Section: Name: Laboratory Questions: Solution Stoichiometry A solution is prepared by dissolving 3.7500 grams iron(III) oxalate...
2. Describe how you would prepare 250.00 mL of 0.150 M ammonium ion solution beginning with solid ammonium phosphate, (NH),PO
Calculate the concentrations of hydroxide and hydronium ions in a solution prepared by dissolving 0.471 g of solid NaOH in enough water to make 225 mL of solution. Kw = 1.0E-14. Hydroxide ion concentration? M The number of significant digits is set to 3; the tolerance is +/-4% LINK TO TEXT Hydronium ion concentration? M The number of significant digits is set to 3; the tolerance is +/-4%
A solution is prepared by dissolving 200.0 g of iron (III) chloride (162.2 g/mol) in 200.0 mL of water. What is the molarity of the solution?
A solution of iron (II) sulfate was prepared by dissolving 10.00g of FeSO4-7H20 (FW= 277.9) in water and diluting up to a total volume of 250 ml. The solution was left to stand, exposed to air, and some of the iron (II) ions became oxidized to Iron (III) ions. a 25.0 ml sample of this partially oxidized solution required 23.70 ml of 0.0100M potassium dichromate K2Cr2O7 solution for complete reaction in the presence of dilute sulfuric acid. Calculate the percentage...
First name Last name Consider a solution prepared by dissolving 2.20 grams of Cach, in 500.ml of water, then answer the questions below 1. How many moles of Cach are being used? 2. What is the mass of water being used? 3. What is the molality of the CaCl solution? 4. What is the van t'Hoff factor for the Caci? 5. What is the change (A) in the boiling point of the solution from that of pure water? 6. What...
Solid ammonium sulfide is slowly added to 75.0 mL of a 0.0691 M iron(III) nitrate solution. The concentration of sulfide ion required to just initiate precipitation is M.
What is the molarity of a solution prepared by dissolving 5.90 grams of calcium nitrite [Ca(NO2)2, molar mass=132.10 g/mol] in enough water to make a 106.0 mL soln?
A solution of a theoretical triprotic acid was prepared by dissolving 5.981 g of solid in enough DI water to make 500.0 mL of solution. 13.87 mL of a 0.446 M solution was required to titrate 20.00 mL of this acid's solution. What is the concentration of the acid solution? What is the molar mass of the acid? Hint: You need to calculate the total moles in the 500.0 mL solution (the full 500.0 mL was NOT titrated).
Solution A is prepared by dissolving 89.4 g of Na3PO4 in enough water to make 1.50 L of solution. Solution B is 2.5 L of 0.696 M Na2SO4. a) What is the molar concentration of Na3PO4 in Solution A? 0.36 M b) How many millilitres of Solution A will give 2.50 g of Na3PO4? 41.95 mL c) A 50.0 mL sample of Solution B is mixed with a 75.00 mL sample of Solution A. Calculate the concentration of Na+ ions...
A student wishes to prepare 300-mL of a 0.236 M iron(III) acetate solution using solid iron(III) acetate, a 300-ml volumetric flask, and deionized water. (a) How many grams of iron(III) acetate must the student weigh out? (b) Which of the following would NOT be an expected step in the procedure used by the student? O Add additional water to the flask, mixing as each portion is added. O Add a small amount of water to the volumetric flask and swirl...