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In the titration of 265.0 mL of 0.4000 M HONH2 with 0.2000 M HBr, how many mL of HBr are required to reach the halfway point?

In the titration of 265.0 mL of 0.4000 M HONH2 with 0.2000 M HBr, how many mL of HBr are required to reach the halfway point?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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**Titration Calculation Question** In the titration of 265.0 mL of 0.4000 M HONH₂ with 0.2000 M HBr, how many mL of HBr are required to reach the halfway point? *Analysis:* In a titration, the halfway point is when half of the analyte (HONH₂ in this case) has reacted with the titrant (HBr). To find the volume of HBr needed, calculate the moles of HONH₂ and determine when half of it is neutralized by HBr. 1. Calculate moles of HONH₂: \[ \text{moles of HONH₂} = \text{volume (L)} \times \text{molarity} = 0.265 \, \text{L} \times 0.4000 \, \text{M} \] 2. Determine moles of HONH₂ at halfway point (half the initial moles). 3. Using the 1:1 stoichiometry of the reaction, find the volume of 0.2000 M HBr: \[ \text{volume of HBr (L)} = \frac{\text{moles of HBr needed}}{\text{molarity}} \] 4. Convert volume from liters to milliliters. This calculation allows understanding of the titration process up to the halfway point.
Transcribed Image Text:**Titration Calculation Question** In the titration of 265.0 mL of 0.4000 M HONH₂ with 0.2000 M HBr, how many mL of HBr are required to reach the halfway point? *Analysis:* In a titration, the halfway point is when half of the analyte (HONH₂ in this case) has reacted with the titrant (HBr). To find the volume of HBr needed, calculate the moles of HONH₂ and determine when half of it is neutralized by HBr. 1. Calculate moles of HONH₂: \[ \text{moles of HONH₂} = \text{volume (L)} \times \text{molarity} = 0.265 \, \text{L} \times 0.4000 \, \text{M} \] 2. Determine moles of HONH₂ at halfway point (half the initial moles). 3. Using the 1:1 stoichiometry of the reaction, find the volume of 0.2000 M HBr: \[ \text{volume of HBr (L)} = \frac{\text{moles of HBr needed}}{\text{molarity}} \] 4. Convert volume from liters to milliliters. This calculation allows understanding of the titration process up to the halfway point.
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