1. Molarity Molarity (M) = # moles of solute/ # liters of solution Calculate the molarity of 557 mL of solution containing 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.)

2. Molarity 1.A student wishes to make a 0.213 M CaCl 2 solution using 9.58 g of CaCl 2. 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 M KOH solution forming 843 mL of solution. Calculate the concentration of the dilute solution. Why should the concentration be less? ANS: 1.06 M

3. Molarity A student wishes to determine the concentation (STANDARDIZE) a NaOH solution. The student titrates 21.83 mL of the NaOH solution using 23.81 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.

4. Molarity A chemist adds 3.82 M Nitric acid to 3.05 g of metallic copper. The reaction produces copper(II) nitrate, nitrogen dioxide, and water. 1. Write the balanced molecular equation. 2. Calculate the volume (mL) of acid required. ANS: 50.3 mL 3. Write the complete ionic equation. 4. Write the net ionic equation.