Suppose your laboratory instructor gave you a sample of KHP contaminated with NaCl to standardize vour NaOH in the first part of Experiment 15. Which of the following statements are true (select all that apply)? The volume of NaOH(aq) required to reach the equivalence point would be larger than if the contaminant were not present The volume of NaOH(aq) required to reach the equivalence point would be smaller than if the contaminant were not present The volume of NAOH(aq) required to reach the equivalence point would not be affected by the contaminant The molarity of the NaOH would be higher than the correct molarity The molarity of the NaOH would be lower than the correct molarity The molarity of the NaOH would be unaffected (same as the correct molarity)

Suppose your laboratory instructor gave you a sample of KHP contaminated with NaCl to standardize vour NaOH in the first part of Experiment 15. Which of the following statements are true (select all that apply)? The volume of NaOH(aq) required to reach the equivalence point would be larger than if the contaminant were not present The volume of NaOH(aq) required to reach the equivalence point would be smaller than if the contaminant were not present The volume of NAOH(aq) required to reach the equivalence point would not be affected by the contaminant The molarity of the NaOH would be higher than the correct molarity The molarity of the NaOH would be lower than the correct molarity The molarity of the NaOH would be unaffected (same as the correct molarity)

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

Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the solution pH before the titration begins? (Two decimal places) Type your answer...
If you perform this experiment with a titrant of 0.5M NaOH , would you expect your results in Data Table 2 to change or stay the same? Explain the answer.
Which of the following is true of a buffer solution that contains equivalent amounts of acid and conjugate base? The pH will always be greater than 7, regardless of the acid and conjugate base. The pH of the solution will be equal to the pKa of the acid. The pH of the solution will be equal to Kw. The pH will be equal to the concentration of the conjugate base. The pH will be equal to the concentration of the acid.
Question 2: lab on thermodynamic data for the dissolution of borax
Volume of acetic acid (HC2H3O2) in the first titration (L) 10 mL Volume of acetic acid (HC2H3O2) in the second titration (L) 10 mL Normality of sodium hydroxide (NaOH) (N) 0.1 N Volume of sodium hydroxide (NaOH) in the first titration (L) 10 mL = ……..L Volume of sodium hydroxide (NaOH) in the second titration (L) 10 mL = ……..L Normality of acetic acid (HC2H3O2) in the first titration (N) Normality of acetic acid (HC2H3O2) in the secondtitration (N) Average normality of acetic acid (HC2H3O2) (N) Mass % of acetic acid (HC2H3O2) (%)
When 30.00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the pH increases. - Find the pH when the volume of NaOH added is 0.02 mL less than the volume required to reach the equivalence point. - Find the pH when the volume of NaOH added is 0.01 mL less than the volume required to reach the equivalence point.
Calculate the amount of 6M HCl required to neutralize the solutions in beakers #1 and #2. Note: Saturated NaHCO3 has a concentration of about 1.1M. (use the last page for your calculations)
You measure 0.210 gram of unknown diprotic acid into a beaker. You add distilled water and a chemical indicator. You slowly add titrant 0.100M NaOH acid solution. Your first equivalence point is reached after 15mL NaOH has been added. The second equivalence point is reached after 30.0mL. WHat is the molar mass of the unkown diprotic acid?
Please only answer the question below. The questions shown are already solved, you don’t need to add anything, they are there for context. 3) Calculate the [Ba2+] left in solution when Ca2+ starts to precipitate. Then calculate the % of the original Ba2+ left in solution when Ca2+ starts to precipitate. A) 1.1 • 10^-2 % B) 2.8 • 10^-7 % C) 9.3 • 10^-3 % D) 6.7 • 10^-3 % E) 5.6 • 10^-3 %
Graph the following titration data and determine if the acid is monoprotic, diprotic, or triprotic. acid 1 acid 3 Volume (mL) 0.0 1.30 1.0 1.35 2.0 1.60 2.15 4.0 3.57 4.2 5.00 4.5 6.05 5.0 6.50 5.5 6.72 6.0 7.00 7.0 11.10 7.5 12.46 8.0 13.51 9.0 13.89 9.5 14.00 10.0 14.00 N 3.0 Talolo PH PH d. acid 2 Volume (ml) Hint: Monoprotic: has only 1 inflection Diprotic: has 2 inflections Triprotic: has 3 inflections 0 1 PH 1.01 1.32 1.59 5 10 2.23 12.4 3.56 12.5 7.00 12.6 10.44 13. 11.10 Volume of titrant added (mL) monoprotic a. acid1: monoprotic, acid2: diprotic, acid3: triprotic b. acid1: diprotic, acid2: monoprotic, acid3: triprotic c. acid1: diprotic, acid2: triprotic, acid3: monoprotic acid1: triprotic, acid2: monoprotic, acid3: diprotic e. acid1: triprotic, acid2:diprotic, acid3: monoprotic Volume (mL) pH pH 0.00 2.10 1.00 2.50 1.50 4.20 2.00 4.50 2.50 4.70 3.00 5.00 3.50 6.60 4.00 6.70 4.50 5.00 5.50 6.00 9.70 6.50 9.80 7.00 10.10 7.50 10.50 8.00 10.70 7.00 7.40 7.80 Volume of titrant…
Question 6 (1 point) 14 12 10 8 PH 00 6 4 2 0 0 20 40 60 volume added (mL) Consider the graph. What type of titration does it represent? A strong base titrated with a strong acid. A weak acid titrated with a strong base. A weak base titrated with a strong acid. A strong acid titrated with a strong base.
Determine the concentration of H2SO4 when 10 mL of the surround water was collected near the C & H Sugar Company. Your sample was titrated with 5 ml of 0.5 Molar NaOH solution to neutral the pH. Determine the concentration of H2SO4 in your water sample.