Multiple Choice
You have a beaker holding 25.0 mL of 1.5 M HCl. You then add 10.0 mL of 2.0 M NaOH to the beaker. What is the pH of the solution after the addition of the NaOH?
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6. Chemical Quantities & Aqueous Reactions
Solution Stoichiometry
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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
Identify the balanced chemical equation: 2 HBr (aq) + Ca(OH)2 (aq) → CaBr2 (aq) + 2 H2O (l). This tells us that 2 moles of HBr react with 1 mole of Ca(OH)2.
Calculate the moles of Ca(OH)2 using its volume and molarity. Use the formula: moles = molarity × volume (in liters). Convert 82.56 mL to liters by dividing by 1000.
Use the stoichiometry from the balanced equation to find the moles of HBr needed. Since 2 moles of HBr react with 1 mole of Ca(OH)2, multiply the moles of Ca(OH)2 by 2 to get the moles of HBr.
Calculate the molarity of the HBr solution. Use the formula: molarity = moles of solute / volume of solution (in liters). Convert 34.12 mL of HBr to liters by dividing by 1000.
Compare the calculated molarity of HBr with the given options to determine the correct answer.
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