H+ (aq) + HCO2 (aq) -- H2CO (aq) + H2O(l) What is the equilibrium expression.

What two common assumptions can simplify calculation of equilibrium concentrations in a solution of a weak acid?

Write the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. HF (hydrofluoric acid) b. HC2H3O2 (acetic acid)

Why have chemists not tabulated the fraction ionized for different acids? Such a table would make problems such as calculating the pH of an acid solution quite simple.

Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each: (a) CS2+SHHCS3 (b) BF3+FBF4 (c) I+SnI2SnI3 (d) Al(OH)3+OHAl(OH)4 (e) F+SO3SFO3

Write the base ionization constant expression for the ionization of each of the following bases. In each case, the nitrogen atom accepts the proton. a. CH3NH2 (methylamine) b. C2H5NH2 (ethylamine)

You are asked to calculate the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide is a base, can we say there is no H+. since having H+ would imply that the solution is acidic?

In the following net ionic reaction, identify each species as either a Brnsted-Lowry acid or a Brnsted -Lowry base: CH3COO(aq)+HS(aq)CH3COOH(aq)+S2(aq). Identify the conjugate of each reactant and state whether it is a conjugate acid or a conjugate base.

Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?