I figured all the parts of the problem except for the last one. Can you tell me what to do?
In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 grams. The mustard was then dissolved in 50.0 ml. of distilled water. The total mass of the solution was found to be 49.401 grams. Calculate the weight percent of the mustard in the prepared solution.
7.7
The result of a micro-scale titration showed that 3.91E-5 moles of NaOH were required to titrate a 0.775 gram sample of mustard solution to an orange-red end point.
Calculate the number of grams of acetic acid in the sample of mustard solution.
2.35×10-3
Calculate the weight percent of acetic acid in this titrated sample.
0.30
Using the information provided in the questions above, calculate the weight percent of acetic acid in the original package of mustard prepared above???
the mustard throws me. If water is 1g/ml, how can 50ml of water + mustard weigh less than 50g?
To calculate the weight percent of acetic acid in the original package of mustard prepared, you will need to use the information from the previous questions.
First, calculate the number of moles of acetic acid in the sample of mustard solution. You were given that 3.91E-5 moles of NaOH were required to titrate a 0.775 gram sample of mustard solution. So, the number of moles of acetic acid in the sample can be considered equal to the number of moles of NaOH.
Next, calculate the molar mass of acetic acid, which is 60.052 g/mol.
Now, use the number of moles of acetic acid and the molar mass to determine the grams of acetic acid in the sample. Multiply the number of moles by the molar mass.
Once you have determined the grams of acetic acid in the sample, you can calculate the weight percent. Divide the grams of acetic acid by the mass of the solution (49.401 grams) and multiply by 100 to convert it to a percentage.
This will give you the weight percent of acetic acid in the original package of mustard prepared above.
To calculate the weight percent of acetic acid in the original package of mustard, we need to understand that acetic acid is the main component of mustard.
First, let's calculate the number of moles of acetic acid in the titrated sample. We know that 3.91E-5 moles of NaOH were required to titrate a 0.775 gram sample of mustard solution to an orange-red end point.
Next, we'll use the molar ratio between acetic acid and NaOH from the balanced chemical equation of the reaction to determine the number of moles of acetic acid.
Let's assume the balanced chemical equation for the reaction is:
NaOH + CH3COOH -> CH3COONa + H2O
From the balanced equation, we see that 1 mole of NaOH reacts with 1 mole of acetic acid. Therefore, the number of moles of acetic acid in the sample is also 3.91E-5 moles.
Now, let's calculate the weight of acetic acid in the sample. Since we know the molar mass of acetic acid is approximately 60.05 g/mol, we can use the formula:
Weight (g) = Moles × Molar Mass
Weight_acetic_acid = 3.91E-5 moles × 60.05 g/mol
Weight_acetic_acid = 0.00235 grams
So, there are approximately 0.00235 grams of acetic acid in the sample of mustard solution.
Now, we can calculate the weight percent of acetic acid in the original package of mustard. We know that the mass of the mustard in the package is 3.809 grams.
Weight_percent_acetic_acid = (Weight_acetic_acid / Mass_of_mustard) × 100
Weight_percent_acetic_acid = (0.00235 grams / 3.809 grams) × 100
Weight_percent_acetic_acid ≈ 0.0616%
Therefore, the weight percent of acetic acid in the original package of mustard is approximately 0.0616%.