Mass of unknown transferred Mass of filter paper Mass of paper and dry BaSO, Trial 1 (Yours) 0.294g 0.907g 1.203g Trial 2 (Partners) 0.253g 0.899g 1.163g Give me the Calculations week 1 Mass of dry BasO Calculated percent sulfate in unknown AVERAGE PERCENT SULFATE
The Correct Answer and Explanation is:
To calculate the mass of dry BaSO₄ (barium sulfate) and the percentage of sulfate in the unknown sample, we need to follow a step-by-step process using the data provided from both trials.
Step 1: Calculate the mass of BaSO₄ in each trial.
Trial 1 (Your Sample):
- Mass of paper and dry BaSO₄: 1.203 g
- Mass of filter paper: 0.907 g
Mass of dry BaSO₄ = Mass of paper and dry BaSO₄ – Mass of filter paper
Mass of dry BaSO₄ = 1.203 g – 0.907 g = 0.296 g
Trial 2 (Partner’s Sample):
- Mass of paper and dry BaSO₄: 1.163 g
- Mass of filter paper: 0.899 g
Mass of dry BaSO₄ = Mass of paper and dry BaSO₄ – Mass of filter paper
Mass of dry BaSO₄ = 1.163 g – 0.899 g = 0.264 g
Step 2: Calculate the percent sulfate in the unknown sample for each trial.
To calculate the percent sulfate in the unknown, we first need to know the molar masses:
- BaSO₄ (barium sulfate):
Ba = 137.33 g/mol, S = 32.07 g/mol, O = 16.00 g/mol
Molar mass of BaSO₄ = 137.33 + 32.07 + (4 × 16.00) = 233.39 g/mol
The percentage of sulfate (SO₄) in BaSO₄ is calculated as the mass of SO₄ divided by the mass of BaSO₄, multiplied by 100.
- Molar mass of SO₄ = 32.07 + (4 × 16.00) = 96.07 g/mol
So, the percent sulfate in BaSO₄ is:96.07233.39×100=41.16%\frac{{96.07}}{{233.39}} \times 100 = 41.16\%233.3996.07×100=41.16%
Now we can calculate the percent sulfate in the unknown sample for each trial.
Trial 1:
- Mass of dry BaSO₄ = 0.296 g
- Percent sulfate in BaSO₄ = 41.16%
Percent sulfate in unknown = 0.296 g×41.16100=0.121 g0.296 \, \text{g} \times \frac{{41.16}}{{100}} = 0.121 \, \text{g}0.296g×10041.16=0.121g
Percent sulfate in unknown sample = 12.1%
Trial 2:
- Mass of dry BaSO₄ = 0.264 g
- Percent sulfate in BaSO₄ = 41.16%
Percent sulfate in unknown = 0.264 g×41.16100=0.109 g0.264 \, \text{g} \times \frac{{41.16}}{{100}} = 0.109 \, \text{g}0.264g×10041.16=0.109g
Percent sulfate in unknown sample = 10.9%
Step 3: Calculate the average percent sulfate in the unknown.
Average percent sulfate=12.1%+10.9%2=11.5%\text{Average percent sulfate} = \frac{{12.1\% + 10.9\%}}{2} = 11.5\%Average percent sulfate=212.1%+10.9%=11.5%
Final Results:
- Mass of dry BaSO₄ (Trial 1): 0.296 g
- Mass of dry BaSO₄ (Trial 2): 0.264 g
- Percent sulfate in unknown (Trial 1): 12.1%
- Percent sulfate in unknown (Trial 2): 10.9%
- Average percent sulfate in unknown: 11.5%
This calculation shows the concentration of sulfate in the unknown sample based on the barium sulfate precipitate formed during the experiment. The average value gives a reliable estimate of the sulfate content across both trials.
