A 500 mL sample of waste water contains 26.1 µg of mercury, Hg. If the density of the sample is 1.073 g/mL. Calculate the concentration of mercury in parts per billion (ppb)

If 23.2 ml of NaOH solution is required to neutralize 0.123 g of KHP (molar mass = 204.2 g/mol), then the molarity of NaOH is: Select one: a. 0.026 b. 2.60 C. 0.922 d. 0.014

5.  You have 97.0 mL of a 0.500 M stock solution of HCl that must be diluted to 0.200 M.  How much water (in mL) should be added?   6.  Express the concentration of a 0.120 M solution of NaF in mass percentage (w/w) and in parts per million (PPM).  Assume the density of the solution is 1.00 g/mL.   7.  Assuming 100% dissociation, calculate the freezing point and boiling point (in °C) of a solution with 98.4 g of AgNO3 in 1.00 kg of water.   8.  Calculate the osmolarity of these solutions.  Assume density of the solution is 1.00 g/mL.               (a)  3.80 M MgCl2 solution                                         Osmolarity =               (b)  4.40% w/w glucose (C6H12O6) solution               Osmolarity =

a. Solid sodium hydroxide is slowly added to 125 mL of a 0.275 M iron(II) sulfate solution until the concentration of hydroxide ion is 0.0204 M. The mass of iron(II) ion remaining in solution is  ?grams. b.  Solid silver nitrate is slowly added to 150 mL of a 0.196 M sodium carbonate solution until the concentration of silver ion is 0.0673 M. The percent of carbonate ion remaining in solution is  ?%. c. Solid sodium carbonate is slowly added to 75.0 mL of a 0.435 M magnesium acetate solution until the concentration of carbonate ion is 0.0465 M. The percent of magnesium ion remaining in solution is  ?%.

"Concentrated" sulfuric acid solution is 95% sulfuric acid by mass (and the remainder water) and has a density of 1.64 gr/mL. ( Molar mass of H2SO4= 98 gr/mol) What is the molarity of concentrated sulfuric acid solution? O a. 16M Ob. 12 M 9M Od. 18 M