Titration of Acids and Basesfa Vola!!Part B. Determination of the molar concentration of an unknown acid.Volume of unknown acid used (mL)Final buret reading (mL NaOH)Initial buret reading (mL NaOH)Volume of NaOH used (mL)an unknownandMolarity of unknown acidTrial 110mL9.6 mL0.5mL9,1mLTrial 2Sample calculations for molarity of unknown acid solution:10mL18,9Trial 3Average molarity of unknown acid solution:10mL28.3mL9.6 ml 18,9ml9,3m² 9.4mLmol NaOHused?M N₂OH =M acid= .1Griln.1To multipledecimals

The question is based on the concepts of titrations. we need to calculate concentration of unknown…

Titration of Acids and Bases Mate of a Volatile Part B. Determination of the molar concentration of an unknown acid. Volume of unknown acid used (mL) the Final buret reading (mL NaOH) Initial buret reading (mL NaOH) Volume of NaOH used (mL) Molarity of unknown acid Trial 1 10mL on 9.6 mL 0.5ml 9.1mL Trial 2 Sample calculations for molarity of unknown acid solution: 10ml Average molarity of unknown acid solution: Trial 3 10mL 28.3mL 18.9 9.6 ml 18,9ml 9,3mL 9.4mL mol NaOH used? M NaOH = Macid= .1 Guil To multiple decimals

Titration of Acids and Bases Mate of a Volatile Part B. Determination of the molar concentration of an unknown acid. Volume of unknown acid used (mL) the Final buret reading (mL NaOH) Initial buret reading (mL NaOH) Volume of NaOH used (mL) Molarity of unknown acid Trial 1 10mL on 9.6 mL 0.5ml 9.1mL Trial 2 Sample calculations for molarity of unknown acid solution: 10ml Average molarity of unknown acid solution: Trial 3 10mL 28.3mL 18.9 9.6 ml 18,9ml 9,3mL 9.4mL mol NaOH used? M NaOH = Macid= .1 Guil To multiple decimals

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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I need help please calculating the values!
In the case of over-titration, what should be done to the sample? Select one: a. Dilute the sample with water b. Discard and prepare another sample c. Add acid to revert the color back to faint pink or colorless d. Add more phenolphthalein indicator
3. Titration: Strong Acid / Weak Base. (I warned you to be ready!) Here's the cool chart! Analyte: 20.00 mL 0.100 M Hydrazine (N₂H4) Hd A: initial Vertical (Value) Axis Title 0 B: half equivalence C: equivalence 5 10 15 20 Titrant: mL of 0.100 M HCI added 25 20.00 mL of 0.100 M hydrazine (N₂H4, pKb = 5.77) is titrated with 0.100 M HCl. a) Find the initial pH (point A) and the pH at the equivalence point (point C). b) Find the pH at the half equivalence point (point B).
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What is the best sequence of steps for filling the burette with NaOH for a titration? Lower the burette to eye' level, insert the funnel in the top of the burette, slowly add the NaOH through the funnel, check the burette stopcock is closed O Check the burette stopcock is closed, lower the burette to eye level, insert a funnel in the top of the burette, slowly add the NaOH through the funnel Check the burette stopcock is closed, insert the funnel in the top of the burette, slowly add the NaOH through the funnel, lower the burette to eye level
The graph below represents the titration curve of a A. 1 M strong acid with 1 M strong base B. 1 M weak base with 1 M strong acid C. 1 M strong base with 1 M strong acid D. 1 M weak base with 1 M weak acid E. 1 M weak acid with 1 M strong base
Which one of the following is NOT a source of error during a titration? Group of answer choices Adding too much sodium hydroxide solution to the analyte Refilling the buret during a titration trial Rinsing the buret with the analyte Adding indicator to the analyte
A different titration experiment using a 0.122M standardized NaOH solution to titrate a 26.48 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4) gave the following molarities for 3 trials. Initial Burette Reading (mL) Final Burette Reading (mL) Delivered vol (mL) Acid Concentration (M) Trial 1 0.0345 Trial 2 0.0334 Trial 3 0.0381 From the 3 trials, determine the average Molarity concentration of the H2SO4 to 3 significant digits. Don't include a unit.
Incorrect Your answer is incorrect. • KC: Your answer is incorrect. • Cacl, Vour answer is incorrect. For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll ind K, data in the ALEKS Data tab. Does enlubility change with pH? hiyhest solubility compound pll 5 pll 6 pll 8 yes O no yes Ba(OH), O no O yes Caci, e no
14 Given the hypothetical titration curves below, determine what curve has a stronger acid. 14 a. b. C. d. 12 10 8 6 4 () 0 Curve A Curve B Curve C Cannot be determined A B and C 10 20 30 40 50 60 Volume of 0.1000 M NaOH, mL
The molarity for trial 1 will be 0.4035 and trial 2 molarity will be 0.3587 I need some assistance on question 2 if possible
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