A buffer is made up of 15.0 mL of 0.1 M HC,H,02 and 15.0 mL of 0.1 MNa CH3O2 The solution is diluted with 30.0 mL of water. Five drops of 0.1 M HCl is added. What was observed to happen to the pH and why? O pH increases by 0.1, because OH minus leading to a small increase in pH. reacts with some of the conjugate acid O pH decreases by 0.1, because H* reacts with some of the conjugate base leading to a small decrease in pH. O pH decreases by 7, because OH minus reacts with all of the conjugate acid leading to a large decrease in pH. O pH decreases by 7, because H* reacts with all of the conjugate base leading to a large decrease in pH. O pH increases by 7. because OH minus reacts with all of the conjugate acid leading to a large increase in pH. pH increases by 7, because H* reacts with all of the conjugate base leading to a large increase in pH. O pH decreases by 0.1, because OH minus reacts with some of the conjugate acid leading to a small decrease in pH. O pH increases by 0.1. because H* reacts with some of the conjugate base leading to a small increase in pH.

A buffer is made up of 15.0 mL of 0.1 M HC,H,02 and 15.0 mL of 0.1 MNa CH3O2 The solution is diluted with 30.0 mL of water. Five drops of 0.1 M HCl is added. What was observed to happen to the pH and why? O pH increases by 0.1, because OH minus leading to a small increase in pH. reacts with some of the conjugate acid O pH decreases by 0.1, because H* reacts with some of the conjugate base leading to a small decrease in pH. O pH decreases by 7, because OH minus reacts with all of the conjugate acid leading to a large decrease in pH. O pH decreases by 7, because H* reacts with all of the conjugate base leading to a large decrease in pH. O pH increases by 7. because OH minus reacts with all of the conjugate acid leading to a large increase in pH. pH increases by 7, because H* reacts with all of the conjugate base leading to a large increase in pH. O pH decreases by 0.1, because OH minus reacts with some of the conjugate acid leading to a small decrease in pH. O pH increases by 0.1. because H* reacts with some of the conjugate base leading to a small increase in pH.

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 57P

See similar textbooks

Similar questions

Without doing detailed calculations, sketch the curve for the titration of 30.0 mL of 0.10 M NaOH with 0.10 M HCl. Indicate the approximate pH at the beginning of the titration and at the equivalence point. What is the total solution volume at the equivalence point?
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.
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.
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
Two drops of indicator HIn (Ka = 1.0 109), where HIn is yellow and In is blue, are placed in 100.0 mL of 0.10 M HCl. a. What color is the solution initially? b. The solution is titrated with 0.10 M NaOH. At what pH will the color change (yellow to greenish yellow) occur? c. What color will the solution be after 200.0 mL NaOH has been added?
How many grams of NaF must be added to 70.00 mL of 0.150 M HNO3 to obtain a buffer with a pH of 4.68?
A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.
Define a buffer solution. What makes up a buffer solution? How do buffers absorb added H+ or OH with little pH change? Is it necessary that the concentrations of the weak acid and the weak base in a buffered solution be equal? Explain. What is the pH of a buffer when the weak acid and conjugate base concentrations are equal? A buffer generally contains a weak acid and its weak conjugate base, or a weak base and its weak conjugate acid, in water. You can solve for the pH by setting up the equilibrium problem using the K.a reaction of the weak acid or the Kb reaction of the conjugate base. Both reactions give the same answer for the pH of the solution. Explain. A third method that can be used to solve for the pH of a buffet solution is the HendersonHasselbalch equation. What is the HendersonHasselbalch equation? What assumptions are made when using this equation?
A buffer solution is prepared from 5.15 g NH4NO3 and 0.10 L of 0.15-M NH3; calculate the pH of the solution.
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
The titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major species in solution at points AF. b. Calculate the pH at the halfway points to equivalence, B and D. (Hint: Refer to Exercise 113.)