Multiple Choice
What is the molar concentration of a hydrobromic acid solution if it takes 34.12 mL of HBr to completely neutralize 82.56 mL of 0.156 M Ca(OH)2?
2 HBr (aq) + Ca(OH)2 (aq) → CaBr2 (aq) + 2 H2O (l)
9. Solutions
Solution Stoichiometry
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How many milliliters of 0.325 M HCl are needed to react with 16.2 g of magnesium metal?
2 HCl (aq) + Mg (s) → MgCl2 + H2 (g)
A
33 mL
B
742 mL
C
872 mL
D
3321 mL
E
4100 mL
Verified step by step guidance1
First, determine the moles of magnesium (Mg) using its molar mass. The molar mass of Mg is approximately 24.31 g/mol. Use the formula: moles of Mg = mass of Mg / molar mass of Mg.
Next, use the balanced chemical equation to find the stoichiometric relationship between Mg and HCl. According to the equation, 1 mole of Mg reacts with 2 moles of HCl.
Calculate the moles of HCl required using the stoichiometry from the balanced equation: moles of HCl = 2 * moles of Mg.
Now, use the molarity formula to find the volume of HCl solution needed. Molarity (M) is defined as moles of solute per liter of solution. Rearrange the formula to solve for volume: volume (L) = moles of HCl / molarity of HCl.
Convert the volume from liters to milliliters by multiplying by 1000, since 1 L = 1000 mL.
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