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3 years ago

What is the chemical reaction for Mg + NaOH also with the ionic equations and subscripts?

1 answer:

3 0

<span>The chemical reaction for Mg + NaOH is

Mg (s) + NaOH (aq) -> Mg (OH)2 (s) + Na (aq)
s stands for solid, aq stands for aqueous</span>

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ompare your TLC analysis with the results of the column chromatography. More polar molecules move more slowly through silica tha

Assoli18 [71]

Biphenyl will have a higher R value than the Methyl Orange.

Explanation:

Biphenyl is a aromatic hydrocarbon and it is a nonpolar molecule.

Methyl Orange is a organic compound with a -SO₃⁻Na⁺ polar functional group which will induce a high polarity in the compound.

You may find the chemical structures of both molecules in the attached picture.

Column chromatography, which use as stationary phase silica gel, is a good technique for separation of the Methyl Orange from Biphenyl.

Being a non-polar molecule, Biphenyl will have a higher R value than the Methyl Orange.

To separate them you use a appropriate solvent as eluent, as exemple chloroform, and Biphenyl will elute first from the column and after that, as a separate phase, Methyl Orange will elute thus separating them.

Learn more about:

chromatography

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7 0

3 years ago

The following exothermic reaction is allowed to reach equilibrium. What

Anon25 [30]

The answer is gonna be the last one :)

5 0

3 years ago

Laura sees a horse pulling a buggy.

Tcecarenko [31]

Answer:

Explanation:

I think that the anserw is B.

4 0

2 years ago

Alum is a compound used in a variety of applications including cosmetics, water purification, and as a food additive. It can be

vlabodo [156]

Answer:

The theoretical yield of alum is 19.873 grams and percent yield for this alum synthesis is 45.33%.

Explanation:

Mass of bottle = 10.221 g

Mass of bottle with aluminium pieces = 11.353 g

Mass of aluminium = 11.353 g - 10.221 g = 1.132 g

Mass of alum and bottle = 19.230 g

Mass of alum = 19.230 g - 10.221 g = 9.009 g

Experimental yield of alum = 9.009 g

Theoretical yield of alum:

$2Al(s) +2 KOH(aq) +4H_2SO_4(aq)+10 H_2O(l) \rightarrow 2 KAl(SO_4)_2.12 H_2O(s)+3H_2(g)$

Moles of aluminium = $\frac{1.132 g}{27 g/mol}=0.041926 mol$

According to reaction, 2 moles of aluminum gives 2 moles of alum.

Then 0.041926 mol aluminium will give :

$\frac{2}{2}\times 0.041926 mol=0.041926 mol$ of alum.

Mass of 0.041926 moles of alum:

0.041926 mol × 474 g/mol= 19.873 g

Theoretical yield of alum = 19.873 g

Percentage yield:

$\% Yield =\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100$

Percentage yield of the alum:

$\% Yield =\frac{ 9.009 g}{19.873 g}\times 100=45.33\%$

The theoretical yield of alum is 19.873 grams and percent yield for this alum synthesis is 45.33%.

7 0

3 years ago

You have 47.0 mL of a 2.00 M concentrated or "stock" solution that must be diluted to 0.500 M. How much water should you add?

Inessa [10]

The required volume of water to make the dilute solution of 0.5 M is 188 mL.

<h3>How do we calculate the required volume?</h3>

Required volume of water to dilute the stock solution will be calculated by using the below equation as:

M₁V₁ = M₂V₂, where

M₁ & V₁ are the molarity and volume of stock solution.
M₂ & V₂ are the molarity and volume of dilute solution.

On putting values from the question to the above equation, we get

V₂ = (2)(47) / (0.5) = 188mL

Hence required volume of water is 188 mL.

To know more about volume & concentration, visit the below link:
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6 0

2 years ago