Multiple Choice
A 10.0 mL solution of 0.121 M H₂SO₄ is neutralized by 17.1 mL of KOH solution. What is the molarity of the KOH solution?
3. Chemical Reactions
Stoichiometry
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A sample of acetic acid is composed of 2.05 g of carbon and 2.73 g of oxygen. Calculate the mass of carbon in another sample of acetic acid that is composed of 3.27 g of oxygen.
A
3.27 g
B
1.85 g
C
2.45 g
D
2.05 g
Verified step by step guidance1
Determine the mass ratio of carbon to oxygen in the original sample of acetic acid. This is done by dividing the mass of carbon by the mass of oxygen: \( \text{Ratio} = \frac{2.05 \text{ g C}}{2.73 \text{ g O}} \).
Calculate the mass of carbon in the new sample using the mass ratio obtained in the previous step. Set up a proportion where the mass of carbon in the new sample (\( x \)) is to the mass of oxygen in the new sample (3.27 g) as the original mass ratio: \( \frac{x}{3.27 \text{ g O}} = \frac{2.05 \text{ g C}}{2.73 \text{ g O}} \).
Solve the proportion for \( x \) by cross-multiplying: \( x \times 2.73 = 2.05 \times 3.27 \).
Isolate \( x \) by dividing both sides of the equation by 2.73: \( x = \frac{2.05 \times 3.27}{2.73} \).
Calculate the value of \( x \) to find the mass of carbon in the new sample. This will give you the mass of carbon corresponding to 3.27 g of oxygen in the new sample.
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