1. How much base 0.1 M NaOH was required to neutralize lemon juice from our experiment part 1, and what was the pH at the neutralization point? Osonal u lemon Joce-pH-7.85 2. How much base 0.1 M NAOH was required to neutralize vinegar, and what was the pH at the neutralization point? Kincgar pt - ファて0 3. How much base 0.1 M NaOH was required to neutralize soda drink, and what was the pH at the neutralization point? Socla pH-8.70 sonDlains.cole 4. List the three solutions in order of increasing acid content. (least acidic to most acidic)

1. How much base 0.1 M NaOH was required to neutralize lemon juice from our experiment part 1, and what was the pH at the neutralization point? Osonal u lemon Joce-pH-7.85 2. How much base 0.1 M NAOH was required to neutralize vinegar, and what was the pH at the neutralization point? Kincgar pt - ファて0 3. How much base 0.1 M NaOH was required to neutralize soda drink, and what was the pH at the neutralization point? Socla pH-8.70 sonDlains.cole 4. List the three solutions in order of increasing acid content. (least acidic to most acidic)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.58QE

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A solution contains a mixture of Na2CO3 and NaOH. Using phenolphthalein indicator 25 ml of mixture required 19.5 mL of 0.995 M HCl for the endpoint. With methyl orange, 25 ml of solution required 25 ml of the same HCl for the endpoint. Calculate grams per liter of Na2CO3 in the mixture.
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The following graph shows the pH curve for the titration of 25 mL of a 0.1 M monoprotic acid solution with a 0.1 M solution of a monoprotic base. mL of 0.1 M base added (1) The pH curve represents the titration of a BLANK acid with a BLANK base.(2) Choose a suitable indicator for the endpoint of the titration from the following pulldown list.
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…
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