Molarity

Molarity (M) = # moles of solute/ # liters of solutionCalculate the molarity of 557 mL of solutioncontaining 0.143 mol HCl. Molarity(M) = # mol HCl/ # Liter soln

= 0.143 mol HCl/0.557 L soln = 0.257 M HCl (Round-off to 3 Sig.fig.)

Molarity1. A student wishes to make a 0.213 M CaCl2

solution using 9.58 g of CaCl2. Calculate the volume of the solution. ANS: 0.405 L

2. A student does a titration using 25.71 mL 0.09863 M NaOH. Calculate the moles and mass of NaOH used. ANS: 0.00254 mol (0.102 g)

3. A chemist adds 325 mL of water to 518 mL of 1.73 MKOH solution forming 843 mL of solution. Calculate theconcentration of the dilute solution. Why should theconcentration be less? ANS: 1.06 M

MolarityA student wishes to determine the concentation(STANDARDIZE) a NaOH solution. The studenttitrates 21.83 mL of the NaOH solution using23.81 mL of 0.1140 M HCl.1. Write the balanced neutralization equation.

2. Calculate the concentration (molarity) of NaOH. ANS: 0.1243 M 4 sig. fig.

Molarity

A chemist adds 3.82 M Nitric acid to 3.05 g ofmetallic copper. The reaction producescopper(II) nitrate, nitrogen dioxide, and water.1. Write the balanced molecular equation.2. Calculate the volume (mL) of acid required. ANS: 50.3 mL3. Write the complete ionic equation.4. Write the net ionic equation.