Question 1 and 2
Write the formula and name of the conjugate of each of the following: HCN, NO_2^-, HCO_3^-, CIO_3^-, HI, NH_3, CH_3COOH. KHC_2O_4 is an amphoteric compound. Write a balanced equation for this compound functioning as an acid while in aqueous solution. Do the same for this compound functioning as a base while in aqueous solution. Identify the strongest acid species and the strongest base species that can exist in aqueous solution by their names and formulas. Explain why the deionized water in the laboratory typically has a pH below 7. Calculate the pH of each of the following solutions. a. 0.500 M HCl b. 9.5 times 10^-2 M AI(OH)_3 c. 0.088 M CH_3CH_2COOH, Ka = 1.3 times 10^-5 d. 0.120 M C_5H_5N, Kb = 1.7 times 10^-9 Calculate the Ka for chloroacetic acid if a 0.100 M solution has a pH of 1.95. Calculate the molarity of an aqueous solution of HCN (Ka = 4.9 times 10^-10) whose pH is 5.00.