The temperature at which molarity of pure water is equal to its molality
Never a question like this before and I've been in the business a LOOOOONg time. Since M = mols/L solution and m = mols/kg solvent, then I think the temperature at which the density of water is 1.000 g/mL so google density H2O vs temperature and find that spot.
Calculate the volumeof benzene,C6H6,d=0.88g/ml,molar mass=78.11 g/mol isrequired to produce 1.5 x 10^3 kJ of heat according to the following reaction?
277K
To find the temperature at which the molarity (M) of pure water is equal to its molality (m), we need to understand the definitions of molarity and molality.
Molarity (M) is defined as the number of moles of solute per liter of solution. Molality (m), on the other hand, is defined as the number of moles of solute per kilogram of solvent.
In the case of pure water, since there is no solute, the number of moles of solute is zero. Therefore, the molarity of pure water is always zero, regardless of temperature.
To find the temperature at which the molarity and molality of pure water would be equal, we need to look at the equation relating the two:
Molarity (M) = Molality (m) * Density of the solvent (ρ).
Since the molarity of pure water is always zero, for the equality to hold, we need the density of water to be zero as well.
However, at any temperature above absolute zero, water will always have a non-zero density. Therefore, it is not possible for the molarity and molality of pure water to be equal at any temperature.
In summary, the temperature at which the molarity of pure water is equal to its molality does not exist as it is not possible for the molarity of pure water to be anything other than zero.