In the larger box, draw the flipped chair, in the same orientation. In the smaller box, provide an estimated equilibrium constant.

The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that HCN is a weak acid. acids: 0,0,.. 0.7 mol of KOH is added to 1.0 L of a 0.7M HCN bases: ? solution. other: U 0.1 mol of HNO, is added to acids: 1.0 L of a solution that is bases: 0.4M in both HCN and NaCN. other: U

Incorrect Your answer is incorrect. The statements in the tables below are about two different chemical equilibria. The symbols have their usual meaning, for example AG" stands for the standard Gibbs free energy of reaction and X stands for the equilibrium constant. In each table, there may be one statement that is false because it contradicts the other three statements. If you find a false statement, check the box next to it. Otherwise, check the "no false statements" box under the table. statement AG >0 In K1 AS < AH" T no false statements: false? O O O 0 statement In K 0 AS- AH T AG 1 K=1 no false statements: false? O O O O 6 O E dla A

The undissociated base (B) is present in the greatest concentration, with the products being present in relatively smaller amounts in this equilibrium mixture. How would this affect the magnitude of Kb? Do you expect it to be small or large? Which is the strongest base? Name of base Ammonia (NH3) Methylamine (CH3NH2) Ethylamine (C2H5NH2) Diethylamine (C2H5)2NH Pyridine (CSH5N) Kb value 1.76 x 10-5 Why? 4.4 x 10-4 5.6 x 10-4 Which is the weakest base? 1.3 x 10-3 1.7 x 10-9 Why? The larger the Kb the (stronger/weaker) the base. Since a weak base dissociates incompletely setting up an equilibrium, what method could you think of that you could use to determine the concentration of [OH"] ions given the initial concentration of the acid and its Kb?