What mass of HCl, in grams, is required to react with 0.750 g of Al(OH)3 ? What mass of water, i

What mass of HCl, in grams, is required to react with 0.750...

Key Concepts

Molar Mass

Molar mass is the mass of one mole of a substance, usually expressed in grams per mole. It is crucial for converting between mass and the number of moles in stoichiometric calculations.

Stoichiometry

Stoichiometry is the area of chemistry that uses the balanced chemical equation to calculate quantities of reactants and products. It involves converting between grams, moles, and numbers of particles to determine how much of each substance participates in or is produced by a reaction.

Mole Concept

The mole concept is a fundamental principle in chemistry that acts as a bridge between the atomic scale and quantitative measurements. It allows chemists to relate amounts of substances by converting between the number of particles and measurable masses.

Balanced Chemical Equation

A balanced chemical equation represents a reaction where the number of atoms for each element is conserved, and the coefficients indicate the stoichiometric relationships between reactants and products. This is essential for determining the proportionate amounts needed and produced in the reaction.

Transcript

00:01 Hello friends, in this video we will learn how to do some stociometric calculations.

00:07 So as you can see, we have been given an equation.

00:10 So in this equation, aluminum hydroxide reacts with hydrochloric acid to give aluminum chloride and water molecules.

00:22 Right.

00:22 So our question is, we need to find mass of hydrochloric acid required to revert to react with 0 .75 grams of aluminum hydroxide.

00:46 Right.

00:47 So this is our first question.

00:48 So we need to calculate what is the mass of hydrochloric acid in grams required to react with 0 .75 grams of aluminum hydroxide.

00:57 Then the next question is we need to find out mass of water in grams produced during this reaction.

01:11 So basically in reaction a.

01:24 So when you have 0 .75 grams of aluminum hydroxide, how much water is produced? right.

01:34 So these are the two questions we need to find the answers for.

01:41 Okay, so first, before we solve these questions, we need to find what is the molar mass of each of the compounds mentioned here.

01:50 So first one is aluminum hydroxide.

01:52 So you can go to the periodic table and find out the molar mass.

01:57 Of aluminum hydroxide.

01:59 So how do we find the molar mass of aluminum hydroxide? so basically you have to refer to the periodic table and then add up the masses of all the atoms here.

02:13 So we have one atom of aluminum and from the period of table the mass is 27 grams.

02:19 Then there are three oxygen atoms.

02:21 So each oxygen atom the mass is 16 grams and there are three hydrogen atoms.

02:26 So mass for one hydrogen atom is 1 gram.

02:30 So total it will be 27 plus 48 plus 3 which comes to 18 grams.

02:37 Which comes to 78 grams.

02:50 So similarly we can find for hydrochloric as well, hydrochloric acid as well, and then for aluminum chloride as well, and then for water as well.

03:08 Right.

03:09 So for hydrochloric acid it will be 36 .5 grams.

03:14 Per mole then for aluminum chloride it will be 133 .34 grams per mole and for water it will be 18 grams per mole right so from the abhor reaction we can see that so from this equation we can come to know that 78 grams of aluminum hydroxide reacts with 3 into 36 .5 grams of hydrochloric acid to give aluminum chloride with the molar mass is 133 .34 grams and for water is this it is 3 into 18 grams so right so let's solve this so it is 78 grams and here it is 3 into 36 .5 which comes to 109 .5 grams and here it is aluminum chloride is 133 .34 grams and water is 54 grams right so so this is the basic concept we come to know from here like basic equation and like the molar masses we have got from here okay so let's go to the first problem so we need to find out what is the mass of hydrochloric acid required to react with 0 .75 grams of aluminum hydroxide right so this is our first problem first so let's start try solving this.

05:04 So let me write the problem.

05:06 So mass of hydrochloric acid required to react with 0 .75 gram of aluminum hydroxide.

05:29 Right.

05:30 So from this equation we can see that.

05:35 So from this equation above you can see that 78 gram of aluminum hydroxide reacts with how much gram of hydrochloric acid 109 .5 grams of hcl so we have to calculate how much hcl will be required for reacting with 0 .75 grams of aluminum hydroxide okay, so let's do the calculation here.

06:25 So we have got 0 .75 grams of aluminum hydroxide...

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