When 100cm^3 of a saturated solution of KClO3 at 40°C is desperate; 14g of the salt is recovered. What is the solutions of KClO3 at 40°C (KClO3 = 122.5)
desperate? solutions? I don't know what you want. Please clarify.
To find the concentration of the saturated solution of KClO3 at 40°C, we need to use the given information about the volume and the amount of salt recovered.
First, let's convert the given mass of KClO3 (14g) into moles. We can use the molar mass of KClO3, which is 122.5 g/mol, to calculate the number of moles.
Number of moles of KClO3 = mass / molar mass
Number of moles of KClO3 = 14g / 122.5 g/mol
Number of moles of KClO3 = 0.114 moles
Next, we need to determine the concentration of KClO3 in the saturated solution. Concentration is typically expressed in moles per liter (mol/L) or molarity (M).
Since the volume of the solution is given in cubic centimeters (cm^3), we need to convert it into liters.
1 cm^3 = 1 mL
1 L = 1000 mL
Therefore, the volume of the solution in liters can be calculated as follows:
Volume of solution (in L) = 100 cm^3 / 1000 cm^3/L
Volume of solution (in L) = 0.1 L
Now, we can calculate the concentration (C) in moles per liter (M) using the formula:
C = number of moles / volume of solution
Concentration of KClO3 = 0.114 moles / 0.1 L
Concentration of KClO3 = 1.14 M
So, the concentration of the saturated solution of KClO3 at 40°C is 1.14 M.