Determining the Molarity of a Solution

What is the molarity of a solution containing 17.0 grams of NH3 in 1200. mL of solution?

A. 0.0706 M

B. 0.998 M

C. 0.831 M

D. 1.20 M

E. 14.2 M

F. 0.998 M

Answer:

The correct answer is option C - 0.831 M molarity.

To determine the molarity of a solution containing 17.0 grams of NH3 in 1200 mL of solution, we first need to calculate the number of moles of NH3 present in the solution.

The molarity of a solution is defined as the number of moles of solute per liter of solution. The formula for molarity is given by:

Molarity = moles of solute / volume of solution (in liters)

In this scenario, the mass of NH3 is 17.0 grams and the molar mass of NH3 is 17.04 g/mol. First, we calculate the number of moles of NH3:

Number of moles of NH3 = Mass of NH3 / Molar mass of NH3

= 17.0 g / 17.04 g/mol

= 0.998 mol

Next, we need to find the volume of the solution in liters. The given volume is 1200 mL, which is equivalent to 1.2 L.

Substitute the values into the molarity formula:

Molarity = moles of solute / volume of solution (in liters)

= 0.998 mol / 1.2 L

= 0.831 M

Therefore, the molarity of the solution containing 17.0 grams of NH3 in 1200 mL of solution is 0.831 M.