Select ALL the steps you must take (but do not select any steps that are not essential) when you are preparing to do an acid-base titration (for example HCI titrated with NaOH). Select one or more: O a. Check if funnel is in top of burette, and if so, remove it. V b. Check for and, if necessary, remove air bubble from under tap. O c. Adjust liquid level in the burette to exactly 0.0 mL. O d. Remove burette from clamp to fill it with liquid. е. Add indicator to solution in flask.

Select ALL the steps you must take (but do not select any steps that are not essential) when you are preparing to do an acid-base titration (for example HCI titrated with NaOH). Select one or more: O a. Check if funnel is in top of burette, and if so, remove it. V b. Check for and, if necessary, remove air bubble from under tap. O c. Adjust liquid level in the burette to exactly 0.0 mL. O d. Remove burette from clamp to fill it with liquid. е. Add indicator to solution in flask.

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...

See similar textbooks

Similar questions

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.
Which Cl determination method describes a back titration relying on blood red precipitate formation? a. Mohr method b. Volhard method c. Fajan d. Liebig
Chemistry Given an unknown solid mixture of NaCl and Na2CO3, determine the mass percent of each compound via titration. I'm given 0.1 M HCI 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
Note: Detailed explanations and complete solutions are not needed. A 0.2101 g of unknown organic acid used 14.00 mL and 28.00 mL of 0.1000 N NaOH to reach the first and second equivalence point, respectively during potentiometric titration. Calculate the MW of the unknown acid. a. 75.04 g/mol b. 37.52 g/mol c. 150.1 g/mol d. 225.1 g/mol
Can you help me with d and e? Thank you!
titration curve in acid-base titration is: a. less steep curve for strong analyte versus strong titrant than weak ones b. all acid-base indicator are suitable for use c. the end point does not necessary match pH=7 for all types of acid and base analytes d. weak acid can be used for titrating weak bases
1. How to pick the best indicator for any titration? a. The one that is pink, if the solution is acidic b. The one that is blue if the solution is basic c. The one with pKa of the solution = pH (predicted at the equivalence point) d. It's a trial and error procedure e. None of the above
need both 2 parts soon in detail don't copy I. will downvote
Solve for the pH value when 200 mL of 0.02 M NH3 was titrated with each titrant. a.) 25 mL of 0.05 M HI b.) 80 mL of 0.05 M HI c.) 100 mL of 0.05 M HI Note: The value of Kb is 1.8 x 10-5
acetic acid is a: ______ strong acid, strong base, weak acid, or weak base?? (Circle one) What should be the equivalence point pH be for this experiment? less than 7, equal to 7, pr greater than 7?? (Circle one) Why is the half-equivalence pH (and half-equivalence volume) important in this titration? Explain. From the graph, estimate the half-equivalence volume: ________________ mL From the graph, estimate the half-equivalence pH: ________________ Using these values, calculate the value of Ka for acetic acid: ________________ Acetic acid has a known Ka of 1.8 x 10-5 via the literature. Find the percent error for this experiment. Recall: Percent error = absolute value{(actual - experimental)/ actual}*100%
Solve correctly please.
EXPERIMENT 10 PRE-LABORATORY QUESTIONS STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION NAME DATE 1. What is the purpose of this experiment? 2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this sample? 3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of KHP from the previous question? 4. If the initial volume of the NaOH in the burette was 0.50 mL and the final volume is shown to the right, what is the volume of NaOH used in this titration? 19 5. What is the concentration of the NaOH solution used in this titration? EXPERIMENT 10 155