10.0 mL of NaOH solution with unknown concentration is titrated with 0.10 M of HCl solution in the presence of phenolphthalein indicator. At the end of the titration 15.0 mL of HCl solution is used. What is the number of millimoles and concentration of NaOH solution used? A. 1.5 mmol and 0.15 M NaOH B. 1.0 mmol and 0.15 M NaOH C. 1.5 mmol and 0.1 M NaOH D. 2.0 mmol and 0.1 M NaOH E. 1.0 mmol and 0.1 M NaOH

10.0 mL of NaOH solution with unknown concentration is titrated with 0.10 M of HCl solution in the presence of phenolphthalein indicator. At the end of the titration 15.0 mL of HCl solution is used. What is the number of millimoles and concentration of NaOH solution used? A. 1.5 mmol and 0.15 M NaOH B. 1.0 mmol and 0.15 M NaOH C. 1.5 mmol and 0.1 M NaOH D. 2.0 mmol and 0.1 M NaOH E. 1.0 mmol and 0.1 M NaOH

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

Please look at the graph weak acid/strong base titration curve. Answer the questions below. Fill in the blank with your response. Do not include any units in your answer. Acid-Base Titration 12 10 8. 6. 2. 4. 6. 8. 10 12 Volume (mL) A. The approximate pH at the equivalence point is (Please reply with a 2-digit answer) B. The approximate volume of base added at the equivalence point is mL. (Please reply with a 2-digit answer) C. The volume of base added when pH = pKa is mL. (Please reply with a 2-digit %3D answer) 2.
Question Completion Status: For Solution A, approximately how many mL of HCI were needed to exceed the buffering capacity of this solution? Enter the number only. Don't enter units as part of your answer and don't use commas or scientific notation. Titration curve of Solution A 14 13 12 11- 10 9 8 pH 7 6 5 4 3 2 1 5 4 3 2 1 HCI added (mL) 0 1 2 3 4 5 NaOH added (mL) 14 13 12- 11 10 9 8 pH 7 6.8 2 65 4 3 2 1 Titration curve of Solution B Click Save and Submit to save and submit. Click Save All Answers to save all answers. 54 32 1 HCI added (mL) 0123 NaOH added (mL)
Which of the following is true In an acid-base titration A. Water is never formed B. You are trying to make a precipitate C. Moles acid = moles base at the point of neutralization D. The pH will always be = to 7.0 at the neutralization point
Please don't provide handwritten solution ...
During the standardization of a titrant, it became reddish. What does this mean and how would that affect the titrant's molarity?
Explain the difference between an indicator endpoint for a titration analysis and the true equivalence point for the titration. Please simplify the answer so I can understand. Thanks
In the standardization of NaOH with potassium hydrogen phthalate (KHP). A known amount of KHP is weighed and dissolved in water. This is then titrated incrementally with NaOH from a buret until the phenolphthalein changes color from colorless to pink. Which is the titrand? a.cannot be determined form above scenario b.HCl c.NaOH d.phenolphthalein e.KHP
14 Given the hypothetical titration curves below, determine what curve has a stronger acid. 14 a. b. C. d. 12 10 8 6 4 () 0 Curve A Curve B Curve C Cannot be determined A B and C 10 20 30 40 50 60 Volume of 0.1000 M NaOH, mL
Determine the pH during the titration of 20.6 mL of 0.328 M perchloric acid by 0.206 M barium hydroxide at the following points:a.Before the addition of any barium hydroxide b.After the addition of 8.20 mL of barium hydroxide c. At the equivalence point d. After adding 20.8 mL of barium hydroxide
Which of the following insoluble salts are more soluble in a 0.10 hydrochloric acid solution than in a pure water solution? Chose all that apply a. Nickel (II) sulfide b. barium fluoride c. lead chloride d. lead bromide e. calcium fluoride f. silver sulfite
2)Make a rough plot of pH versus milliliters of acid added for the titration of 50.0 mL of 1.0 M NaOH with 1.0 M HCl. Indicate the pH at the following points and tell how many milliliters of acid are required to reach the equivalence point. a)Before the titration starts b)At the equivalence point c)After an additional 10.0 mL of HCL is added after the equivalence point (i.e. equivalence point volume + 10.0 mL)
A 0.025M solution of hydrochloric acid is titrated with 0.020M of sodium hydroxide. If 250mL of the acid requires 30.0mL of the base for neutralization, calculate the initial concentration of hydrochloric acid.