Question

What is the hydronium ion concentration in a solution of HCl that has a pH of 4.65? × 10n M n = What is the hydroxide ion concentration in a solution of NH3 with a pOH of 4.65? × 10n M n =

Answer 1

Explanation:

Hydronium ions concentration of the solution with pH value of 4.65.

$pH=-\log[H_3O^+]$

$4.65=-\log[H_3O^+]$

$Antilog {-4.65}=[H_3O]$

$[H_3O^+]=2.2387\times 10^{-5} M$

Hydroxide ions concentration of the solution with pOH value of 4.65.

$pOH=-\log[OH^-]$

$4.65=-\log[OH^-]$

$Antilog {-4.65}=[OH^-]$

$[OH^-]=2.2387\times 10^{-5} M$

Answer 2

The hydrogen ions concentration of the solution of HCl that has a pH of 4.65 is 2.23 × 10-5, and the hydroxide ion concentration of a solution of NH3 with a pOH of 4.65 is 2.23 × 10-5 M

pH

pH of a solution is defined as the negative logarithm to the base 10 of the hydrogen ion concentration of the solution.

• pH = -log[H+]
• [H+] = antilog-pH

pH of solution = 4.65

[H+] = antilog -4.65

[H+] = 2.23 × 10-5 M

pOH

pOH of a solution is defined as the negative logarithm to the base 10 of the hydroxide ion concentration of the solution.

• pOH = -log[OH-]
• [OH-] = antilog-pH

pOH of solution = 4.65

[OH-] = antilog -4.65

[OH-] = 2.23 × 10-5 M

Therefore, the hydrogen ions concentration of the solution of HCl that has a pH of 4.65 is 2.23 × 10-5, and the hydroxide ion concentration of a solution of NH3 with a pOH of 4.65 is 2.23 × 10-5 M

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