2. A water sample has 10 µg/L Hg2+ and a density of 1.0 g/mL (atomic weight of Hg = 200.59). Calculate the following: (a) Hg²+ in ppb, (b) Hg²+ in µM, and (c) the number of Hg²+ ion in 1L of this sample containing 10 µg/L Hg2+ (Avogadro's number = 6.022 × 1023 /mol).

A student has a solution that contains 48.1 mg of PNP (MW = 139 g mol-1) in 650 mL of 45.0 % ethanol.  Calculate the concentration of PNP in the solution (in µM).

2. Using the data given below, calculate the percentage of KHP in the impure sample. The molar mass of KHP is 204.219 g/mol. Molarity of NaOH Solution: Mass of Unknown: Volume of Water Used to Dissolve Unknown: Volume of NaOH Used to Reach Equivalence Point: Percent of KHP: 0.1955 M 1.1801 g 30.00 mL 17.01 mL % Stolal Vol)

Solution X 100 mL of 0.10 M NaOH(aq) is mixed with 100 mL of 0.10 M HBr(aq) Solution Y 100 mL of 0.10 M NaBr(aq) is mixed with 100 mL of 0.10 M HBr(aq) Solution Z 100 mL of 0.10 M HC,H,O,(aq) is mixed with 100 mL of 0.10 M NaC,H3O,(aq) 6. A student prepares three solutions, X, Y, and Z, as described in the table above. The values of Ka for the acidic species in the solutions are given in the table below. Species Ka HBr(aq) >>I (very large) HC,H;O,(aq) 1.8 x 10-5 a. Using the information above, write the letters of the solutions in the boxes below to rank the solutions in order of increasing pH. Explain your reasoning for the ranking Lowest pH Highest pH b. Does the pH of solution Y increase, decrease, or remain the same when 100 mL of water is added? Justify your answer. c. The student adds 0.0010 mol of NaOH(s) to solution Y, and adds 0.0010 mol of NaOH(s) to solution Z. Assume that the volume of each solution does not change when the NaOH(s) is added. The pH of solution Y changes…