Use Lewis structures to show how electron pairs move and bonds form and break in this reaction, and identify the Lewis acid. SO, (g) so, (g) +H,O(1) H,SO,(aq)

Open bodies of water can act as carbon sinks due to the ability of carbon dioxide to dissolve in water.  The dissolution of carbon dioxide produces carbonic acid (H2CO3) which then partially dissociates in an equilibrium reaction important for controlling water pH. CO2 (g) + H2O (l) H2CO3 (aq) H2CO3 (aq) ↔ H+ (aq) + HCO3- (aq) The equilibrium between carbonic acid (H2CO3) and bicarbonate (HCO3-) is influenced by the presence of dissolved metals from the bedrock underlying a body of water.  Calcium from limestone (a type of sedimentary rock formed from marine exoskeletons) is one such metal.  The graph below shows how the concentration of dissolved calcium ions (measured in parts per million, or mg/L) affects the concentration of carbon dioxide dissolved in ocean water (measured partial pressure).  Based on this graph and your understanding of equilibrium, in what direction does the presence of limestone shift the carbonic acid/bicarbonate equilibrium?

Calculate the pH of the resulting solution if 29.0 mL of 0.290 M HCI(aq) is added to 39.0 mL of 0.290 M NAOH(aq). pH = Calculate the pH of the resulting solution if 29.0 mL of 0.290 M HCI(aq) is added to 19.0 mL of 0.390 M NAOH(aq). pH =

Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4and 5.4 × 10^–10, respectively, calculate the pH of the following solutions: (a)The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3).  (b)The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.

For each of the following entities • Identify it as a strong or weak acid. • Select the correct arrow to show the changes that occur when the acids are placed in water. • Select the approximate pH for each resulting solution. HCI(aq) is classified as a + acid. The reaction equation with water utilizes which of the following arrows? Choice A Choice B 7 >>7 H2SO3(aq) is classified as a The reaction equation with water would utilize which of the following arrows? Choice A Choice B < 50% H2SO3(aq) + H20(I) • HSO3 (aq) + H30*(aq) The approximate pH of the solution would be

The pOH of an aqueous solution of 0.591 M phenol (a weak acid), C,H5OH, is

(a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.

The ionization constant, K, for weak base, B, is 3.49 x 10-8. What is the pH of a 0.6975 M solution of this base? The equation for the ionization of weak base B as follows. B (aq) + H20(1) = BH*(aq) + OH"(aq) Report your answer with two places past the decimal. THint: Use an ICE table.)

Sodium lactate is the sodium salt of lactic acid.a) Use Acid-Base Properties of Salt Solutions, to explain if sodium lactate, NaC3H5O3(aq), is acidic or basic?b) Use ICE table to determine what is the pH of a solution that contains 0.75mol/L lactic acid, HC3H5O3(aq) (Ka = 1.4 x 10-4), and 0.25mol/L sodium lactate, NaC3H5O3(aq) ?

A 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.