Question

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?
7.4×10−3M
	3.6×10−10M
		8.26
			5.72

Answer 1

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 = 14-2.13 = 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 = 14-4.56 = 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 = 14-8.26 = 5.74

Given pOH = 5.72

As we know that

pH + pOH = 14

pH = 14- pOH = 14-5.72 = 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