Question

1)Determine the molarity (in mol/L) of NH₄⁺ ions in solution when 3.60×10^-2 g of ammonium oxalate is added to enough water to prepare 5.23×10² mL of the solution

2)Calculate the molarity (in mol/L) of the IO₃^− ion in a solution resulting from the dilution of 73.9 mL of 3.88×10^-1 M Ca(IO₃)₂ to a final volume of 687 mL. Report your answer to three significant figures.

3)Calculate the pH (to two decimal places) for the following: 5.67×10^-1 M NaH

4)Determine the pOH (to two decimal places) of the solution that is produced by mixing 4.4 mL of 8.02×10^-1 M K₂O with 7.88 mL of 4.40×10^-3 M Mg(OH)₂.

5)A sample of tris(hyroxymethyl)aminomethane (H₂NC(CH₂OH)₃), which is a base, with a mass of 0.5175 g is dissolved in water and used to standardize a solution of nitric acid. An endpoint is reached when 40.74 mL of nitric acid has been added. Determine the molarity (in mol/L) of the nitric acid solution. Report your answer to four significant figures.

6)The standardized nitric acid solution is then used to titrate 48.25 mL of a solution of sodium lactate (NaC₂H₅OCOO). An endpoint is reached when 15.22 mL of nitric acid has been added. Determine the molarity (in mol/L) of the sodium lactate solution. Report your answer to four significant figures.