Strong and weak acids and bases

Nitric acid, $\ce{HNO3}$, is strong, while nitrous acid, $\ce{HNO2}$, is weak. (i) Outline the difference between a strong and a weak acid. (ii) Deduce the Lewis formula and the molecular geometry for the nitrite ion, $\ce{NO2-}$.

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…

Which solution has a pH of 11.0 at 298 K? A. $10^{-3}\ \mathrm{mol\,dm^{-3}}$ $\ce{KOH(aq)}$ B. $10^{-11}\ \mathrm{mol\,dm^{-3}}$ $\ce{KOH(aq)}$ C. $10^{-3}\ \mathrm{mol\,dm^{-3}}$ $\ce{NH3(aq)}$ D. $10^{-3}\ \mathrm{mol\,dm^{-3}}$ $\ce{HCl(aq)}$

What is the main reason why nitric acid has a lower pH than ethanoic acid of the same concentration? A. Nitric acid is an oxidizing agent. B. Nitric acid ionizes to a greater extent in water. C. The conjugate base of nitric acid is stronger than that of…

Methanoic acid, $\ce{HCOOH(aq)}$, and hydrochloric acid, $\ce{HCl(aq)}$, are both acids. A $0.100\ \mathrm{mol\,dm^{-3}}$ solution of $\ce{HCOOH(aq)}$ has a pH of 2.39 while a solution of $\ce{HCl(aq)}$ of the same concentration has a pH of 1.00. (i) Explain…

In water, HOBr partly ionizes to give the hypobromite ion, $\ce{OBr-}$; the ion is a much weaker sanitizer than the un-ionized acid. The graph shows how the percentages of the dissolved bromine present as HOBr(aq) and as $\ce{OBr-}$(aq) vary with pH at 25 °C.…