(Solved): 3.1 Use the Bronsted-Lowry acid-base theory to write a balanced equation for the ionization of ach ...

3.1 Use the Bronsted-Lowry acid-base theory to write a balanced equation for the ionization of ach of the following species in water: a) \( \mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{ac}) \) b) \( \mathrm{NH}(\mathrm{g}) \) 3.2 Define an amphoteric species. Use appriopriate chemical equation(s) to illustrate your answer. (3) 3.3 a) What is the hydronium ion concentration of a \( 0.0013 \mathrm{M} \) solution of \( \mathrm{HNO}_{3} \) ? b) Calculate the \( \mathrm{pH} \) of the solution. 3.4 A \( 0.015 \mathrm{M} \) solution of hydrogen cyanate, HOCN, has a pH o; \( 2.67 \). Calculate the hydronium ion concentration in the solution. 3.5 \( \mathrm{A} 0.600 \mathrm{M} \mathrm{CH} 3 \mathrm{COOH} \) solution nas a \( \mathrm{pH} \) of \( 2.5 \mathrm{Calculate} \) the ionization constant, \( \mathrm{Ka}_{\text {, }} \) for the acid. 3.6 A \( 40.0 \mathrm{~mL} \) solution of a \( 0.250 \mathrm{M} \mathrm{HCl} \) is titrated with a \( 0.200 \mathrm{M} \) NaOH solution. What volume of the \( \mathrm{NaOH} \) solution is required to reach the equivalence point?