Four solutions of unknown HClHCl concentration are titrated with solutions of NaOHNaOH. The following table lists the volume of each unknown HClHCl solution, the volume of NaOHNaOH solution required to reach the equivalence point, and the concentration of each NaOHNaOH solution. HClHCl Volume (mL)(mL) NaOHNaOH Volume (mL)(mL) [NaOH][NaOH] (M)(M) 24.00 mLmL 23.44 mLmL 0.1201 MM 11.00 mLmL 20.22 mLmL 0.0952 MM 23.00 mLmL 11.88 mLmL 0.1128 MM 3.00 mLmL 5.88 mLmL 0.1325 MM 1. Calculate the concentration (in MM) of the unknown HClHCl solution in the first case. HClVolume (mL) NaOH Volume (mL) [NaOH](M) 24.00 mL 23.44 mL 0.1201 M 2. Calculate the concentration (in MM) of the unknown HClHCl solution in the second case. HCl Volume (mL) NaOH Volume (mL) [NaOH] (M) 11.00 mL 20.22 mL 0.0952 M 3. Calculate the concentration (in MM) of the unknown HClHCl solution in the third case. HCl Volume (mL) NaOH Volume (mL) [NaOH][NaOH] (M) 23.00 mL 11.88 mL 0.1128 M 4. Calculate the concentration (in MM) of the unknown HClHCl solution in the fourth case. HCl Volume (mL) NaOH Volume (mL) [NaOH] (M) 3.00 mL 5.88 mL 0.1325 M
Four solutions of unknown HClHCl concentration are titrated with solutions of NaOHNaOH. The following table lists the volume of each unknown HClHCl solution, the volume of NaOHNaOH solution required to reach the equivalence point, and the concentration of each NaOHNaOH solution. HClHCl Volume (mL)(mL) NaOHNaOH Volume (mL)(mL) [NaOH][NaOH] (M)(M) 24.00 mLmL 23.44 mLmL 0.1201 MM 11.00 mLmL 20.22 mLmL 0.0952 MM 23.00 mLmL 11.88 mLmL 0.1128 MM 3.00 mLmL 5.88 mLmL 0.1325 MM 1. Calculate the concentration (in MM) of the unknown HClHCl solution in the first case. HClVolume (mL) NaOH Volume (mL) [NaOH](M) 24.00 mL 23.44 mL 0.1201 M 2. Calculate the concentration (in MM) of the unknown HClHCl solution in the second case. HCl Volume (mL) NaOH Volume (mL) [NaOH] (M) 11.00 mL 20.22 mL 0.0952 M 3. Calculate the concentration (in MM) of the unknown HClHCl solution in the third case. HCl Volume (mL) NaOH Volume (mL) [NaOH][NaOH] (M) 23.00 mL 11.88 mL 0.1128 M 4. Calculate the concentration (in MM) of the unknown HClHCl solution in the fourth case. HCl Volume (mL) NaOH Volume (mL) [NaOH] (M) 3.00 mL 5.88 mL 0.1325 M
General Chemistry - Standalone book (MindTap Course List)
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ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.149QP: A solution of weak base is titrated to the equivalence point with a strong acid. Which one of the...
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Four solutions of unknown HClHCl concentration are titrated with solutions of NaOHNaOH. The following table lists the volume of each unknown HClHCl solution, the volume of NaOHNaOH solution required to reach the equivalence point, and the concentration of each NaOHNaOH solution.
| HClHCl Volume (mL)(mL) | NaOHNaOH Volume (mL)(mL) | [NaOH][NaOH] (M)(M) |
| 24.00 mLmL | 23.44 mLmL | 0.1201 MM |
| 11.00 mLmL | 20.22 mLmL | 0.0952 MM |
| 23.00 mLmL | 11.88 mLmL | 0.1128 MM |
| 3.00 mLmL | 5.88 mLmL | 0.1325 MM |
1. Calculate the concentration (in MM) of the unknown HClHCl solution in the first case.
| HClVolume (mL) | NaOH Volume (mL) | [NaOH](M) |
| 24.00 mL | 23.44 mL | 0.1201 M |
2. Calculate the concentration (in MM) of the unknown HClHCl solution in the second case.
| HCl Volume (mL) | NaOH Volume (mL) | [NaOH] (M) |
| 11.00 mL | 20.22 mL | 0.0952 M |
3. Calculate the concentration (in MM) of the unknown HClHCl solution in the third case.
| HCl Volume (mL) | NaOH Volume (mL) | [NaOH][NaOH] (M) |
| 23.00 mL | 11.88 mL | 0.1128 M |
4. Calculate the concentration (in MM) of the unknown HClHCl solution in the fourth case.
| HCl Volume (mL) | NaOH Volume (mL) | [NaOH] (M) |
| 3.00 mL | 5.88 mL | 0.1325 M |
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