Question

1. If the hydroxide concentration is 7.24 x 10-³M is the solution acidic or basic?

2. If the [OH-] concentration is 2.8 x 10-7M is the solution acidic or basic?

3. If the concentration of [H] is 5.10 x 10-6M, what is the [OH-] concentration and is the solution acidic or basic?

4. If the [H3O+] concentration is 3.89 x 10-M is the solution acidic or basic? What is the [OH-] concentration?

5. Is a solution with a hydroxide concentration of 4.88 x 10-6M acidic or basic?

6. Find the hydronium ion concentration of a solution with a [OH-] concentration of 8.13 x 10-4M.

7. What is the pH of a solution with a pOH of 5.19?

8. Find the pOH of a solution with a pH of 3.78. Is this solution acidic or basic?

9. Find the hydroxide ion concentration of a solution with a [H₂O*] concentration of 9.22 x 10-8 M.

10. Is a solution with a [OH-] concentration of 5.39 x 10-12 acidic, basic, or neutral?​

Answer 1

1. If the hydroxide concentration is 7.24 x 10-³M, the solution is basic.

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2. If the [OH-] concentration is 2.8 x 10-7M, the solution is basic.

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3. If the concentration of [H+] is 5.10 x 10-6M, we can use the equation for the ion product of water to find the [OH-] concentration. The ion product of water, Kw, is equal to [H+][OH-] and has a constant value of 1.0 x 10-14 at 25°C. Rearranging the equation, we have [OH-] = Kw / [H+]. Plugging in the given values, we get [OH-] = (1.0 x 10-14) / (5.10 x 10-6) ≈ 1.96 x 10-9M. Therefore, the [OH-] concentration is approximately 1.96 x 10-9M, and the solution is basic.

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4. If the [H3O+] concentration is 3.89 x 10-M, the solution is acidic. To find the [OH-] concentration, we can use the equation [H3O+][OH-] = Kw. Rearranging the equation, we have [OH-] = Kw / [H3O+]. Plugging in the values, we get [OH-] = (1.0 x 10-14) / (3.89 x 10-M) ≈ 2.57 x 10-12M. Therefore, the [OH-] concentration is approximately 2.57 x 10-12M.

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5. A solution with a hydroxide concentration of 4.88 x 10-6M is basic.

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6. To find the hydronium ion (H3O+) concentration from the [OH-] concentration, we can use the equation [H3O+][OH-] = Kw. Rearranging the equation, we have [H3O+] = Kw / [OH-]. Plugging in the given values, we get [H3O+] = (1.0 x 10-14) / (8.13 x 10-4) ≈ 1.23 x 10-11M. Therefore, the hydronium ion concentration is approximately 1.23 x 10-11M.

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7. The pH of a solution can be calculated from the pOH using the equation pH + pOH = 14. Given that the pOH is 5.19, we can subtract it from 14 to find the pH. Therefore, the pH is 14 - 5.19 = 8.81.

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8. The pOH of a solution can be calculated from the pH using the equation pH + pOH = 14. Given that the pH is 3.78, we can subtract it from 14 to find the pOH. Therefore, the pOH is 14 - 3.78 = 10.22. This solution is basic because the pOH is greater than 7.

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9. The concentration of [H₂O*] provided is incorrect because water is not an ionic species, so it does not have a concentration of its own. Please verify the correct concentration of an ion or molecule.

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10. A solution with an [OH-] concentration of 5.39 x 10-12 is acidic because the hydroxide ion concentration is very low.