An aqueous solution of nickel(II) bromide, NiBr2, is made by dissolving 11.2 grams of nickel(II) bromide in sufficient water In a 250. ml volumetric flask, and then adding enough water to fill the flask to the mark. What is the weight/volume percentage of nickel(II) bromide in the solution? Weight/volume percentage

A student dissolved 6.00 g of Co(NO 3) 2 in enough water to make 100. mL of stock solution. He took 4.00 mL of the stock solution and then diluted it with water to give 275. mL of a final solution. How many grams of NO 3 - ion are in the  final solution?

Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H 2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 14.8 gg . What mass of H2 gas would be produced by the complete reaction of the aluminum block?

Apply the concepts of stoichiometry and solution concentration in this section.  Potassium iodide reacts with lead (II) nitrate in the following precipitation reaction 2 KI (aq)  + Pb(NO3)2 (aq)       KNO3 (aq)    +  PbI2 (s). What volume of 0.200 M KI solution is required to completely precipitate all of the lead in 255mL of a 0.312 M Pb(NO3)2 solution?           An solution is made by dissolving 28.4 g of glucose (C6H12O6) in 355 g of water. The final volume of the solution is 378 mL. Calculate the molarity, molality, mole fraction, mole percent and mass percent of the solution,                          Hydrochloric acid is usually purchased in a concentrated form that is 37.0 % HCl by mass and has a density of 1.20 g/mL. Describe exactly how to prepare 2.85 L of a 0.500 M HCl to be used in Dr. Henary’s CHEM1211K lab from the concentrated solution. Hint (Find molarity of concentrated solution and use dilution equation. This is how your solution are prepared)