0.12 M acetic acid + 0.15 M sodium acetate 0.25 M hydroiodic acid + 0.24 M potassium iodide 0.30 M ammonium bromide + 0.31 M ammonia 0.15 M calcium hydroxide + 0.22 M calcium bromide 0.33 M hydrofluoric acid + 0.24 M potassium fluoride

Sulfuric acid is listed in a catalog with a concentration of 95-98%. A bottle of the acid in the stockroom states that 1.00 L has a mass of 1.84 kg. To determine the concentration of sulfuric acid in the stockroom bottle, a student dilutes 5.00 mL to 500. mL She then takes four 10.00-mL samples and titrates each with standardized sodium hydroxide (c = 0.1760 M). (a) What is the average concentration of the diluted sulfuric acid sample? (b) What is the mass percent of H2SO4 in the original bottle of the acid?

A 2.20-g sample of an unknown acid (empirical formula = C3H4O3) is dissolved in 1.0 L of water. A titration required 25.0 mL of 0.500 M NaOH to react completely with all the acid present. Assuming the unknown acid has one acidic proton per molecule, what is the molecular formula of the unknown acid?

It took 25.06 0.05 mL of a sodium hydroxide solution to titrate a 0.4016-g sample of KHP (see Exercise 79). Calculate the concentration and uncertainty in the concentration of the sodium hydroxide solution. (See Appendix 1.5.) Neglect any uncertainty in the mass.

Suppose 50.0 mL of 0.250 M CoCl2 solution is added to 25.0 mL of 0.350 M NiCl2 solution. Calculate the concentration, in moles per liter, of each of the ions present after mixing. Assume that the volumes are additive.

Two students titrate different samples of the same solution of HCl using 0.100 M NaOH solution and phenolphthalein indicator (Figure 4.12). The first student pipets 20.0 mL of the HCl solution into a flask, adds 20 mL of distilled water and a few drops of phenolphthalein solution, and titrates until a lasting pink color appears. The second student pipets 20.0 mL of the HCl solution into a flask, adds 60 mL of distilled water and a few drops of phenolphthalein solution, and titrates to the first lasting pink color. Each student correctly calculates the molarity of an HCl solution. What will the second students result be? (a) four times less than the first students result (b) four times greater than the first students result (c) two times less than the first students result (d) two times greater than the first students result (e) the same as the first students result