WebMar 3, 2024 · A 0.520 g sample of an unknown nonelectrolyte compound is dissolved in 4.02 g of lauric acid (Kf = 3.90 °C/m). The freezing point depression is determine to be 4.20 °C. What is the molar mass of the compound? ... To find the molar mass of the compound divide grams by the number of moles . 0.520g/ 0.00433 = 120.1 g/mol. WebMay 4, 2013 · Original Question. A lab team places .0250g of an unknown solid acid in an Erlenmeyer flask. They neutralize the solid acid with 15.0ml of .210 M Na(OH)(aq).One mole of the acid reacts with one mole of the …
Molar Mass of Butane Lab Flashcards Quizlet - lab report.docx
WebExpert Answer. 1). Freezing is an exothermic process where heat released and state of matter changed to solid so entrop …. Freezing causes an in entropy increase decrease To determine the molar mass of an unknown from the freezing point depression, the freezing points of both the pure solvent and the solution need to be measured True False. WebStep 1. Make use of the chemical formula to determine the number of atoms of each element in the compound. Step 2. Multiply the atomic weight of each element with its … fn postoffice\u0027s
Worked example: Calculating molar mass and number of moles
WebApr 9, 2024 · Science Chemistry When 2.65 g of an unknown weak acid (HA) with a molar mass of 85.0 g/mol is dissolved in 250.0 g of water, the freezing point of the resulting solution is -0.259 °C. Part A Calculate K, for the unknown weak acid. The freezing point depression constant (Kr) for water is 1.86 °C/m. Express your answer using two … WebMay 22, 2024 · 2 Answers. Suppose the mass of the gas is m and its molar mass and the volume under the given conditions are M and V, respectively. Thus, the number of moles ( n) and the density ( d) of the gas under the given conditions is: Substitute these values in the Ideal Gas Law, P V = n R T . Since you know P, T, and d, numerically, you can calculate … WebWith such a molar mass, your substance may be nitric acid $\ce{HNO3}$, whose molar mass is $\pu{63 g/mol}$. But this choice is improbable, because, in aqueous solution, nitric acid is partly dissociated into ions. It could be ethanediol $\ce{C2H4(OH)2}$, with a molar mass of $\pu{62 g/mol}$. So it is hard to guess the nature of your solute ... fnp organization professional