Find the volume of 0.110 M hydrochloric acid necessary to react completely with 1.54 Al(OH)3.

Please explain how to do this.

Here is a worked example of a stoichiometry problem. Just follow the steps.

http://www.jiskha.com/science/chemistry/stoichiometry.html

Oh, I'd be happy to explain, but first let me put on my lab coat and clown nose!

To find the volume of hydrochloric acid necessary to react completely with aluminum hydroxide (Al(OH)3), we need to use the balanced chemical equation and a little stoichiometry.

The balanced equation for the reaction between hydrochloric acid (HCl) and aluminum hydroxide is:

3HCl + Al(OH)3 -> AlCl3 + 3H2O

From the equation, we can see that 3 moles of HCl react with 1 mole of Al(OH)3 to produce 1 mole of AlCl3 and 3 moles of water.

Now, we need to convert the given concentration of hydrochloric acid (0.110 M) to moles. This can be done using the formula:

moles = concentration (M) x volume (L)

Since we are trying to find the volume, we rearrange the formula to:

volume (L) = moles / concentration (M)

For our reaction, we know that 3 moles of HCl react with 1 mole of Al(OH)3. Therefore, the number of moles of HCl needed is given by:

moles of HCl = (moles of Al(OH)3) x (3 moles HCl / 1 mole Al(OH)3)

Given that we have 1.54 moles of Al(OH)3, we can substitute this value into the equation:

moles of HCl = 1.54 moles Al(OH)3 x (3 moles HCl / 1 mole Al(OH)3)

Simplifying the equation, we find:

moles of HCl = 4.62 moles HCl

Now that we have the number of moles of HCl, we can calculate the volume using the formula:

volume (L) = moles / concentration

Using the given concentration of 0.110 M, we substitute the values:

volume (L) = 4.62 moles HCl / 0.110 M

Calculating this, we get:

volume (L) = 42 L

So, the volume of 0.110 M hydrochloric acid necessary to react completely with 1.54 moles of aluminum hydroxide is approximately 42 liters.

Now, wasn't stoichiometry a "fun reaction" to complete?

To find the volume of hydrochloric acid necessary to react completely with 1.54 Al(OH)3, we need to use the balanced chemical equation for the reaction.

The balanced equation for the reaction between hydrochloric acid (HCl) and aluminum hydroxide (Al(OH)3) is:

3HCl + Al(OH)3 -> AlCl3 + 3H2O

This equation tells us that 3 moles of hydrochloric acid will react with 1 mole of aluminum hydroxide to produce 1 mole of aluminum chloride and 3 moles of water.

Since we are given the concentration of hydrochloric acid, which is 0.110 M (moles per liter), we can use this information to find the number of moles of hydrochloric acid needed to react completely with 1.54 moles of aluminum hydroxide.

To do this, we can use the equation:

moles = concentration x volume

Rearranging the equation, we have:

volume = moles / concentration

First, let's calculate the number of moles of aluminum hydroxide:

moles of Al(OH)3 = mass / molar mass

If we have the mass of aluminum hydroxide, we can calculate the number of moles. Let's assume the mass of Al(OH)3 is given in the problem.

Once we have the moles of aluminum hydroxide, we can use the stoichiometry of the balanced equation. Since the stoichiometric ratio between hydrochloric acid and aluminum hydroxide is 3:1, we can multiply the moles of aluminum hydroxide by 3 to get the moles of hydrochloric acid required.

Finally, we can plug the moles of hydrochloric acid and the concentration into the equation to find the volume:

volume = moles / concentration

This will give us the volume of 0.110 M hydrochloric acid necessary to react completely with 1.54 moles of aluminum hydroxide.

To find the volume of hydrochloric acid necessary to react completely with Al(OH)3, we need to use the balanced chemical equation for the reaction between hydrochloric acid (HCl) and aluminum hydroxide (Al(OH)3).

The balanced chemical equation for the reaction is:
3HCl + Al(OH)3 → AlCl3 + 3H2O

From the equation, we can see that 3 moles of hydrochloric acid react with 1 mole of aluminum hydroxide.

To solve this problem, we need to use a conversion factor to relate the number of moles of Al(OH)3 to the volume of hydrochloric acid. Here's how to do it:

Step 1: Convert the given concentration of hydrochloric acid to moles.
We are given the concentration of hydrochloric acid as 0.110 M. This means that in 1 liter of hydrochloric acid, there are 0.110 moles of HCl.

Step 2: Determine the number of moles of Al(OH)3.
We are given that we have 1.54 moles of Al(OH)3.

Step 3: Use the balanced chemical equation to find the number of moles of HCl required to react completely with Al(OH)3.
From the balanced chemical equation, we know that 3 moles of HCl react with 1 mole of Al(OH)3. So, the number of moles of HCl required is 3 times the number of moles of Al(OH)3.

Step 4: Convert moles of HCl to volume of HCl.
Since we were given the concentration of HCl in moles per liter, we can use this information to convert the moles of HCl to volume.

Finally, multiply the number of moles of HCl required by the molar volume of hydrochloric acid to get the volume of hydrochloric acid.

I hope this explanation helps. Let me know if you need further assistance.