the density at 20 degrees celcius of a .258m solution of glucose in water is 1.0173 g/ml, and the molar mass of glucose is 180.2 g/mol. What is the MOLARITY of the solution? i need an explanation on how to go about solving this...
Here is a page that gives this information plus other interesting combinations you may need form time to time.
http://chemistry.twu.edu/tutorial/ConcConvSum.html
Post your work if you need additional assistance. Or we shall be happy to check your work.
You should not have double posted. Bob Pursley told you how to work the problem. The site I posted may still be of help to you.
To find the molarity of the solution, we need to understand the relationship between molarity, density, and molecular weight. Here's the step-by-step process to solve the problem:
Step 1: Calculate the mass of the glucose in the solution:
Mass = Density x Volume
Given that the density of the solution is 1.0173 g/ml and the volume is 0.258 m, we can calculate the mass as follows:
Mass = 1.0173 g/ml x 0.258 ml = 0.2628 g
Step 2: Determine the number of moles of glucose:
Moles = Mass / Molecular Weight
The molecular weight of glucose is given as 180.2 g/mol. Plugging in the values, we get:
Moles = 0.2628 g / 180.2 g/mol = 0.001459 mol
Step 3: Calculate the molarity of the solution:
Molarity = Moles / Volume
Given that the volume of the solution is 0.258 L (converted from 0.258 m), we can calculate the molarity as follows:
Molarity = 0.001459 mol / 0.258 L = 0.00566 M (rounded to five decimal places)
Therefore, the molarity of the glucose solution is approximately 0.00566 M.
Note: In this calculation, it is important to ensure that the units are consistent. Make sure to convert the volume from m^3 to L and the mass from g to kg if necessary.