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pH worksheet (#1)

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**1. What is the pH of a solution with a hydrogen ion concentration of 1**

1. What is the pH of a solution with a hydrogen ion concentration of 1.0 x 10-5 M? pH = -log [H+] = - log (1.0 x 10-5 ) = 5

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**2. What is the pH of a solution with a hydrogen ion concentration of 4**

2. What is the pH of a solution with a hydrogen ion concentration of 4.5 x 10-8 M? pH = -log [H+] = - log (4.5 x 10-8 ) = 7.34

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**3. What is the pOH of a solution with a hydrogen ion concentration of 1.0 x 10-10 M?**

pH = -log [H+] = - log (1.0 x ) = 10 Now use: pH + pOH = 14 14 – 10 = 4, so the pOH = 4

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**We need to use: pOH = - log [OH-]**

4. What is the pOH of a solution with a hydroxide ion concentration of 1.0 x M? We need to use: pOH = - log [OH-] pOH = - log [1.0 x ] pOH = 10

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**5. What is the hydroxide ion concentration in a solution with a pH of 5?**

pH = - log [ H+] - pH = log [ H+] 10x (- pH) = 10x log [ H+] 10x (- 5) = 10x log [ H+] 10-5 = [ H+] = 1.0 x M

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**This is our [H+], we need [OH-]**

We need to use: [H+] x [OH-] = 1.0 x M [1.0 x M] x [OH-] = 1.0 x M [1.0 x M] [1.0 x M] = 1.0 x 10 -9

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**6. What is the hydrogen ion concentration in a solution with a pH of 9**

pH = - log [ H+] - pH = log [ H+] 10x (- pH) = 10x log [ H+] 10x (- 9.7) = 10x log [ H+] = [ H+] = 2.0 x M

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**7. What is the hydronium ion concentration of a solution with a pH of 2.5?**

pH = - log [ H+] - pH = log [ H+] 10x (- pH) = 10x log [ H+] 10x (- 2.5) = 10x log [ H+] = [ H+] = 3.2 x M

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