Multiple Choice
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)
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13. Solutions
Solution Stoichiometry
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)
A
0.326 M
B
0.755 M
C
0.811 M
D
1.38 M
E
1.85 M
Verified step by step guidance1
Start by writing the balanced chemical equation for the reaction: 2 HBr (aq) + Ca(OH)2 (aq) → CaBr2 (aq) + 2 H2O (l). This equation shows that 2 moles of HBr react with 1 mole of Ca(OH)2.
Calculate the moles of Ca(OH)2 using its molar concentration and volume. Use the formula: \( \text{moles of Ca(OH)}_2 = \text{concentration} \times \text{volume} \). Convert the volume from mL to L by dividing by 1000.
Determine the moles of HBr required to neutralize the Ca(OH)2. Since the stoichiometry of the reaction is 2:1, multiply the moles of Ca(OH)2 by 2 to find the moles of HBr.
Calculate the molar concentration of HBr using the moles of HBr and the volume of HBr solution. Use the formula: \( \text{concentration of HBr} = \frac{\text{moles of HBr}}{\text{volume of HBr in L}} \). Convert the volume from mL to L by dividing by 1000.
Review the calculated molar concentration of HBr and compare it with the given options to identify the correct answer.
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