Part A
Complete the first row.
Express your answer using two significant figures.
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Part B
Complete the first row.
Express your answer using two decimal places.


[OH−] =  3.6•10.10  M 
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Part C
Complete the first row.
Express your answer using two decimal places.


pH =  8 
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Part D
Complete the first row. Indicate whether the solution is acidic or basic.
Complete the first row. Indicate whether the solution is acidic or basic.


pOH =  5.7 
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Correct
Part E
Complete the second row.
Express your answer using two significant figures.
acidic 
basic 
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Part F
Complete the second row.
Express your answer using two decimal places.


[H+] =  M 
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Part G
Complete the second row.
Express your answer using two decimal places.


pH = 
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Part H
Complete the second row. Indicate whether the solution is acidic or basic.
Complete the second row. Indicate whether the solution is acidic or basic.


pOH = 
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Part I
Complete the third row.
Express your answer using two significant figures.
acidic 
basic 
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Part J
Complete the third row.
Express your answer using two significant figures.


[H+] =  M 
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Part K
Complete the third row.
Express your answer using two decimal places.


[OH−] =  M 
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Part L
Complete the third row. Indicate whether the solution is acidic or basic.
Complete the third row. Indicate whether the solution is acidic or basic.


pOH = 
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Part M
Complete the fourth row.
Express your answer using two significant figures.
acidic 
basic 
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Part N
Complete the fourth row.
Express your answer using two significant figures.


[H+] =  M 
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Part O
Complete the fourth row.
Express your answer using two decimal places.


[OH−] =  M 
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Part P
Complete the fourth row. Indicate whether the solution is acidic or basic.
Complete the fourth row. Indicate whether the solution is acidic or basic.


pH = 
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Complete the following table by calculating the missing entries and indicating whether the solution is acidic or basic.
[H+]  [OH−]  pH  pOH  Acidic or basic? 
7.4×10^{−3}M  
3.6×10^{−10}M  
8.26  
5.72 
Expert Answer
Given [H+] = 7.4*10^3 M
As we know that
[H+] [OH] = 10^14
[OH] = (10^14)/[H+] = (10^14)/(7.4*10^3) = 1.35*10^12 M
pH = – log[H+] = – log(7.4*10^3) = 2.13 (acidic)
pH + pOH = 14
pOH = 14 pH = 142.13 = 11.87
Given [OH] = 3.6*10^10 M
As we know that
[H+] [OH] = 10^14
[H+] = (10^14)/[OH] = (10^14)/(3.6*10^10) = 2.77*10^5 M
pH = – log[H+] = – log(2.77*10^5) = 4.56 (acidic)
pH + pOH = 14
pOH = 14 pH = 144.56 = 9.44
Given pH = 8.26 (basic)
As we know that
pH = – log[H+]
8.26 = log[H+]
[H+] = 10^(8.26) = 5.5*10^9 M
[H+] [OH] = 10^14
[OH] = (10^14)/[H+] = (10^14)/(5.5*10^9) = 1.82*10^9 M
pH + pOH = 14
pOH = 14 pH = 148.26 = 5.74
Given pOH = 5.72
As we know that
pH + pOH = 14
pH = 14 pOH = 145.72 = 8.28 (basic)
pH = – log[H+]
8.28 = log[H+]
[H+] = 10^(8.28) = 5.25*10^9 M
[H+] [OH] = 10^14
[OH] = (10^14)/[H+] = (10^14)/(5.25*10^9) = 1.90*10^6 M