Question

HELP!!!

Answer 1

Answer: The concentration of hydronium ions in a solution is $2.5\times 10^{-5}$ and the concentration of hydroxide ion concentration is $4\times 10^{-10}$

Explanation:

• pH is defined as negative logarithm of hydrogen ion concentration. It is basically defined as the power of hydrogen ions in a solution.

Mathematically,

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

pH of the solution = 4.6

Putting values in above equation, we get:

$4.6=-\log[H^+]$

$[H^+]=antilog(-4.6)$

$[H^+]=2.5\times 10^{-5}$

We are given:

pH of the solution = 4.6

• To calculate the hydroxide ion concentration of the solution, we need to determine the pOH of the solution first. And to calculate that we use the equation:

$pH+pOH=14\\pOH=14-4.6=9.4$

• pOH is defined as negative logarithm of hydroxide ion concentration. It is basically defined as the power of hydroxide ions in a solution.

Mathematically,

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

pOH of the solution = 9.4

Putting values in above equation, we get:

$9.4=-\log[OH^-]$

$[OH^-]=antilog(-9.4)$

$[OH^-]=4\times 10^{-10}$

Hence, the concentration of hydronium ions in a solution is $2.5\times 10^{-5}$ and the concentration of hydroxide ion concentration is $4\times 10^{-10}$

Answer 2

Answer:

2.5 × 10⁻⁵ M H₃O⁺ and 4.0 × 10⁻¹⁰ M OH⁻.

Explanation:

∵ pH = - log[H₃O⁺]

∴ 4.6 = - log[H₃O⁺].

∴ log[H₃O⁺] = - 4.6.

∴ [H₃O⁺] = 2.51 x 10⁻⁵.

∵ [H₃O⁺][OH⁻] = 10⁻¹⁴.

[H₃O⁺] = 2.51  x 10⁻⁵ M.

∴ [OH⁻] = 10⁻¹⁴/[H₃O⁺] = 10⁻¹⁴/(2.51  x 10⁻⁵ M) = 3.98 × 10⁻¹⁰ M ≅ 4.0 × 10⁻¹⁰ M.

So, the right choice is: 2.5 × 10⁻⁵ M H₃O⁺ and 4.0 × 10⁻¹⁰ M OH⁻.