Strong acid and strong base Strong acid and weak base C. Weak acid and their conjugate base D. Weak base and their conjugate acid a solution has to be a buffer, its pH should be a buffer, it's pH should be At 7 C. At is Ka value D. At its pKa value At 14 hat is the pH of a solution composed of 0.20 M NH3 and 0.15 M NH&CI? 2.15 C. 8.26 D. 9.38 4.62 hich of the following is the correct representation of Henderson – Hasselbalch uation? [A] = pK. +lo$HA] C. pH = pK – log [proton donor] [proton acceptor] H = proton acceptor] E. pH = pka+ log [protondonor] D. All of the above cording to Henderson-Hasselbalch equation, when the pH of a solution comes equal to its pKa, the solution becomes a buffer This condition is hieved when Concentration of proton donor become zero. Concentration of proton acceptor become zero. The concentration of proton donor equals the concentration of proton ceptor. The concentration of proton donor become log 1/10th of concentration of pton acceptor. trogen has the same oxidation number in all of the following EXCEPT_
Strong acid and strong base Strong acid and weak base C. Weak acid and their conjugate base D. Weak base and their conjugate acid a solution has to be a buffer, its pH should be a buffer, it's pH should be At 7 C. At is Ka value D. At its pKa value At 14 hat is the pH of a solution composed of 0.20 M NH3 and 0.15 M NH&CI? 2.15 C. 8.26 D. 9.38 4.62 hich of the following is the correct representation of Henderson – Hasselbalch uation? [A] = pK. +lo$HA] C. pH = pK – log [proton donor] [proton acceptor] H = proton acceptor] E. pH = pka+ log [protondonor] D. All of the above cording to Henderson-Hasselbalch equation, when the pH of a solution comes equal to its pKa, the solution becomes a buffer This condition is hieved when Concentration of proton donor become zero. Concentration of proton acceptor become zero. The concentration of proton donor equals the concentration of proton ceptor. The concentration of proton donor become log 1/10th of concentration of pton acceptor. trogen has the same oxidation number in all of the following EXCEPT_
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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
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![1) Buffers are mixtures of
A. Strong acid and strong base
B. Strong acid and weak base
C. Weak acid and their conjugate base
D. Weak base and their conjugate acid
2) If a solution has to be a buffer, its pH should be a buffer, it's pH should be
A. At 7
B. At 14
C. At is Ka value
D. At its pka value
3) What is the pH of a solution composed of 0.20 M NH3 and 0.15 M NH&CI?
A. 2.15
С. 8.26
B. 4.62
D. 9.38
4) Which of the following is the correct representation of Henderson – Hasselbalch
equation?
А.
С.
[A]
pH = pKa+ log-
[HA]
[proton donor]
pH = pK. - log
[proton acceptor]
B. pH = pk, + log=
[proton acceptor]
[proton donor]
D. All of the above
5) According to Henderson-Hasselbalch equation, when the pH of a solution
becomes equal to its pKa, the solution becomes a buffer This condition is
achieved when
A. Concentration of proton donor become zero.
B. Concentration of proton acceptor become zero.
C. The concentration of proton donor equals the concentration of proton
acceptor.
D. The concentration of proton donor become log 1/10th of concentration of
proton acceptor.
6) Nitrogen has the same oxidation number in all of the following EXCEPT_
A. NO3
B. N2O5
C. NH&CI
D. Ca(NO3)2
7) What is the oxidizing agent in the reaction: 2Na + 2H20 → 2NAOH + H2
A. Na
В. На
C. H2O
D. NaOH
8) What does Sn** → Sn2* represents?
A. Hydrolysis
B. Oxidation
C. Reduction
D. None of the above
16
9) What is the oxidation number of sulfur in H2SO3?
A. +1
В. +2
С. +3
D. +4
10) Which of the following is a redox reaction?
A. 2KBR + F2 → 2KF + Br2
B. 2HCI + Mg(OH)2 → 2H20 + MgCl2
C. 2NACI + H2SO4 → NazSO4 + 2HCI
D. Ca(OH)2 + Pb(NO3)2 → Ca(NO3)2 + Pb(OH)2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fab7d4da2-e2dc-4e4a-8e30-5463dee45524%2F1ee4c0e8-2f30-4826-89a0-c3bc03bab201%2Flw2u6a9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1) Buffers are mixtures of
A. Strong acid and strong base
B. Strong acid and weak base
C. Weak acid and their conjugate base
D. Weak base and their conjugate acid
2) If a solution has to be a buffer, its pH should be a buffer, it's pH should be
A. At 7
B. At 14
C. At is Ka value
D. At its pka value
3) What is the pH of a solution composed of 0.20 M NH3 and 0.15 M NH&CI?
A. 2.15
С. 8.26
B. 4.62
D. 9.38
4) Which of the following is the correct representation of Henderson – Hasselbalch
equation?
А.
С.
[A]
pH = pKa+ log-
[HA]
[proton donor]
pH = pK. - log
[proton acceptor]
B. pH = pk, + log=
[proton acceptor]
[proton donor]
D. All of the above
5) According to Henderson-Hasselbalch equation, when the pH of a solution
becomes equal to its pKa, the solution becomes a buffer This condition is
achieved when
A. Concentration of proton donor become zero.
B. Concentration of proton acceptor become zero.
C. The concentration of proton donor equals the concentration of proton
acceptor.
D. The concentration of proton donor become log 1/10th of concentration of
proton acceptor.
6) Nitrogen has the same oxidation number in all of the following EXCEPT_
A. NO3
B. N2O5
C. NH&CI
D. Ca(NO3)2
7) What is the oxidizing agent in the reaction: 2Na + 2H20 → 2NAOH + H2
A. Na
В. На
C. H2O
D. NaOH
8) What does Sn** → Sn2* represents?
A. Hydrolysis
B. Oxidation
C. Reduction
D. None of the above
16
9) What is the oxidation number of sulfur in H2SO3?
A. +1
В. +2
С. +3
D. +4
10) Which of the following is a redox reaction?
A. 2KBR + F2 → 2KF + Br2
B. 2HCI + Mg(OH)2 → 2H20 + MgCl2
C. 2NACI + H2SO4 → NazSO4 + 2HCI
D. Ca(OH)2 + Pb(NO3)2 → Ca(NO3)2 + Pb(OH)2
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