Calculate the molarity of the solution containing 28.33 g of C6H12O6 in 1.28 L.

To calculate the molarity (M) of a solution, you can use the formula:

M = moles of solute / liters of solution

First, we need to find the moles of solute, which in this case is glucose (C6H12O6). To do this, we use the molar mass of glucose, which we can calculate using the periodic table. The molar mass is as follows:

C: 12.01 g/mol (there are 6 Carbons, so 6 * 12.01 g/mol) H: 1.008 g/mol (there are 12 Hydrogens, so 12 * 1.008 g/mol) O: 16.00 g/mol (there are 6 Oxygens, so 6 * 16.00 g/mol)

Now, we calculate the molar mass of C6H12O6:

(6 * 12.01 g/mol) + (12 * 1.008 g/mol) + (6 * 16.00 g/mol) = 72.06 g/mol + 12.096 g/mol + 96.00 g/mol = 180.156 g/mol

Now we can convert the mass of glucose into moles:

28.33 g / 180.156 g/mol = 0.1573 moles

Now we have the volume of the solution as 1.28 liters. We can insert these values into the molarity formula:

M = 0.1573 moles / 1.28 L = 0.1229 M

So, the molarity of the glucose solution is 0.1229 M.

Extra: Molarity is a very common way to express the concentration of a solution in chemistry. It indicates the number of moles of solute (the substance being dissolved) per liter of solution. It's important because it allows chemists to know exactly how many particles of the substance are present in a given volume of solution, which is critical for reactions and processes in the lab.

The concept of molarity is fundamental to many aspects of chemistry, including stoichiometry in chemical reactions, because reactions often depend on the concentration of the reactants. By knowing the molarity, a chemist can calculate how much of each reactant is needed to react completely in a chemical reaction.