If the #pH=12# for a solution of potassium hydroxide, what is #[HO^-]#?

Answer 1

#[HO^-]# #=# #0.01*mol*L^-1#.

We know, or should know that (i) #pH=-log_10[H_3O^+]#, and #pOH=-log_10[HO^-]#; and (ii), given that #K_w=[H_3O^+][""^(-)OH]=10^-14# under standard conditions, #pK_w=pH+pOH=14.#

We have #pH=-log_10[H_3O^+]=12#; thus #[H_3O^+]=10^-12*mol*L^-1#, and #pOH=2#, and thus #[HO^-]=10^-2*mol*L^-1#.

What is #[K^+(aq)]#?

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Answer 2

Cooper Anderson

To find the concentration of hydroxide ions (([HO^-])) in a solution with a pH of 12, you can use the formula: ([HO^-] = 10^{-pH}). Substituting the given pH value into the formula: ([HO^-] = 10^{-12}). Calculating this gives ([HO^-] = 10^{-12}) M. Therefore, the concentration of hydroxide ions in the solution is (10^{-12}) M.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.