Multiple Choice
How many grams of zinc metal are required to produce 3.5 liters of hydrogen gas at STP according to the chemical equation Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)?
3. Chemical Reactions
Stoichiometry
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How many milliliters of 1.50 M H₂SO₄ are needed to neutralize 75.0 g of NaOH?
A
1000 mL
B
250 mL
C
750 mL
D
500 mL
Verified step by step guidance1
Calculate the number of moles of NaOH using its molar mass. The molar mass of NaOH is approximately 40.00 g/mol. Use the formula: \( \text{moles of NaOH} = \frac{\text{mass of NaOH (g)}}{\text{molar mass of NaOH (g/mol)}} \).
Write the balanced chemical equation for the neutralization reaction: \( \text{H}_2\text{SO}_4 + 2\text{NaOH} \rightarrow \text{Na}_2\text{SO}_4 + 2\text{H}_2\text{O} \). This shows that 1 mole of H₂SO₄ reacts with 2 moles of NaOH.
Determine the moles of H₂SO₄ needed to neutralize the moles of NaOH calculated in step 1. Use the stoichiometry from the balanced equation: \( \text{moles of H}_2\text{SO}_4 = \frac{\text{moles of NaOH}}{2} \).
Use the molarity of the H₂SO₄ solution to find the volume needed. The formula for molarity is \( M = \frac{\text{moles of solute}}{\text{liters of solution}} \). Rearrange to find the volume: \( \text{volume (L)} = \frac{\text{moles of H}_2\text{SO}_4}{1.50 \text{ M}} \).
Convert the volume from liters to milliliters by multiplying by 1000, since 1 L = 1000 mL. This will give you the volume of 1.50 M H₂SO₄ needed to neutralize the given amount of NaOH.
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