

Thus, solubility is 6.31x10⁻⁶M

3 0

4 years ago

Sulfur and oxygen react to produce sulfur trioxide. In a particular experiment, 7.9 grams of SO3 are produced by the reaction of

galina1969 [7]

Answer:

$\%\, yield\, \, SO_3=82.29$

Explanation:

First write the balance eqation of chemical reaction:

$2S(s) +3O_2(g) \rightarrow 2SO_3(g)$

Remember writing any chemical reaction from its elemetal form then write the elements in their natural form i.e. how that element exists in the nature here sulphur exists in solid monoatomic form in the nature and oxygen in gaseous diatomic form.

mass of oxygen given=5gram

mole of oxygen $=5/32mol=0.16mol$

mass of sulpher given=6gram

mole of sulpher $=6/32mol=0.19mol$

from the above balanced equaion;

2 mole of sulphur reacts with 3 mole Oxygen completely

1 mole of sulphur reacts with 1.5 mole Oxygen completely

0.19 mole of sulphur reacts with $1.5\times 0.19$ i.e. 0.285 mole Oxygen completely.

but we have 0.16 mole so oxygen will be the limiting reagent and sulpher will be the excess reagent

so product will depend on the limiting reagent

from the balance equation

3 mole of sulpher gives 2 mole $SO_3$

1 mole of sulpher will give 2/3 mole $SO_3$

0.16 of sulpher will give 0.12 mole $SO_3$

mass of $SO_3$ =9.6gram this is theoreical production of $SO_3$

and

actual production of $SO_3$ =7.9gram

$\%\, yield \,\, SO_3=\frac{Actual \,yield}{theoretical\, yield}\times 100$

$\%\, yield\, \, SO_3=\frac{7.9}{9.6} \times 100=82.29$

$\%\, yield\, \, SO_3=82.29$

3 0

3 years ago

Would precipitation occur when 500 mL of a 0.02M solution of AgNO3 is mixed with 500 mL of a 0.001M solution of NaCl? Show your

Oksanka [162]

We know,
AgNO3 + NaCl ⇒ NaNO3 + AgCl(s)
The moles of Na+ present:
0.5 L * 0.001 mol/L
= 5 x 10⁻⁴ mol
Moles of Ag+ present:
0.5 * 0.02
= 0.01 mol
The limiting reactant is Na
Therefore, the moles of Ag reacted:
5 x 10⁻⁴
AgCl is insoluble in water; therefore, the AgCl formed will precipitate

7 0

3 years ago

What is the total number of moles of oxygen atoms present in one mole of Mg(CIO3)2?

Hitman42 [59]

4) 6!!!!!!!!!!!!!!
Nanananabxnjajakaz

8 0

3 years ago

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An unknown amount of helium (He) gas occupies 10.5 L at 1.52 atm pressure and 335 K. What is the mass of helium gas in the conta

Masteriza [31]

Answer:

The lectures in this unit cover gases. This lecture covers the Ideal Gas Law and partial pressures.

Ideal Gas Law

In our previous lecture we discovered a relationship between the pressure, volume, temperature,

and number of moles in gases. After scientists worked out the individual relationships between

pressure, volume, temperature, and the number of moles, it was clear that a single law could

bring all of these individual laws together. This unifying law is called the ideal gas law. An

ideal gas is one which follows the ideal gas law. Not all gases are perfectly ideal in this sense

but most of them are close enough to it that the law applies well.

I. Ideal Gas Law

The Ideal Gas Law unifies all these independent laws as follows:

PV = nRT

Where P = Pressure, V = Volume, T = Temperature, and n = number of moles.

The remaining value, R, is the constant which makes the rest of these factors work together

mathematically. Once the relationship between all individual factors was found it was trivial to

calculate R: it is the value of

PV

nT for any gas since they all act the same way!

There are several numerical values for R depending on which units you are using (atm or torr or

bars, L or mL, Joules (energy) etc). Our class uses this one:

R = .0821

L·atm

mole·K

The ideal gas law helps us calculate variables such as pressure, volume, temperature, or number

of moles without having to make a comparison.

For example, if 3.5 moles O2 has a volume of 27.0 L at a pressure of 1.6 atm, what is the

temperature of the sample?

Here we are given n = 3.5 moles, V = 27.0 L, P = 1.6 atm. We rearrange the ideal gas law to

solve for temperature as follows:

PV = nRT

PV

nR = T

(1.6 atm)(27.0 L)

(3.5 moles)(0.0821 L·atm/mol·K) = 150.3 K

Explanation:

4 0

3 years ago

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