17. Acid and Base Equilibrium

The pH of a $0.0040$ M solution of $C_a{\left(OH\right)}^2$ (assume complete dissociation at 25 °C) is closest to:

A solution containing aqueous HCl would most likely have which property at 25 °C?

Which statement best describes the behavior of a strong acid such as $HCl$ in water when calculating pH?

What is the pH of a $0.001 M$ $NaOH$ solution at $25°C$ (assume complete dissociation)?

What is the pH of a $0.050 M$ $\mathrm{Li}OH$ solution at $25°C$? Assume $\mathrm{Li}OH$ is a strong base that dissociates completely.

What is the pH of a $0.00125$ M $HCl$ solution at $25°C$? (Assume $HCl$ is a strong acid and fully dissociates.)

What is the pH of a $0.0040 M$ solution of $HN{O}_3$, assuming it is a strong acid that dissociates completely in water?

At 25 °C, what is the pH of a $1.00\times 100^{\mathrm{}}$ M aqueous solution of sodium hydroxide, $NaOH$, assuming it dissociates completely?

What is the pH of a $0.0235$ M $HCl$ solution at $25°C$, assuming complete dissociation?

What is the pH of a $0.000100$ M solution of hydrobromic acid, HBr, assuming it behaves as a strong acid and water autoionization is negligible?

What is the pH of a 2.8 M solution of HClO_4, assuming complete dissociation?

Pyridinium bromide (C5H5NHBr) is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. A solution of pyridinium bromide has a pH of 2.92. Kb for pyridine is 1.7×10^-9. What is the molarity of the solution?

What is the pH of an aqueous $8.5\times {10}^{-3}$ M HI solution at 25 °C? (Assume HI is a strong acid.)