Over much ofthe titrationcurve, the pHlies within 1 pHunit of the pka.In this range,the change inpH with molesof base addedis minimal.131211109876TO43210NHHCOOHNH3pk of NH4HCOOpk of HCOOH.525.75Moles base added per mole acidTitration curves of weak acids.1.0At the midpointof the titrationwhere half theacid isneutralized,pH=pKaPart ACalculate the pH of a 1.0 M NH4Cl solution. (Ką for NH4+ is5.62 × 10-10)Express your answer to two decimal places.pH =SubmitPart BpH =SubmitVO ΑΣΦCalculate the pH of the solution that results following addition of 10 mLof 1.0 M NaOH to 50 mL of 1.0 M NH₂ Cl.Express your answer to two decimal places.Part CRequest Answer5 ΑΣΦ?Request Answer?Calculate the pH of the solution that results following addition of 21 mLof 1.0 M NaOH to 50 mL of 1.0 M NH₂ Cl.Express your answer to two decimal places.

Given:Part A:Concentration of NH4Cl = Part B:For NH4Cl:For NaOH:Part C:For NH4Cl:For NOH:The pH of a…

Answered: Over much of the titration curve, the…

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...

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Question

Over much of
the titration
curve, the pH
lies within 1 pH
unit of the pka.
In this range,
the change in
pH with moles
of base added
is minimal.
13
12
11
10
9
8
7
6
TO
4
3
2
1
0
NH
HCOOH
NH3
pk of NH4
HCOO
pk of HCOOH
.5
25
.75
Moles base added per mole acid
Titration curves of weak acids.
1.0
At the midpoint
of the titration
where half the
acid is
neutralized,
pH=pKa
Part A
Calculate the pH of a 1.0 M NH4Cl solution. (Ką for NH4+ is
5.62 × 10-10)
Express your answer to two decimal places.
pH =
Submit
Part B
pH =
Submit
VO ΑΣΦ
Calculate the pH of the solution that results following addition of 10 mL
of 1.0 M NaOH to 50 mL of 1.0 M NH₂ Cl.
Express your answer to two decimal places.
Part C
Request Answer
5 ΑΣΦ
?
Request Answer
?
Calculate the pH of the solution that results following addition of 21 mL
of 1.0 M NaOH to 50 mL of 1.0 M NH₂ Cl.
Express your answer to two decimal places.

Expert Solution

Step 1: Given

Given:

Part A:

Concentration of NH₄Cl = $space 1.0 space straight M$

$straight K subscript straight a space of space NH subscript 4 superscript plus equals 5.62 cross times 10 to the power of negative 10 end exponent$

Part B:

For NH₄Cl:

$table row cell Concentration space end cell equals cell space 1.0 space straight M space end cell row cell Volume space end cell equals cell space 50 space mL end cell end table$

For NaOH:

$Concentration space equals space 1.0 space straight M space Volume space equals space 10 space mL$

Part C:

For NH₄Cl:

$table row cell space Concentration space end cell equals cell space 1.0 space straight M space end cell row cell Volume space end cell equals cell space 50 space mL end cell end table$

For NOH:

$table row cell Concentration space end cell equals cell space 1.0 space straight M space end cell row cell Volume space end cell equals cell space 21 space mL end cell end table$

The pH of a solution is determined using the negative logarithm of the hydrogen ion concentration (H⁺). The pH of a solution is a measure of its acidity or alkalinity on a logarithmic scale ranging from 0 to 14.

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