calculate the molar hydroxide ion concentration of each of the following solutions given the pH 4.53. Answer should be for OH-.
Please show me how to do this in step by step
I tried putting in 10 xy-4.53= 0.000029512 which is 3.0 * 10^-5
It says that the answer is wrong.
To calculate the molar hydroxide ion (OH-) concentration from a given pH, you can use the following steps:
Step 1: Convert the given pH to the hydrogen ion concentration (H+).
Given pH = 4.53
H+ concentration = 10^(-pH)
= 10^(-4.53)
= 3.24 * 10^(-5) M
Step 2: Determine the concentration of hydroxide ion (OH-) using the concept of water dissociation.
In pure water at 25°C, the concentration of H+ and OH- ions are equal, each being 1.00 * 10^(-7) M.
Since the solution you have is not neutral, you have to consider the dissociation of water as well.
Step 3: Use the concept of Kw (ionization constant for water) to find [OH-].
Kw = [H+][OH-]
[H+] = 3.24 * 10^(-5) M (from Step 1)
[OH-] = Kw / [H+]
Kw at 25°C is generally considered as 1.00 * 10^(-14) M^2. You can use this value for calculation.
[OH-] = (1.00 * 10^(-14) M^2) / (3.24 * 10^(-5) M)
Step 4: Calculate the value of [OH-] and express it in proper scientific notation:
[OH-] ≈ 3.09 * 10^(-10) M
Therefore, the molar hydroxide ion concentration (OH-) in the given solution with a pH of 4.53 is approximately 3.09 * 10^(-10) M.