객관식
You mix a 125.0-mL sample of a solution that is 0.0117 M in NiCl₂ with a 175.0-mL sample of a solution that is 0.250 M in NH₃. After the solution reaches equilibrium, what concentration of Ni²⁺(aq) remains?
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6. Chemical Quantities & Aqueous Reactions
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
검증된 단계별 안내1
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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