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3 years ago

13. Which could be true about an unknown sample with a pH of 7? (2 points)

Chemistry

2 answers:

Rasek [7]3 years ago

7 0

Answer: Option (a) is the correct answer.

Explanation:

Substance which show pH less than 7 are acidic in nature. For example, HCl being a strong acid has pH very less than 7.

Substances which show pH greater than 7 are basic in nature. For example, NaOH being basic in nature has pH greater than 7.

Whereas substances which have pH equal to 7 are neutral in nature, that is, they are neither acidic nor basic.

For example, water is neutral in nature.

Thus, we can conclude that the statement it contains only water is true about an unknown sample with a pH of 7.

laiz [17]3 years ago

5 0

The best and most correct answer among the choices provided by your question is the first choice or letter A.

A ph of 7 contains only water.

I hope my answer has come to your help. Thank you for posting your question here in Brainly. We hope to answer more of your questions and inquiries soon. Have a nice day ahead!

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bija089 [108]

Answer: The value of $K_c$ for the net reaction is $\frac{K_b}{K_w}$

Explanation:

The given chemical equations follows:

Equation 1: $B(aq.)+H_2O(l)\rightleftharpoons HB^+(aq.)+OH^-(aq.);K_b$

Equation 2: $H^+(aq.)+OH^-(aq.)\rightleftharpoons H_2O(l);\frac{1}{K_w}$

The net equation follows:

$B(aq.)+H^+(aq.)\rightleftharpoons HB^+(aq.);K_c$

As, the net reaction is the result of the addition of first equation and the second equation. So, the equilibrium constant for the net reaction will be the multiplication of first equilibrium constant and the second equilibrium constant.

The value of equilibrium constant for net reaction is:

$K_c=K_1\times K_2$

We are given:

$K_1=K_b$

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Putting values in above equation, we get:

$K_c=K_b\times \frac{1}{K_w}=\frac{K_b}{K_w}$

Hence, the value of $K_c$ for the net reaction is $\frac{K_b}{K_w}$

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3 years ago