if 53.0mL of 0.150M of HCl is needed to neutralize all the NH3 from a 2.28g sample of organic material. what is the mass percent of notrogen in the sample?

NH3 HCl ==> NH4Cl

mols HCl = M x L = ?
mols NH3 must be the same as mols HCl.
mols N (not N2) = same as mols NH3.
g N = mols N x atomic mass N = ?
%N = (grams N/mass sample)*100 = ?

2

Well, isn't that a titrifying question! To find the mass percent of nitrogen in the sample, we need to follow a few steps. Let's shake things up and start crunching some numbers!

First, let's calculate the number of moles of HCl used. We have a volume of 53.0 mL and a concentration of 0.150 M. So, Moles of HCl = Volume (L) × Concentration (M). Don't worry, I'll help you convert mL to L, because we need to keep things in the same units.

53.0 mL = 0.0530 L
Moles of HCl = 0.0530 L × 0.150 M

Now, we need to figure out the moles of NH3 that can be neutralized by the HCl. Since the reaction between HCl and NH3 is 1:1, and moles = mass / molar mass, we can calculate the moles of NH3:

Molar mass of NH3 = 17.03 g/mol
Moles of NH3 = 2.28 g / 17.03 g/mol

Finally, let's determine the moles of nitrogen in the sample. Again, since the reaction is 1:1, we'll use the same number of moles of NH3 as nitrogen:

Moles of nitrogen = Moles of NH3

Now, to calculate the mass percent of nitrogen in the sample, we divide the mass of nitrogen by the total mass of the sample (2.28 g) and multiply by 100:

Mass percent of nitrogen = (Moles of nitrogen × Molar mass of nitrogen) / 2.28 g * 100

Now, I'm not just a clown, I'm a jokester too, so here's a little bonus: Why did the acid go to therapy? Because it had too many neutralizing reactions and needed to find its balance!

To find the mass percent of nitrogen in the sample, we need to determine the number of moles of NH3 in the organic material. Then, we can calculate the mass percent using the formula:

Mass percent of nitrogen = (mass of nitrogen / mass of sample) * 100

First, let's calculate the number of moles of HCl used to neutralize all the NH3.

Number of moles of HCl = volume of HCl (in L) * concentration of HCl (in mol/L)

Given:
Volume of HCl = 53.0 mL = 0.053 L
Concentration of HCl = 0.150 M

Number of moles of HCl = 0.053 L * 0.150 mol/L = 0.00795 mol

According to the balanced chemical equation (assuming complete reaction):

NH3 + HCl -> NH4Cl

The stoichiometric ratio between NH3 and HCl is 1:1. This means that 1 mole of NH3 reacts with 1 mole of HCl.

Since the number of moles of HCl used equals the number of moles of NH3 in the organic material, we have:

Number of moles of NH3 = 0.00795 mol

Next, let's calculate the molar mass of NH3.

Molar mass of NH3 = 14.01 g/mol (molar mass of nitrogen) + 3 * 1.01 g/mol (molar mass of hydrogen) = 17.04 g/mol

To determine the mass of nitrogen in the sample, we can use the moles of NH3 and the molar mass of nitrogen:

Mass of nitrogen = moles of NH3 * molar mass of nitrogen = 0.00795 mol * 14.01 g/mol = 0.111 g

Now, we can calculate the mass percent of nitrogen in the sample:

Mass percent of nitrogen = (mass of nitrogen / mass of sample) * 100

Given:
Mass of sample = 2.28 g

Mass percent of nitrogen = (0.111 g / 2.28 g) * 100 = 4.87%

Therefore, the mass percent of nitrogen in the sample is approximately 4.87%.