Calculate the pH and pOH of the following solutions. (a) 0.51 M CsOH (b) 0.0040 M HI (c) 0.13 M

step 1 In answering this question, we have to recall that pH is equal to negative log, the concentratio

Calculate the pH and pOH of the following solutions. (a)...

Calculate the $\mathrm{pH}$ and $\mathrm{pOH}$ of the following solutions.
(a) $0.51 \mathrm{M} \mathrm{CsOH}$
(b) $0.0040 \mathrm{M} \mathrm{HI}$
(c) $0.13 M \mathrm{LiOH}$
(d) $0.66 \mathrm{MHClO}_{4}$

Key Concepts

pH and pOH calculation

pH and pOH are logarithmic measures of the hydrogen ion [H+] and hydroxide ion [OH-] concentrations in a solution, respectively. The definitions pH = -log[H+] and pOH = -log[OH-] provide a convenient way to express the acid-base balance in aqueous solutions, and under standard conditions, they are related by the equation pH + pOH = 14.

Strong acids and bases

Strong acids and bases are compounds that completely dissociate in water, meaning that the concentration of hydrogen ions or hydroxide ions produced is equal to the concentration of the acid or base added. This complete dissociation simplifies the calculation processes for pH and pOH, as the ion concentration can be directly inferred from the known molarity of the acid or base.

Water Ionization Constant (Kw)

The water ionization constant, Kw, reflects the self-ionization equilibrium of water, given by [H+][OH-] = 1.0 × 10^-14 at 25°C. This constant is crucial in relating the pH and pOH of a solution, as it allows for the calculation of one value when the other is known.

Logarithmic calculations

The use of base-10 logarithms is fundamental in converting ion concentrations to pH and pOH values. Understanding and applying logarithmic transformations is essential for handling the wide range of ion concentrations encountered in acid-base chemistry and for making the scale of these concentrations more manageable.

Transcript

Please give Ace some feedback