Acid Base Review Station Activity

List the strong acids and strong bases What happens if the following substances are in solution (equilibrium, reaction, buffer)? – weak base – weak acid and a strong base – Acid and base – Weak acid and its conjugate base – Weak acid – Strong acid and strong base

1.Fifty mL of 5 M nitric acid needs to be diluted to 1 M. Water is added until this concentration is met. What is the final volume? What is the initial and final pH of the nitric acid? 2. If 50.0 grams of solid salicylic acid (HC 7 H 5 O 3, Ka=1.07x10 -3 ) are dissolved in 500mL of water, what is the pH?

Does substance A depict a strong or a weak acid? Explain. Compare the strengths of A and B. Justify your choice. Which would have a larger Ka? How do you know? A B

Strengths of weak acids and weak bases Answer the following questions: 1.Which of the two acids is stronger, HOCl or HOBr? Justify in terms of Ka. 2.Hypoiodous acid has the formula HOI. Predict whether HOI is a stronger acid or a weaker acid than the acid that you identified in part 1. Justify your prediction in terms of chemical bonding. 3.Which of the two conjugate bases, OCl -1 or OBr -1, is stronger? Justify your answer. AcidKa at 298 K HOCl2.9 x HOBr2.4 x 10 -9

Write balanced, net-ionic equations for the neutralization reactions below. Assume that all species are in aqueous solution. 1.Potassium hydroxide and hydroiodic acid 2.Ascorbic acid (H 2 C 6 H 6 O 6 ) and barium hydroxide (assume ascorbic acid is monoprotic  it releases only one hydrogen ion) 3.Hydrocyanic acid (HCN) and silicate (SiO 3 -2 ) 4.Ammonia and sulfuric acid (while this acid is diprotic, the first proton is released much easier than the second, so write the reaction when just one proton reacts) A.Underneath each substance write an ‘A’ or a ‘B’ to indicate whether it is an acid or a base. Do this under the reactants and the products. B.Define monoprotic and diprotic. Give an example of a triprotic acid. (Diprotic and triprotic acids are called polyprotic acids)

1.When 20 mL of 0.55 M acetic acid (Ka=1.8E-5) reacts with 45 mL of calcium hydroxide, the indicator changes colors indicating that the ___________ __________ has been reached. 2.What is the concentration of calcium hydroxide? 3.What is the pH of the solution at the __ __?

A) Write the equilibrium expression for the reaction of methylamine (CH 3 NH 2 ) with water. B) Determine the Kb of a M solution of methylamine with a pH of C) Is methylamine an acid or a base? Is it weak or strong? How do you know?

Phosphoric acid forms 3 separate equilibrium reactions; in each reaction just 1 proton (H + ) pops off – Write the three equilibrium reactions K a1 is the equilibrium constant for the first proton removal, K a2 is for the second, etc. – How do these values compare to each other? The following ions are in order. Do they go in order of increasing or decreasing concentration in a solution of phosphoric acid? Justify your answer. – H 3 PO 4, H 2 PO 4 1-, HPO 4 2-, PO 4 3- FormulaK a1 K a2 K a3 H 3 PO x x x10 -13