Use VSEPR theory to draw structures, with ideal bond angles, for boric acid and the anion it forms when it reacts with water.
1 answer:
According to VSEPR theory, the molecular geometry of boric acid is found to be trigonal planar.
<h3>What is Boric acid? </h3>Boric Acid, which is also known as orthoboric acid, hydrogen borate, boracic acid, is basically a weak acid. It is an acidic hydrate of boric oxide having antifungal, mild, antiseptic and antiviral properties.
<h3>Structure of Boric acid</h3>It has two-dimensional structure, that lies on a plane. According to VSEPR theory, the molecular geometry of boric acid is found to be trigonal planar.
The oxygen atom in both the compounds are sp3 hybridised and ideal bond angle of boric acid is 109°28′.
<h3>Prepartion of boric acid</h3>- Boric acid is prepared by the reaction borax with the mineral acid,
Na2B4O7·10H2O + 2HCl → 4 B(OH)3 + 2 NaCl + 5 H2O
- It can be formed as a by-product of the hydrolysis of boron trihalides and diborane. The reaction is as below:
B2H6 + 6H2O→ 2B(OH)3 + 6H2
BX3 + 3H2O → B(OH)3 + 3HX (X = Cl, Br, I)
<h3>Uses of boric acid</h3>- It is mainly used in the manufacturing of monofilament fibre glass.
- It is also used in the combination along with denatured alcohol in the jewellery industries.
- It is typically used in electroplating.
- It is also used in manufacturing of flat LCD panel displays.
Thus, we concluded that the molecular geometry of boric acid is found to be trigonal planar.
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Answer: The percent yield of the reaction is 74 %
Explanation:
To calculate the number of moles, we use the equation:
.....(1)
For oxygen gas:
The chemical equation for the reaction of titanium and chlorine gas follows:
By Stoichiometry of the reaction:
4 moles of aluminium reacts with 3 moles of oxygen.
So, 0.092 moles of aluminium reacts with = of oxygen
As, given amount of oxygen is more than the required amount. So, it is considered as an excess reagent.
Thus, aluminium is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
4 moles of aluminium produce = 2 moles of
So, 0.092 moles of aluminium will produce = of
Now, calculating the mass of aluminium oxide:
To calculate the percentage yield of titanium (IV) chloride, we use the equation:
Experimental yield = 3.5 g
Theoretical yield = 4.7 g
Putting values in above equation, we get:
Hence, the percent yield of the reaction is 74 %
The answer is in the attachment below:
