pH scale and hydrogen ion concentration

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.…

A solution has a pH of 4.0 at 298 K. What is the hydroxide ion concentration, [$\ce{OH-}$], in $\mathrm{mol\,dm^{-3}}$? A. 10 B. $10^{-4}$ C. $10^{-10}$ D. $10^{-18}$

Which of these aqueous solutions has the highest pH? A. $0.10\ \mathrm{mol\,dm^{-3}}$ $\ce{HCl}$ B. $1.0\ \mathrm{mol\,dm^{-3}}$ $\ce{NH3}$ C. $0.10\ \mathrm{mol\,dm^{-3}}$ $\ce{KOH}$ D. $1.0\ \mathrm{mol\,dm^{-3}}$ $\ce{KOH}$

A small volume of $0.050\ \mathrm{mol\,dm^{-3}}$ hydrobromic acid is placed in a beaker fitted with a pH probe. Distilled water is then run into the beaker at a constant rate and the pH is logged continuously; the temperature is held at 298 K. (i) Sketch, on…