pH scale and hydrogen ion concentration

Calculate the pH of a 0.125 mol dm$^{-3}$ solution of sodium hydroxide.

In aqueous solution hydrogen cyanide behaves as a weak acid. (i) Write an equation for the ionization of hydrogen cyanide in water. (ii) Outline two ways in which a solution of 0.050 $\mathrm{mol\,dm^{-3}}$ $\ce{HCN}$ could be distinguished experimentally from…

What is the pH of a 0.020 $\mathrm{mol\,dm^{-3}}$ solution of nitric acid, $\ce{HNO3(aq)}$? A. 1.0 B. 1.7 C. 2.0 D. 12.3

Which of these solutions has a pH greater than 7 at 25 °C? A. $[\ce{H+}] = 1.0 \times 10^{-5}\ \mathrm{mol\,dm^{-3}}$ B. $[\ce{OH-}] = 1.0 \times 10^{-10}\ \mathrm{mol\,dm^{-3}}$ C. $[\ce{H3O+}] = 1.0 \times 10^{-11}\ \mathrm{mol\,dm^{-3}}$ D.…

The pH of a solution is measured as 4.0. Which value, in $\mathrm{mol\,dm^{-3}}$, is the hydrogen-ion concentration, $[\ce{H+}]$, of this solution? A. $4.0 \times 10^{-4}$ B. $1.0 \times 10^{-4}$ C. $1.0 \times 10^{4}$ D. $4.0 \times 10^{4}$

Nitric acid is a strong acid manufactured on a large scale. A pH probe is immersed in a small volume of $0.010\ \mathrm{mol\,dm^{-3}}$ nitric acid. The pH is recorded while distilled water is added to the acid at a steady rate and at constant temperature. (i)…