What is the molarity of a solution that contains 2.35 g of NH3 in 0.0500L of solution?

Question

A)1.00MB) 47.0 MC) 27.6MD) 2.76ME)0.0276M

Sarai Dooley Jr. · Accepted Answer

You have 2.35g in 0.0500 litres or 1 /0.050*2.35 = 47g per litremolar mass of NH3 = 17g/mol 147g = 47/17 = 2.765moles per litreMolarity = 2.76M , answer D

Sarai Dooley Jr. · Answer

Here is a descriptive solution to this problem:Given:Weight of NH3 = 2.35 gVolume of solution = 0.0500 LSolution:Molarity = Number of moles per liter of solutionMolarity = Number of moles / 1LNumber of moles = Weight / Molecular Weight (Mass)Molecular Weight (Mass) of NH3 = (1)(14) + (3)(1) = 17 g / moleNumber of moles = 2.35 g / 17 g / moleNumber of moles = 0.1382 moleMolarity = 0.1382 mole / 0.0500 LTherefore:Molarity = 2.765 Molar (Prepared in a 50 mL volumetric flask using 2.35 g NH3)Answer is D).Good Luck !!!!

Sarai Dooley Jr. · Answer

You need to find out how many g there are in 1L:2.35 in 0.05L = 2.35 / 0.05 in 1L = 47g.The molar mass of ammonia is: 17 g per mole.47 / 17 = 2.76M.

Sarai Dooley Jr. · Answer

Answer is D....2.76MMolarity = (grams of NH3 / M.W. of NH3) / liters of solution

Sarai Dooley Jr. · Answer

1 mole NH3 = 1(N) + 3(H) = (1x14) + (1x3) =17gNumber of moles = mass present in solution/mass of 1mole=2.35g/17g=0.138molesconcentration = number of moles/volume=0.138/0.5 = 0.276/mol/l

Dr. Karlee Tillman

What is the molarity of a solution that contains 2.35 g of NH3 in 0.0500L of solution?

5 Answers

AI-Powered Insights

Want to answer this question?

Categories

Tags

Related Questions