Raoult's law states that the partial vapor pressure of a substance is equal to the total vapor pressure of the solvent multiplied by the mole fraction of the substance. This also takes into account things like ion dissociation in a solution [Van't Hoff factor].
Dalton's law of partial pressures says that in a mixture of non-reacting gases, the total pressure of these gases is equal to the sum of the partial pressures of the individual gases (where the partial pressure of a given gas is calculated by multiplying the mole fraction of that gas by the total pressure).
Therefore, Raoult’s Law deals with vapor pressures while Dalton’s Law deals with non-reacting gases. However, the sum of pressures given by Raoult’s Law will results in the total amount of pressure of the [vapor] solution (which follows Dalton’s Law). So Dalton’s Law still holds in that the sum of vapor pressures is the total vapor pressure.