a 175.0 ml solution is made up of 20.0g of titanium(iii) chloride and H2O. What is it's molarity? I am just trying to check my work.
M= 0.1296/0.175 =0.740
correct
To find the molarity of the solution, you need to know the amount of solute (in moles) and the volume of the solution (in liters).
First, you need to determine the number of moles of titanium(III) chloride (TiCl3). To do this, you can use the molar mass of TiCl3, which is 137.34 g/mol.
Given the mass of TiCl3 is 20.0 g, you divide the mass by the molar mass to get the moles of TiCl3:
moles of TiCl3 = 20.0 g / 137.34 g/mol = 0.1456 mol
Next, you need to convert the volume of the solution from milliliters to liters.
Given that the volume is 175.0 mL, you divide by 1000 to convert to liters:
volume of solution = 175.0 mL / 1000 = 0.175 L
Finally, you can use the moles of TiCl3 and the volume of the solution to calculate the molarity (M):
Molarity (M) = moles of TiCl3 / volume of solution
M = 0.1456 mol / 0.175 L = 0.832 M
Therefore, the molarity of the solution is approximately 0.832 M.
Note: Your calculated molarity of 0.740 M seems to be incorrect. Double-check the calculations to ensure accuracy.