A student performed a titration to determine the exact concentration of NaOH(aq). The titration was performed against a standard 0.1000 M HCl(aq) solution. Phenolphthalein indicator was used. The following end-point volumes were recorded by the student in units mL: Trial Number Volume 25.03 25.10 25.07 25.06 5 25.25 6 43.83 Calculate the Qcalc value for the last data point assuming that it is the only outlier. Provide your answer to two decimal places. 1 2 3 4

A student performed a titration to determine the exact concentration of NaOH(aq). The titration was performed against a standard 0.1000 M HCl(aq) solution. Phenolphthalein indicator was used. The following end-point volumes were recorded by the student in units mL: Trial Number Volume 25.03 25.10 25.07 25.06 5 25.25 6 43.83 Calculate the Qcalc value for the last data point assuming that it is the only outlier. Provide your answer to two decimal places. 1 2 3 4

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 26P

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Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
The equation for a reaction by which a solution of sodium carbonate may be standardized is 2HC7H5O2+Na2CO32NaC7H5O2+H2O+CO2. A student determines that 5.038g of HC7H5O2 uses 51.89mL of sodium carbonate solution in the titration. Find the molarity of the sodium carbonate.
It is a solution of unknown concentration in which a solution of accurately known concentration is gradually added until the reaction is complete. Analyte Endpoint Indicator Titrant
A solution of HCl was titrated against sodium carbonate. What is the normality of acid for Trial 3 in the given data? T1 T2 0.3562 0.3479 0.3042 Weight (g) Initial V (mL) 0.80 1.60 0.40 Final V (mL) 35.20 36.70 39.80 Vol HCI used (ml) 35.10 39.40 N of HC (eq/L) 0.1954 0.1870 Average N of HCl (eq/L)
o/index.html?deploymentld%=55750828934189288909969212&eiSBN=9781305657571&snapshotld%32199898&id%3... ☆ IDTAP Q Search this cou Use the References to access important values if needed for this question. The concentration of H3ASO3 in a solution is determined by titration with a 0.1945 M Ce+ solution. The balanced net ionic equation for the reaction is: 2Ce*(aq) + H3ASO3(aq) + 5H2O(1) 2Ce*(aq) + H3ASO4(aq) + 2H3O*(aq) (a) If 19.83 mL of the 0.1945 M Ce** solution are needed to react completely with 30.00 mL of the H3ASO3 solution, what is the concentration of the H3ASO3 solution? M (b) Which of the two solutions was in the buret during the titration? (c) Suppose at the end of the titration, the solution containing the Ce³* ion is transferred to a volumetric flask and diluted to 300. mL. What is the concentration of Ce3+In the diluted solution? Submit Answer 5 question attempts remaining
Che. 065: Acid -Base Titration: Part I: Standardization of NaOH(aq): Molarity of NaOH(aq) is determined by using the stoichiometry reaction with a strong acid such as HCl(aq). Part II: Molarity and mass % of acetic acid CH3COOH(aq) in a vinegar solution are determined by the reaction with NaOH(aq). Part I: Standardization of NaOH(aq): Use a 50.00 mL. Buret : wash it with tap H2O twice, with deionized H2O twice and twice with 0.100 M HCl (aq). Fill the buret with 0.100 M HCl(aq), remove the air bubble and adjust the initial buret reading to 0.00 mL. Get two 125 mL. Erlenmeyer. To each Erlenmeyer flask add 20.00 mL. HCl(aq) from the buret. Burette Holder 3P Burette Flask Support Stand Trail 2 Trial 1 Initial buret reading of HCl(aq): 0.00 mL. Final buret reading of HCl(aq): 20.00 mL. Volume of HCl(aq) : Initial buret reading of HCl(aq): 20.00 mL. Final buret reading of HCl(aq): 40.00 mL. Volume of HCl(aq) Add 3 drops of phenolphethaleine to each Erlenmeyer flask, the color of solution is…
. Lets pretend for a moment that you’re now working as an analyst working for the policedepartment. You are asked to analyze a white powder confiscated from a suspect. The complainantclaimed that the powder was used by the suspect to slowly poison the victim. Suppose the suspectclaimed it is only sodium chloride, how would you analyze the material to confirm that is indeed NaCl.Outline the qualitative test that must be done and provide inference for each test.(NOTE: Make sure analysis is in logical order backed up with chemical reactions if possible because youwill present it during the court hearing)An honest MISTAKE in the analysis can be a reason why innocent person will suffer in jail or a trueblooded murderer will escape the case.
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A student prepares a weak acid solution by dissolving 0.2400 g HZ to give 100. mL solution. The titration requires 30.0 mL of 0.1025 M NaOH. Calculate the molar mass of the acid. (a) Would the molar mass be too high, too low, or unaffected if the student accidentally used 0.1400 g in the calculation? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated (b) Would the molar mass be too high, too low, or unaffected if the student accidentally used 20.0 mL instead of 30.0 mL? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated
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In a 4.9 mm aqueous solution of benzoic acid (C6H₂CO₂H), what is the percentage of benzoic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. O Round your answer to 2 significant digits. []% x10 X Ś |||