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- Answer the ff. problems; 1.) Compute the % mass of a solution containing 5g sodium chloride in 150g solution? What is the molality of the solution. What is the mole fraction of Sodium chloride? 2.) What is the molarity of a solution containing 15 g sulphuric acid in 150ml solution? What is the normality of the Solution?Calculate the molality of a solution that is prepared by mixing 35.5 mL of CH3OH (d=0.792g/mL) and 298 mL of CH3CH2CH2OH (d=0.811g/mL): Can you please show detailed steps, I know the right answer is 3.63Solve: A solution is prepared by dissolving 120 g KMnO4 in 2L of water at 25oC. The final volume of the solution is 2.12 L. Calculate the molarity, molality, osmotic pressure, boiling point, and freezing point. Kb = 0.51oC/m and Kb = 1.82oC/m (Please type answer no write by hend)
- An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (SG= 1.114; MW = 62.07 g/mole) and water at 20oC. The density of the mixture is 1.070 g/mL. Express the concentration of ethylene glycol as:a) Volume percentb) Mass percentc) Molarityd) Molalitye) Mole fractionA solution of table sugar in water contains 5.25% by mass sucrose. Calculate: a)the mass of sucrose in 225 g of solution b) the amount of solution needed to obtain 70.0 g of sucrose c) the mass of water contained in 450 g of the solution d)the mole fraction of sucrose and water in 5.25% by mass sucrose ANSWER THE LETTER D ONLY. ThanksSolve the problem: 1. A solution of H2SO4 H2SO4 containing 50.0% H2SO4 by mass has a density of 1.40 g/Ml. Express its concentration in terms of mole fraction, mole percent, molarity, molality and normality.
- What is the molality (m) of a solution prepared by dissolving 78.0 g ethylene glycol, HOCH2CH2OH, in 1500. g of water? Show work.A solution consists of 30.4 g of hydrochloric acid, HCl, and 99.6 g water and has a density of 1.12 g/mL.Calculate the weight percent of HCl, the molality of HCl, the mole fraction of HCl, and the molarity of HCl in the solution.Answer: weight percent = ________% molality = ______ m mole fraction = _______ molarity = ____ MKindly answer the following with proper sig figs and check the data below. Looking for: Mass of solute? Mass of solvent? Molality of the solution? Molar mass of the solute? % error of the MM of unknown solute? Thank you!
- How many grams of benzoic acid (molar mass = 122.12 g/mol) must be dissolved in 9.00 g of lauric acid to create a solution with a molality of 0.910 mol/kg lauric acid? (Hint: Pay attention to units)Given the following: density of water= 1 g/ml volume of water = 12ml mass of water= ? boiling point of water = 100 ° C. boiling point of solution = 104 °C. a.) what is mass of water and delta Tb=? b.) if Molar mass theoretical = 30 g/molew then what is m? c. ) What is the MM of the solute? d.) calculate the % error ? pls help me answer thankyouuuColligative properties such as freezing point depression were used to find the molar mass of an unknown compound (nowadays we have more advanced instrumentation/techniques). The overall equation is: ∆Tf = mKf since m = (mol solute)/(kg solvent) we can write: ∆Tf = [(mol solute)/(kg solvent)]Kf We can then reorganize the equation to solve for moles of solute: mol solute = (∆Tf )(kg solvent)/Kf Since we also know the mass of the solute used, we can plug this in to solve for molar mass: Molar Mass = grams solute / moles solute Calculate the molar mass of the solute from the data in the 3rd trial (2nd one with solute added) (hint: we want think of total grams of solute added and total temperature change)