Question

What is the [H3O+] of a solution with a pH of 2.56? 2.56 M, 2.75 x 10-3 M, 363 M, or -0.408 M

Answer 1

PH=2.56

pH=-lg[H₃O⁺]

[H₃O⁺]=10^(-pH)

[H₃O⁺]=10⁻²·⁵⁶=0.00275=2.75×10⁻³ mol/L

2.75×10⁻³ M

Answer 2

Answer:

The concentration of hydronium ions in solution is $2.75\times 10^{-3} M$.

Explanation:

The pH of the solution is defined as negative logarithm of hydronium ions concentration in a solution. Mathematically written as:

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

Given, the pH of the solution = 2.56

$2.56=-\log[H_3O^+]$

$[H_3O^+]=0.002754 M=2.75\times 10^{-3} M$

The concentration of hydronium ions in solution is $2.75\times 10^{-3} M$.