a) You have 11 moles of glucose (C6H12O6).    How many moles of glucose do you have?       If this were dissolved into 0.5 liters of water, what would the Molarity of that solution be?       b) You have 210 g of CHF3. How many moles of CHF3 do you have? If this were dissolved to a molarity of 8 M, what would the volume of the solution be?

How much glucose, C6H12O6, in grams, must be dissolved in water to produce 61.5 mL of 0.395 M C6H12O6?

What is the molarity of ZnCl2 that forms when 25.0 g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 285 mL . Zn(s)+CuCl2(aq)→ZnCl2(aq)+Cu(s) Part B: Hard water often contains dissolved Ca2+ and Mg2+ ions. One way to soften water is to add phosphates. The phosphate ion forms insoluble precipitates with calcium and magnesium ions, removing them from solution. A solution is 0.055 M in calcium chloride and 0.095 M in magnesium nitrate. What mass of sodium phosphate would you add to 1.0 L of this solution to completely eliminate the hard water ions? Assume complete reaction. Express your answer using two significant figures   Part C: Enter an equation for the precipitation reaction that occurs (if any) when solutions of ammonium chloride and silver nitrate are mixed. Express your answer as a chemical equation. Identify all of the phases in your answer. Enter noreaction if no precipitate is formed.

What is the mass in grams of solute in a. 32.0 ml of 0.150 M C6H12O11 b. 3.92 L of 6.23 x 10 -3 M H2O2

A saline solution contains 0.770 g of NaCl (molar mass = 58.55 g/mol) in 118 mL of solution. The concentration is 0.112 M. What is the concentration of Na and Cl ions in this solution given in molarity and rounded to 3 significant figures?

You have a solution of KCl that has a concentration of 0.0457M. What is the concentration in g/cm3. The molar mass of KCI is 74.5513 g/mol.

What is the molarity of a 3.00 m solution of KCl dissolved in water, given that the solution has a density of 1.13 g/mL?

What is the molarity of a solution in which 23.1 g of sodium sulfate (Na2SO4) is dissolved in enough water to make 250. mL of solution? 0.0922 M 0.652 M 0.163 M 0.205 M

Calcium nitrate  (Ca(NO3)2 ; MM =164.0878 g/mol)) dissolves in cold water to the extent of 266 g per 100. mL.  What is the concentration (mol/L) of nitrate ions in this solution? Ca(NO3)2 -> Ca+2 + 2 NO3-

Imagine you are preparing a solution of NaCl and a solution of CaCl2.  After you prepare them you go out to lunch with your colleagues.  When you come back you cannot remember which solution is in which container because you forgot to label the containers before going to lunch.  What experiments can you perform to identify each solution?