Assume that you are right-handed and are performing a titration with a burette. For proper technique, you should be using O a. your left hand to control the stop-cock, making sure the stop-cock is on the same side as your dominant hand. O b.your right hand to control the position of the stop-cock, keeping your left hand free to swirl the Erlenmeyer flask. O. both hands to control the stop-cock position, and you must position your line-of-sight at 45 degrees to the burette. O d. both hands to carefully control the position of the stop-cock because you want to ensure that you do not miss the endpoint of the titration.

Assume that you are right-handed and are performing a titration with a burette. For proper technique, you should be using O a. your left hand to control the stop-cock, making sure the stop-cock is on the same side as your dominant hand. O b.your right hand to control the position of the stop-cock, keeping your left hand free to swirl the Erlenmeyer flask. O. both hands to control the stop-cock position, and you must position your line-of-sight at 45 degrees to the burette. O d. both hands to carefully control the position of the stop-cock because you want to ensure that you do not miss the endpoint of the titration.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 10P

See similar textbooks

Similar questions

Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink in the base form (pH 10.0). It is a weak acid with a pKa of 8.7. What fraction is in the acid form when the acid color is apparent? What fraction is in the base form when the base color is apparent?
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.
Instructions: Refer to the photo below. Answer the ff: a. Start of the titration b. Before equivalence point
Why you can't always use M1V1 = M2V2 in all titration problems?
Given an unknown solid mixture of NaCl and Na2CO3, determine the mass percent of each compound via titration. I'm given 0.1 M HCl standard solution and bromocresol green pH indicator, as well as standard lab equipment including a buret. What would the procedure for this look like? Will upvote
Sample containing arsenic weighing 0.800 are titrated with a standard iodine soluton. what should be the normality of the iodine in order that each ml of titrant represents 1/2% As2O3 in the sample (Answer: 0.0809 N show full solution please)
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
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 a successful trial. c) Add a couple drops of phenolphthalein into the buret to turn the sodium hydroxide solution dark pink. That will really make your instructor happy.......right? d) Add a couple drops of phenolphthalein into the acid flask. If it remains clear, nothing's wrong. If it changes to dark pink, I guess you need to restart! e) Add a couple drops of phenolphthalein into the acid flask just for the heck of it. You need to restart anyways, but why not have some fun?
If you think carefully about what happens during the course of aweak acid–strong base titration, you can learn some very interestingthings. For example, let’s look back at Figure 17.9 and pretendyou did not know that acetic acid was the acid being titrated. Youcan figure out the pKa of a weak acid just by thinking about thedefinition of Ka and looking at the right place on the titrationcurve! Which of the following choices is the best way to do this? (a) At the equivalence point, pH = pKa. (b) Halfway to theequivalence point, pH = pKa. (c) Before any base is added,pH = pKa. (d) At the top of the graph with excess base added,pH = pKa.
Advantages of potentiometric titrations over 'classical' visual indicator methods: (select the correct statement(s)). Can be used for colored, turbid or fluorescent analyte solution. Can be used if there is no suitable indicator or if the color change is difficult to visualize. Both answers 1 and 2 are correct
A student performs this experiment but forgets to remove air bubbles from the NaOH buret valve. (a) Would the measured volume of NaOH added in the back-titration be incorrectly high or low? (b) How would this error affect the results of the experiment? Question 2 options: (a) incorrectly low (b) % CaCO3 incorrectly high (a) incorrectly high (b) % CaCO3 incorrectly high (a) incorrectly low (b) % CaCO3 incorrectly low (a) incorrectly high (b) % CaCO3 incorrectly low
Moles SCN- used in titration (mol)Moles of Agt in 20.0 mL titrated (mol) [Ag*lequil (M)X= [Ag*Jinit - [Ag*lequil = Change (M) solve for flask d e and f