This lab revolves around Molarity, which represents the relationship between the moles of something to the volume of the solution. So a solution that is 4.00 mol/L NaOH has 4.00 moles of NaOH for every liter of solution; or a solution that is only 250 mL in volume has 1.00 mole of NaOH. If we poured more water into the solution it would be diluted and the concentration would decrease. mol solute Molarity = L solution Acid-Base Neutralization reactions: acids and bases are chemical opposites-when they are in the presence of each other, they react and are both neutralized. The mole ratios of the reactions today are one-to-one; in other words, one mole of base will neutralize one mole of acid, or in other words: when neutralized the moles of base and the moles of acid will be equal. This is the molar relationship you will use today in this lab. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(1) Begin by preparing the titrant, NaOH: Weigh out approximately 2.00 g NaOH and transfer it to your 250 mL volumetric flask. Fill the bulb of the flask approximately 2/3 full of high purity water and mix until the NaOH is completely dissolved. Then fill with water to the marker and mix thoroughly. Preparation of base: Mass of NaOH used: Volume of solution: *Molarity of NaOH in mol/L