What is the mass of 0.5 g/cm3

Calculate the concentration of so42− ions in a 0.010 m aqueous solution of sulfuric acid. express your answer to four decimal pl

dimulka [17.4K]

Answer: 0.00649M

The question is incomplete,


You are told that the first ionization of the sulfuric acid is complete and the second ionization of the sulfuric acid has a constant Ka₂ = 0.012


With that you can solve the question following these steps"


1) First ionization:


H₂SO₄(aq) --> H⁺ (aq) + HSO₄⁻ (aq)

Under the fully ionization assumption the concentration of HSO4- is the same of the acid = 0.01 M

2) Second ionization


HSO₄⁻ (aq) ⇄ H⁺ + SO₄²⁻ with a Ka₂ = 0.012


Do the mass balance:


 HSO₄⁻ (aq) H⁺ SO₄²⁻

 0.01 M - x x x

Ka₂ = [H⁺] [SO₄²⁻] / [HSO₄⁻]

=> Ka₂ = (x²) / (0.01 - x) = 0.012


3) Solve the equation:

x² = 0.012(0.01 - x) = 0.00012 - 0.012x

x² + 0.012x - 0.0012 = 0


Using the quadratic formula: x = 0.00649


So, the requested concentratioN is [SO₄²⁻] = 0.00649M

4 0

3 years ago

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A salt contains only magnesium and one of the halide ions. A 0.0776-g sample of the salt was dissolved in water, and an excess o

sdas [7]

Answer:

The formula of the magnesium halide is MgF₂

Explanation:

All halides, X, produce a salt with Mg with the formula:

MgX₂

-There are 2 moles of the halide ion per mole of Mg-

With the mass of the MgSO₄ we can find moles of magnesium sulfate = Moles Mg.

With moles of Mg we can know the moles of the halide -1 mole Mg = 2 moles of Halide-

And we can find the mass of Mg in the 0.0776g sample. Subtracting we can find the mass of the halide and, with the mass and moles of the halide we can find its molecular weight and its identity:

Moles MgSO₄ -Molar mass: 120.366g/mol- = Moles Mg:

0.150g * (1mol / 120.366g) = 1.2462x10⁻³ moles Mg

Moles halide:

1.2462x10⁻³ moles Mg * 2 = 2.4924x10⁻³ moles Halide

Mass Mg -Molar mass: 24.305g/mol:

1.2462x10⁻³ moles Mg * (24.305g / mol) = 0.0303g Mg

Mass halide:

0.0776g - 0.0303g Mg = 0.0473g

Molecular weight of the halide:

0.0473g / 2.4924x10⁻³ moles =

18.98g/mol

This molecular weight is the molecular weight of Fluoride ion, F⁻,

<h3>The formula of the magnesium halide is MgF₂</h3>

6 0

3 years ago

Give the oxidation state of the metal species in each complex. ru(cn)(co)4 -

kogti [31]

The given complex ion is as follow,

[Ru (CN) (CO)₄]⁻

Where;
[ ] = Coordination Sphere

Ru = Central Metal Atom = Ruthenium

CN = Cyanide Ligand

CO = Carbonyl Ligand

The charge on Ru is calculated as follow,

Ru + (CN) + (CO)₄ = -1
Where;
-1 = overall charge on sphere

0 = Charge on neutral CO

-1 = Charge on CN

So, Putting values,

Ru + (-1) + (0)₄ = -1

Ru - 1 + 0 = -1

Ru - 1 = -1

Ru = -1 + 1

Ru = 0
Result:
Oxidation state of the metal species in each complex [Ru(CN)(CO)₄]⁻ is zero.

3 0

3 years ago

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Which of the following describes the characteristics of a plasma?

Scorpion4ik [409]

There are essentially 5 states of matter-

1) Solid

2) Liquid

3) Gas

4) Plasma

5) Bose-Einstein Condensate

Plasma comprises of positive and negatively charged particles that are formed in extremely high temperature conditions. A characteristic of plasma is that it is not dense enough. The ions tend to be far apart, which makes them to spread out and imparts compressibility.

Ans B)

7 0

3 years ago

a block of iron has the dimensions of 3.00 cm x 3.00 cm x 3.00 cm. it has a mass of 213 g. what is its density? a. 638 g/cm3 b.

Juliette [100K]

Volume = 3 cm × 3cm × 3cm
= 27 cm ³

Mass = 213 g

Density = $\frac{MASS}{VOLUME}$

= $\frac{213 g}{27 cm ^{3} }$

 = 7.89 g / cm³

Thus answer is D.

8 0

3 years ago

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