3How to Titrate: Lab Techniques TitrationTitration Procedures:Add about 100mL of a 0.1 M NAOH solution to a 250mL beaker.2. Obtain a buret and rinse with about 10 ml of the NaOH solution.3. Fill the buret with NaOH and record starting volume to the nearest 1m" of a milliliter.4. Measure out exactly 10.0 ml of HC in a graduated cylinder and add it to a 250mL Erlenmeyerflask along with 1 drop of phenolphthalein indicator.5. Slowly add the NaOH to the flask with the acid and swirl. Continue adding the base until acolor change (faint pink) occurs and remains for at least 10 seconds. This is the endpoint ofthis neutralization eaction.6. Read and record the ending volume of NaOH in the buret,7. Repeat steps 1 through 6 two more times for Trials 2 and 3.8. Calculate the volume of base added in each trial.9. Use the volume of base added and the volume of acid added to calculate the molarity of theacid for each trial.10. Calculate the average molarity of the acid.11. Calculate the percent eror of your acid molarity by comparing it to the molarity that yourteacher gives you.1.Titration: Sulfuric Acid + Sodium HydroxideTrial 3DATA TABLE10 pts.All volumes are correctly recorded to theTrial 1of a milliliter. Units are corect.Volumes are recorded, but are incorrectTrial 25 pta.or notaccurate ennuphNo data shownO pts.Volume of HCI used10.0ml10.0ml10.0ml1.00ml0.40ml3,00mlStarting volume of NaOH35.9ml34.4ml35.7mEnding volume of NaOH35.0ml34.0ml32.7mlVolume of NaOH usedAnalysis of Data:PA 12:51围acer enus (Alt+/)100%Heading 3Arlal1024 I56or notuccurate enough.No data shownO pts.Volume of HCI used10.0ml10.0ml10.0mlStarting volume of NaOH1.00ml0.40ml3.00mlEnding volume of NaOH35.9ml34.4ml35.7mlVolume of NaOH used35.0ml34.0ml32.7mlAnalysis of Data:Calculate the molarity f the HCI for each trial that was titrated using your volume of NaOH used.Show all work with proper units and report your answer below. Continue on the back if necessary.NaOH + HCI → H,O + NaCICalculate the average molarity of the HCI that was titrated. Show your work.Average molarity of HCI :Percent Error:% (show your work)V O 12:52围

The given titration is an example of a typical acid-base titration. Here, the acid HCl is being…

Analysis of Data: Calculate the molarity f the HCI for each trial that was titrated using your volume of NaOH used. Show all work with proper units and report your answer below. Continue on the back if necessary. NaOH + HCI → H,0 + NaCI Calculate the average molarity of the HCI that was titrated. Show your work. Average molarity of HCI:

Analysis of Data: Calculate the molarity f the HCI for each trial that was titrated using your volume of NaOH used. Show all work with proper units and report your answer below. Continue on the back if necessary. NaOH + HCI → H,0 + NaCI Calculate the average molarity of the HCI that was titrated. Show your work. Average molarity of HCI:

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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Reaction A Sodium Sodium Acetic acid Water hydroxido acetate Use the titration data to calculate the molarity of acetic acid in the vinegar. Try a sample calculation Refer to Section 4 for sample calculations: A 5.00 ml sample of vinegar was titrated with 0.08751 M N2OH. The sample requires 22.31 mL of NAOH to reach the endpoint. Calculate the molarity of the acetic acid (CH,COOH) solution in the vinegar sample. The density of the vinegar solution has been determined to be 1.0052 g/ml. If the vinegar is being manufactured, and is supposed to have a molar concentration between 0.45 and 0.60, can this batch be sold? Section 2: Safety Precautions and Waste Disposal prepare you for this lab, watch the following video on setting up and performing a t pdf 9 Math 30 Online Fi...pdf 2 220 1678 final fall..pdf hp
Part C – Acid–base and solubility equilibria 1. Rinse 4 regular size test tubes and a 10 mL measuring cylinder thoroughly with water. Number the test-tubes from 1 to 4 in a test tube rack. 2. Into each of test tubes 1 – 3 put a small amount of solid benzoic acid (put the same amount – about the size of a pea – in each test tube). 3. Add 2 mL (use the measuring cylinder) of water to tube 1 and shake to mix the contents. 4. Add 2 mL (measuring cylinder) of 2 M HNO3 to tube 2 and shake to mix the contents. 5. Rinse the measuring cylinder with water, then use it to add 2 mL of 2 M NaOH to tube 3 and shake for about 10 seconds to mix the contents. Rinse the measuring cylinder. 6. Pour about half of the solution from tube 3 into tube 4, than add 2 mL of 2 M HNO3 to tube 4. 7. Allow the test tubes to stand for 2 or 3 minutes then record the appearance of the mixtures in each test tube. 8. Answer the questions on the results page relating to this equilibrium system.
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A student is making a titration curve. To do so, they added 15.00 mL of 0.1300 M HCl to a flask. They then added 14.40 mL of 0.1170 M NaOH to the flask. What is the pH at this point in the titration curve?
Some soluble compounds are listed in the table below. Complete the table by filling in the name or chemical formula of each compound, whichever is missing. (If there is more than one way to name the compound, choose the name used when the compound is dissolved in water.) Also classify the compound using the checkboxes. compound 0 HCH₂ CO₂ NH3 HCIO4 name barium hydroxide 0 0 type of compound (check all that apply) strong weak strong weak acid base base acid ionic molecular 0 0 0 0 X S
Please answer the question! Find the molarity and mass percent of ammonium hydroxide solutions. Thanks!
||| O ACIDS AND BASES Calculating percent dissociation of a weak... A student prepares a 0.41 mm aqueous solution of acetic acid (CH3cO₂H). Calculate the fraction of acetic acid that is in the dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. % 0 x10 0/3 X
At the beginning of a titration, the acetic acid burette reads 0.30 mL. At the end of the titration. thé burette reads 27.70 mL. What volume had been added to the flask? Answer to two places past the decimal.
Calculate the molarity of the HCl using 25.00 mL of HCl solution and the volume of the 0.3000 M NaOH also 25ml