Created by StemPy LabA laboratory stock of sodium chloride solution is labelled (molal), and its density is . A student needs its molarity, in moles per litre of solution, to plan a dilution, and she must not confuse the two terms. Atomic masses in : Na 23, Cl 35.5. What is the molarity of the stock solution?
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← A student dissolves 6.00 g of urea, CO(NH₂)₂ (molar mass 60 g mol⁻¹), in 100 g of water (molar mass 18 g mol⁻¹). The density of the solution is 1.02 g mL⁻¹. (i) Its molality is 1.00 mol kg⁻¹. (ii) The mass per cent of urea is 6.00%. (iii) Its molarity is also 1.00 mol L⁻¹. (iv) The mole fraction of urea is 0.0177. (v) If the solution is warmed in a sealed flask, its molarity stays the same. How many of the statements above are correct?An element X forms a volatile chloride that contains 83.5% chlorine by mass. At the same temperature and pressure, the vapour of this chloride is 85.0 times as dense as hydrogen gas. The atomic mass of chlorine is 35.5 u. A student first takes the formula to be XCl. What is the atomic mass of X? →
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