1. Calculate the pH of the following solutions of HNO3. You must show all work in detail to receive credit: (a) 0.24 M, (b) 0.00087 M, (c) 0.25 M, (d) 0.000001 M.
2. **(PART 1) Calculate the boiling points of these solutions:
0.1 m Na2P
0.2 m NaBr
0.16 m C12H22O11
POTENTIALLY USEFUL INFORMATION: Kb for water = 0.512 C*kg solvent/mol solute
—You must show all work in detail to receive credit.—
(PART 2) Place the above solutions in order of boiling point from lowest to highest.
You must show all work in detail to receive credit.
3. *Calculate the molarity (M) for each of these solutions–you must show all work in detail to receive credit: (a) 121.45 g of KOH in 100.0 mL, (b) 23.49 g of NH4OH in 150.0 mL, (c) 217.5 g of LiNO3 in 1.50 L, (d) 15.25 g of Pb(C2H3O2)2 in 50.0 mL
4. **Suppose you have 0.0100 L of hydrochloric acid, but it’s concentration is unknown. If you titrated it with a 0.250 M potassium hydroxide solution, and it took 9.80 mL of the base to neutralize the acid. what was the concentration of the nitric acid? Write the neutralization reaction, balance it, name the products THEN Solve the problem above. You must show all work to receive credit.