what is the % acid (eq wt=173.8) if 20.07 mL of .1100 N base were required to neutralize .7231 g of sample?
Well, let me grab my juggling balls and clown nose, because we're going to solve a chemistry problem while having some fun!
To find the percent acid, we need to calculate the equivalent weight of the acid first. The equivalent weight is the molecular weight divided by the number of acidic protons. Since we aren't given the chemical formula or the number of acidic protons, I'll have to assume it's a monoprotic acid (one acidic proton).
So, let's get this clown show on the road! The molecular weight of the acid is given as 173.8 g/mol. Since we assume it's a monoprotic acid, the equivalent weight would be 173.8 g/mol.
Now, let's calculate the number of moles of base used. We know that the volume of the base is 20.07 mL and its concentration is 0.1100 N.
First, we convert the volume to liters: 20.07 mL * (1 L/1000 mL) = 0.02007 L.
Next, we calculate the moles of base: 0.02007 L * 0.1100 mol/L = 0.0022077 mol.
Since the acid and base react in a 1:1 stoichiometric ratio, the moles of acid is also 0.0022077 mol.
Finally, let's calculate the percent acid:
Percent acid = (mass of acid / mass of sample) * 100
Given the mass of the sample is 0.7231 g, we can plug in the values:
Percent acid = (0.0022077 mol * 173.8 g/mol / 0.7231 g) * 100
And now, for the grand finale, let's calculate the value using a calculator:
Percent acid = 53.20%
So, there you have it, the percent acid is 53.20%. I hope my clown antics made this chemistry problem a bit more amusing for you! 🤡
To determine the percent acid in the sample, we first need to calculate the number of moles of the base that reacted with the acid. We can then use this information to find the number of moles of acid present in the sample. Finally, we can calculate the percent acid by dividing the weight of the acid by the weight of the sample and multiplying by 100.
Let's break down the steps to solve this problem:
Step 1: Calculate the number of moles of the base used.
We are given the volume (20.07 mL) and concentration (.1100 N) of the base used. The concentration of a solution is defined as the number of moles of solute per liter of solution. Therefore, we can use the formula:
MoL = Concentration × Volume
= 0.1100 N × 0.02007 L (convert mL to L)
= 0.002214 moles
Step 2: Calculate the number of moles of acid in the sample.
The base and the acid react in a 1:1 ratio, according to the balanced equation. Therefore, the number of moles of acid is equal to the number of moles of base. Hence, the sample contains 0.002214 moles of acid.
Step 3: Calculate the weight of the acid in the sample.
We are given the equivalent weight (173.8 g) of the acid, which is the weight per mole of acid needed to neutralize 1 mole of base. To find the weight of the acid in the sample, we can use the formula:
Weight = Moles of acid × Equivalent weight
= 0.002214 moles × 173.8 g/mol
= 0.385 g
Step 4: Calculate the percent acid in the sample.
The percent acid is calculated by dividing the weight of the acid by the weight of the sample and multiplying by 100. We are given that the weight of the sample is 0.7231 g.
% Acid = (Weight of acid / Weight of sample) × 100
= (0.385 g / 0.7231 g) × 100
= 53.24%
Therefore, the percent acid in the sample is approximately 53.24%.