Why is it important not to add too much HCI and go past the endpoint? O The volume of acid added will be lower than expected for the calculations. O The color change can reverse. O The solution could bubble out of the flask. O The volume of acid added will reflect more than acid required to neutralize the base. U

Why is it important not to add too much HCI and go past the endpoint? O The volume of acid added will be lower than expected for the calculations. O The color change can reverse. O The solution could bubble out of the flask. O The volume of acid added will reflect more than acid required to neutralize the base. U

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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Which of the following statements concerning acid-base indicators is true? Select one: a. All the above statements are true. O b. Acid-base indicators are derived from weak acids. O c. Only small quantities of indicators are added to a solution. O d. The acid and base forms of indicator are different colours.
If 8.00 mL of a different hydrochloric acid solution had a known concentration of 0.3456 M, how many mL of the 0.1679M NaOH solution would be required to reach the equivalence point?(3 sig figs)
A student titrates a weak acid with 0.100M NaOH, adding 35.64 mL before a dark pink color is seen. Realizing that the end point has been passed, he then adds 2.77 mL 0.0500 M HCI until the solution is neutralized. How many moles of H* were present in the initial weak acid solution? Type answer:
Find the normality of sodium carbonate (molar mass = 106) in a solution containing 0.212 g carbonate in 100 ml solution if the carbonate is used as a dibasic base means it has 2 OH-.
if a substance changes color at a higher ph but acids neutralize at a lower ph, would that affect the results of an experiment?
I The endpoint of an acid-base titration is defined as the point where O A. The amount (moles) of acid and base present are equivalent and a physio-chemical change occurs. O B. All the base added from the burette is used up. O C. Excess titrant is present. O D. The number of moles of acid and base are equal.
If 8.00 mL of a different hydrochloric acid solution had a known concentration of 0.3456 M, how many mL of the 0.1232M NaOH solution would be required to reach the equivalence point? (3 sig figs)
How many grams of NaF (41.98817 g/mol) would have to be added to 2.00 L of 0.100 M HF (20.01 g/mol) to yield a solution with a pH of 4.00. The pKa of HF is 3.80?
How can you define an indicator? ( for acid and base solutions )
Determine which of the following statements is/are FALSE: Statement 1: The endpoint is when all the analyte has reacted with a small excess of titrant Statement 2: At the endpoint, the concentration of analyte will be slightly artificially high Statement 3: According to the image below, the titrant needs to be added dropwise in Figure 2 L L L L 1 2 3 4 Select one: Only statement 2 Only statement 3 Statements 1 and 3 Statements 1 and 2 Statements 2 and 3
What is the concentration of an HNO3 solution in percent by mass that was determined to have a concentration of 0.669 M in a titration experiment? Assume a density of 1.00 g/mL. Your Answer: Answer units Previous Page Next Page Page 4 of 15
Do the 2nd and 3rd questions according to the table below. Indicator Acid color Color change, pH range Base color Methyl orange Red 3.1-4.5 Yellow Brome tymol blue Yellow 6.0-7.6 Blue 2) When the above-mentioned indicators are dropped into the two separate 10* M HCI solution, what will the color of solutions be respectively? A. Red, blue B. Red, yellow C. Yellow, yellow D. Yellow, blue E. Orange, green 3) When the above-mentioned indicators are dropped into the two separate 10 M NAOH solution, what will the color of solutions be respectively? A. Red, blue B. Red, yellow C. Yellow, yellow D. Yellow, blue E. Orange, green В. When the above-mentioned indicators are dropped into the 0.1 M NH3, what will the color of solution be? K, for NH3: 1x105