. Solubility Calculate molality of . g of ethanoic acid (CH COOH) in g of benzene. Molar mass of C H O : × + × + × = g mol – Moles of C H O = .
g g mol − = . mol Mass of benzene in kg = g/ g kg – = × – kg Molality of C H O = Moles of C H O kg of benzene . mol g kg g − = . mol kg – .
Calculate the mass percentage of benzene (C H ) and carbon tetrachloride (CCl ) if g of benzene is dissolved in g of carbon tetrachloride. . Calculate the mole fraction of benzene in solution containing % by mass in carbon tetrachloride. .
Calculate the molarity of each of the following solutions: (a) g of Co(NO ) . 6H O in . L of solution (b) mL of . M H SO diluted to mL.
. Calculate the mass of urea (NH CONH ) required in making . kg of . molal aqueous solution.
. Calculate (a) molality (b) molarity and (c) mole fraction of KI if the density of % (mass/mass) aqueous KI is . g mL - . Every solid does not dissolve in a given liquid.
While sodium chloride and sugar dissolve readily in water, naphthalene and anthracene do not. On the other hand, naphthalene and anthracene dissolve readily in benzene but sodium chloride and sugar do not. It is observed that polar solutes dissolve in polar solvents and non polar solutes in non- polar solvents. In general, a solute dissolves in a solvent if the intermolecular interactions are similar in the two or we may say like dissolves like .
When a solid solute is added to the solvent, some solute dissolves and its concentration increases in solution. This process