7. 15 mL of a 0.105 M solution of NaOH is titrated with 0.116 M of HCI solution. 5.0 mL of acid is added to the solution.What is the pH of the solution? 1.58 13.1 O 12.7 1.3 8. A 0.5M phosphate buffer at pH 7 was diluted to form a 0.045 M solution.What is the volume of the stock solution needed to prepare 2L of the diluted phosphate buffer solution? 0.18 L 2.22 L 22.2 L 0.045 L

7. 15 mL of a 0.105 M solution of NaOH is titrated with 0.116 M of HCI solution. 5.0 mL of acid is added to the solution.What is the pH of the solution? 1.58 13.1 O 12.7 1.3 8. A 0.5M phosphate buffer at pH 7 was diluted to form a 0.045 M solution.What is the volume of the stock solution needed to prepare 2L of the diluted phosphate buffer solution? 0.18 L 2.22 L 22.2 L 0.045 L

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 49P

See similar textbooks

Similar questions

When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)