What is the molarity of a solution that contains 2.35 g of nh3 in 0.0500 l of solution?

2 answers:

5 0

M = 2.76 M. To determine the molarity of any solution, the following equation is applied: M = n/V. Here, n signifies the number of moles of NH3, and V represents the solution volume in liters. Since we do not possess the moles of NH3, we must calculate it. Utilizing the mass, we can derive the moles with n = m/MM. Using the given mass and the reported molar mass of NH3 as 17.031 g/mol, we calculate: n = 2.35 g / 17.031 g/mol = 0.138 moles. With this mole quantity, the molarity calculation proceeds: M = 0.138 moles / 0.05 L, resulting in M = 2.76 mol/L. This value indicates the concentration, or molarity, of the NH₃ solution.

castortr0y [2.9K]7 days ago

3 0

Molarity is defined as the number of moles present in one liter of solution. Given the mass of NH₃ is 2.35 g and its molar mass is 17 g/mol, the moles of NH₃ in 2.35 g can be calculated as 2.35 g / 17 g/mol = 0.138 mol. Consequently, in a 0.05 L solution, the number of moles amounts to 0.138 mol. Therefore, the concentration in 1 L is: 0.138 mol / 0.05 L x 1L = 2.76 mol. Thus, the molarity of NH₃ is 2.76 M.

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