Boxes 1-4 X: pH = 4.850 (this is the pH ofyour buffer)Y: 0.250 M(this is the total concentration, the sum ofthe concentrations of both conjugates)IMPORTANT: For all of your answers, enter:• Numbers only (no units)A leading zero before the decimal (only necessary ifthere are not any non-zero digits). 3 digits after the decimal (to the 1/1000 column,don't worry about significant figures)• Round only the last digit of you answer (beuse un-rounded numbers in all your calculations!)toExamples: 0.123 , 98.765Can you believe I just said no units and sig figs? These sure.are strange days!Your answers:What is the concentration of the conjugate acid in yourbuffer?M conj. acidWhat is the concentration of the conjugate base in your - Round only the last digit of you answer (be sure touse un-rounded numbers in all your calculations!)Examples: 0.123 , 98.765Can you believe I just said no units and sig figs? These sureare strange days!Your answers:What is the concentration of the conjugate acid in yourbuffer?M conj. acidWhat is the concentration of the conjugate base in yourbuffer?M conj. baseWhat is the volume of the aqueous solution required tomake 100.0 mL of the buffer?mL1.00 M solutionWhat is the mass of the solid salt required to make 100.0mL of the buffer?g salt

An acidic substance furnishes hydrogen ions in an aqueous solution and changed to its conjugate…

Answered: Boxes 1-4

Science

Chemistry

Boxes 1-4

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 7RQ: Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations...

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Concept explainers

Matter and Measurement

In the universe, there is matter, energy, and void space. The universe contains energy and void space. The definition of matter can be considered as something which possesses mass and consumes space. Chemistry is that branch of science which deals with the study of matter. Under chemistry, nature, composition, and the changes occurring to matter are discussed.

Question

Boxes 1-4

X: pH = 4.850 (this is the pH of
your buffer)
Y: 0.250 M
(this is the total concentration, the sum of
the concentrations of both conjugates)
IMPORTANT: For all of your answers, enter:
• Numbers only (no units)
A leading zero before the decimal (only necessary if
there are not any non-zero digits)
. 3 digits after the decimal (to the 1/1000 column,
don't worry about significant figures)
• Round only the last digit of you answer (be
use un-rounded numbers in all your calculations!)
to
Examples: 0.123 , 98.765
Can you believe I just said no units and sig figs? These sure.
are strange days!
Your answers:
What is the concentration of the conjugate acid in your
buffer?
M conj. acid
What is the concentration of the conjugate base in your

- Round only the last digit of you answer (be sure to
use un-rounded numbers in all your calculations!)
Examples: 0.123 , 98.765
Can you believe I just said no units and sig figs? These sure
are strange days!
Your answers:
What is the concentration of the conjugate acid in your
buffer?
M conj. acid
What is the concentration of the conjugate base in your
buffer?
M conj. base
What is the volume of the aqueous solution required to
make 100.0 mL of the buffer?
mL
1.00 M solution
What is the mass of the solid salt required to make 100.0
mL of the buffer?
g salt

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. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
A quantity of 0.25 M sodium hydroxide is added to a solution containing 0.15 mol of acetic acid. The final volume of the solution is 375 mL and the pH of this solution is 4.45. a What is the molar concentration of the sodium acetate? b How many milliliters of sodium hydroxide were added to the original solution? c What was the original concentration of the acetic acid?
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.

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