Determine the pH of the following solutions. Explain. [HCl]=0.001M and [NaOH]=1x10-2 M. Thank you!?

HCl is a strong acid which completely ionizes in water to give hydrogen ions.
[H⁺] = [HCl]ₒ = 0.001 M
OR: [H₃O⁺] = [HCl]ₒ = 0.001 M

pH = -log[H⁺] = -log(0.001) = 3
OR: pH = -log[H₃O⁺] = -log(0.001) = 3


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NaOH completely dissociates in water to give hydroxide ions.
[OH⁻] = [NaOH]ₒ = 1 × 10⁻² M

pOH = -log[OH⁻] = -log(1 × 10⁻²) = 2
pH = pKw - pOH = 14 - 2 = 12

[HCl] means moles of hydrochloric acid per liter of the solution. To determine the pH of an acid solution, use the following equation.

pH = -1 * log [H3O+1]

Since hydrochloric acid is a strong acid, the concentration of the hydronium ion is equal to the hydrochloric acid.

pH = -1 * log 0.001
This is 3

[NaOH]=1x10-2 M.

Since sodium hydroxide is a strong base, the concentration of the hydroxide ions is equal to to the concentration of the base. In this problem, the concentration of these ions is 1 * 10^-2. There are two ways to determinate pH of this solution.

#1 Determine the pOH. Then use the following equation to determine the pH.

pOH + pH = 14
pOH = -1 * log 1 * 10^-2
This is 2.

2 + pH = 14
pH = 12

OR

[H3O+1] * [OH-1] =1 * 10^-14
[H3O+1] * (1 * 10^-2) = 1 * 10^-14
[H3O+1] = 1 * 10^-12
pH = -1 * log (1 * 10^-12) = 12

I hope these explanations and equations are helpful for you.

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