Mass Of Solution Lab Report

In this investigation, the mass (g) of a beaker and a graduated cylinder were calculated and recorded into a lab notebook. The density of distilled water was calculated without any NaCl by measuring the mass of a sample of water in a beaker, and then subtracting the mass of the beaker to leave the mass of water. This measurement was recorded into a lab notebook in Table 1 under “Total Mass of Solution” and “Mass of solution”. The contents of the beaker are then transferred to a graduated cylinder. The Measurement is recorded in a lab notebook in Table one under “Volume of Solution (mL)”. The percent mass of NaCl is zero because there was no NaCl was added to the sample. This is recorded into a lab notebook in Table 1 under “% w/w NaCl”. Density …show more content…
The beaker and the graduated cylinder were cleaned and dried. A small quantity of NaCl was measured out (Below 15% by mass of the solution). Then the mass (g) NaCl was measured and the mass of the beaker was subtracted. This number was recorded in a lab notebook in Table 1 under “Mass of NaCl (g)”. Then water was added to the NaCl. The mass (g) of the solution was measured, and the mass of the beaker was subtracted from the number obtained. Then was recorded in Table 1 under “Total Mass of Solution”. The beaker was stirred until no NaCl crystals could be observed. The Solution was moved to the graduated cylinder. The graduated cylinder’s mass (g) was measured. The mass of the graduated cylinder is subtracted from the measurement. The volume (mL) is measured in the graduated cylinder. The mass and the volume were recorded into a lab notebook in Table 1 under “Mass of Solution (g)” and “Volume of Solution (mL)”, respectively. The Density was calculated by diving the recorded mass by the recorded volume. This measurement was recorded in a lab notebook in Table 1 under “Density of Solution (g/mL)”. This process was repeated 4 …show more content…
The hotplate was preheated to 300 ̊C. While the hotplate was warming up, the sample was prepared. The mass of the hot dish with a watch glass were calculated and recorded in a lab notebook. A small amount of the unknown is poured into the hot dish (about the size of a quarter). The sample’s mass was measured with the solution in the hot dish. The mass (g) of the hot dish and watch glass are subtracted from the measurement. This was recorded in a lab notebook in Table 3 under “Mass of Solution Used (g)”. The sample was then placed on the hot plate with the watch glass over the hot dish. The unknown was left on the hotplate until there was no more condensation on the watch glass. The hot dish was placed on the lab counter, and left to cool. Once the hot dish has cooled down, the mass (g) of the hot dish measured. The mass of the hotplate and watch glass is subtracted from the measurement. This measurement is recorded in a lab notebook in Table 3 under “Mass of Remaining NaCl (g)”. The two measurements in sections “Mass of Remaining NaCl (g)” and “Mass of Solution Used (g)” are used to find percent by mass. This value is then recorded in a lab notebook in Table 3 under “% w/w