Review | constants | periodic table percent ionization can be used to quantify the extent of ionization of an acid in solution and is defined by the following formula for the acid ha: percent ionization=[ha] ionized[ha] initial×100% percent ionization increases with increasing ka. strong acids, for which ka is very large, ionize completely (100%). for weak acids, the percent ionization changes with concentration. the more diluted the acid is, the greater percent ionization. a convenient way to keep track of changing concentrations is through what is often called an i. c.e table, where i stands for "initial concentration," c stands for "change," and e stands for "equilibrium concentration." to create such a table, write the concentrations of reactant(s) and product(s) across the top, creating the columns, and write the rows i. c.e on the left-hand side. such a table is shown below for the reaction: a+b⇌ab initial (m)change (m)equilibrium (m)[a] [b][ab]
a certain weak acid, ha, has a ka value of 1.0×10−7.
part a.) calculate the percent ionization of ha in a 0.10 m solution.
part b.) calculate the percent ionization of ha in a 0.010 m solution.

Many reactions take place in aqueous solution. when potential reactants are mixed, a reaction will occur if there is some driving force that favors the formation of products. it is often convenient to categorize reactions in terms of these driving forces: precipitate formation, in which an insoluble solid is formed, weak electrolyte formation, as in a neutralization reaction involving water, or transfer of electrons, as in a redox reaction. these reactions can be represented by full molecular equations, which contain all species in the reaction mixture, or by net ionic equations, which show only the species that actually undergo a change. the latter does not contain the spectator ions, which do not undergo a net change or do not take part in the reaction. part a when the following two solutions are mixed: k2co3(aq)+fe(no3)3(aq) the mixture contains the ions listed below. sort these species into spectator ions and ions that react. drag the appropriate items to their respective bins. view available hint(s) spectator ions ions that react part b what is the correct net ionic equation, including all coefficients, charges, and phases, for the following set of reactants? assume that the contribution of protons from h2so4 is near 100 %.ba(oh)2(aq)+h2so4(aq)→ express your answer as a chemical equation. view available hint(s) nothing provide feedback