One of your classmates (or you, perhaps!) forgot to add phenolphthalein indicator before starting the titration, and he/she already began adding sodium hydroxide from the buret! Uh oh...what should be done? a) Just restart. The trial is completely ruined. b) Add a couple drops of phenolphthalein into the acid flask. If it remains clear, nothing's wrong. If it changes to dark pink, record the final buret reading and call it

One of your classmates (or you, perhaps!) forgot to add phenolphthalein indicator before starting the titration, and he/she already began adding sodium hydroxide from the buret! Uh oh...what should be done? a) Just restart. The trial is completely ruined. b) Add a couple drops of phenolphthalein into the acid flask. If it remains clear, nothing's wrong. If it changes to dark pink, record the final buret reading and call it

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 11P

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ou let your partner do a trial since you're nice. He/she adds a few mL of NaOH, but you realize that nobody recorded the initial buret level! RATS! What do you do? a) Just get light pink since that's the point of titrations anyways. b) Finish the titration and record the final buret reading. Ask your instructor what the initial buret reading was since he knows all of them by heart...right? c) Just record the current level as the "initial" reading. Precision isn't THAT important. d) Restart the trial since you have no idea how much NaOH was added so far.
Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Standardization of Titrant Question 7 Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX __ ET TOPIC: Determination of Molar Concentration of each component (Double Indicator Titration) Question 8 No blank correction Ex ___ ET Question 9 Bubbles trapped in the tip of burette: EX ___ ET Question 10 Measuring the sample volume using a volumetric pipet while looking downwards at the meniscus: EX ___ ET
Please answer it ALL ASAP and CORRECTLY for an upvote. PROVIDE YOUR FULL SOLUTION. You prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 ml of 0.13 M ammonium chloride. The dissociation constant of ammonia is 1.8x10^-5 What is the total volume of the buffer? What is the final concentration of the base? What is the final concentration of the salt? What is the acid strength of the solution? What is the pH of the buffer solution?
Complete the following: 1. Random error, also called _________arises from the effects of uncontrolled variables in the measurement. 2. The ____________,measures how closely the data are clustered about mean. 3. The chemical equilibrium in which all the reactants and products are in the same phase are called____________. 4. Reaction that go to completion and never proceed in the reverse direction are said to be_____________ 5. The equation for buffer is the__________equation. 6. A ___________solution is one that resists changes in pH when small quantities of an acid or an alkali added to it. 7. __________is the pH of the pure, neutral and polyprotic
A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…
A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…
A BS Medical Technology student was asked to determine the molecular weight of a diprotic acid using acid-base titration. This student performed fourtrials. Firstly, the student used potassium hydrogen phthalate (KHP, 204.22 g/mol) as standard to determine the exact concentration of the NaOHtitrant. The results of the student are summarized in the table below:Note: The stoichiometric relationship of KHP to NaOH is 1:1Standardization Trial 1 Trial 2 Trial 3 Trial 4KHP Mass, g 0.5033 0.5066 0.6989 0.6843Volume NaOH used, mL 24.32 25.61 24.67 24.56After the standardization, the student weighed different amounts of the unknown acid. In a similar fashion, the student performed acid-base titrationusing phenolphthalein as indicator. The results of the molecular weight determination are summarized below:Note: The stoichiometric relationship of Unknown acid to NaOH is 1:2Molecular WeightDeterminationTrial 1 Trial 2 Trial 3 Trial 4Unknown Mass, g 0.1234 0.1034 0.1178 0.1322Volume NaOH used, mL…
Analytic chemistry.How to test the Na+ in the original solution? and NH4+?
I need help calculating the concentration of acid in each buffer solution show in the second picture!!!! ALSO - make sure for the unrounded values there is 6 sig figs!! EXPERIMENTAL DATA Sample HIn (mL) 1.10 M Acetic Acid (mL) 0.90 M Sodium Acetate (mL) 1 10.00 8.00 2.00 2 10.00 7.00 3.00 3 10.00 6.00 4.00 4 10.00 5.00 5.00 5 10.00 4.00 6.00 6 10.00 3.00 7.00 7 10.00 2.00 8.00 8 10.00 1.00 9.00 9 10.00 10.00 mL NaOH (0.10 M) 10 10.00 10.00 mL HCl (0.10 M)
While preparing the samples for analysis, you forgot that you already added phenolphthalein indicator so you added some more. What will be its effect in the volume of the titrant needed to reach the endpoint? Select one: A. Increase B. Decrease C. No effect D. Cannot be determined Primary standards are used to determine the exact concentration of the titrant. Based on the criteria of primary standards, which of the following cannot be used as a primary standard? Select one: A.Oxalic acid B. Sodium hydroxide C. Sodium carbonate D. Potassium dichromate During titration, you notice that the retention of the faint pink color is longer than earlier. Your lab partner suggested that you add a “half-drop” to prevent over-titration of the analyte solution. Is it ethical to do the “half-drop” technique? Select one: A. NO. It will cause error in calculations if you forgot to record the volume reading before adding the half-drop. B. YES. No error in calculations will be encountered provided…
Volumetric Analysis In Part A, a drop of the NaOH titrant adheres to the side of the buret (because of a dirty buret) between the initial and final readings for the titration. As a result of the “clean glass” error, how will the calculated molar concentration of the NaOH solution be affected?
Trial 1: Initial pH= 3.92mL Mass of KHP and Paper= 0.868g Mass of paper= 0.357g Mass of KHP= 0.511g Trial 2: Initial pH= 4.09ml Mass of KHP and Paper= 0.870g Mass of paper= 0.359g Mass of KHP= 0.511g 1)Use Kb, the number of moles of C8H4O4^2- at the equivalence point, and the total volume at that point to calculate the pH for each sample at the equivalence point. Compare these calculated results with the experimental results.