The water quality index is made up of multiple tests that include the following: pH, Turbidity, Temperature, Dissolved Oxygen, Nitrates, Phosphates, Total Solids, Fecal Coliform Bacteria, and Biological Oxygen Demand. It brings all of this data together to form one rating on the health of the stream. (Abid, 2011) Then that number is put on a percentage scale, which is easy to interpret, even by the public. (Abid, 2011) pH is the first test that measures acidity. pH is the first test, and is important because it measures how acidic the water is, with the normal range around seven.
9. What is meant by “dynamic equilibrium”? EQUILIBRIUM APPLICATIONS: SOLUBILITY 1. a) Calculate the solubility of AgBr in pure water. Ksp of AgBr is 7.7(10-13 [8.8(10-7 mol/L] b) Calculate the solubility of AgBr in a 0.10 mol/L NaBr solution. [7.7(10-12 mol/L] 2.
• It uses a scale to describe the acidity level and the pH scale ranges from 0 to 14. A pH of 7 is neutral. A pH less than 7 is acidic. A pH greater than 7 is basic. c) Name 2 different methods of measuring pH of substances (in a laboratory)?
It would be classified as a base, if the number given by the probe was higher than seven. It is considered an acid, if the number given by the probe was lower than seven. If the number was seven it would be classified as neutral. Water and acetic acid is what makes up Vinegar. It was important to know what vinegar was made up of to fine the percent composition when continuing on with the second investigation of this laboratory.
Alkalinity can be defined as the capacity to neutralize acids. Carbonates (CO32-) are a major constituent in natural water that helps it behave as a buffer. Acid rain can reduce the alkalinity of water and hence would decrease its pH. In this experiment, water sources that measure pH below 5.6 will be considered acidic precipitation. Water from a variety of sources that receive precipitation is being sampled.
The concentration of a solution is the amount of solute that is dissolved into each unit of solvent. In this lab, water (H2O) will be the solvent and sugar/sucrose (C12H22O11). When the density of the solute is greater than the density of the solvent, the density is directly proportional to the concentration of the solute. The relative density of the solute to the solvent can be observed by placing some solute into the solvent without mixing. If the solute floats, then the density of the solvent is greater than the density of the solute.
This particular reaction is a strong acid and a strong base which means that when the reaction reaches the equivalence point, the moles of the acid and the base are equal and the solution is neutral so the pH should be around 7.0 depending on the final volume of each solution. To get this data, we will titrate an HCl solution with NaOH solution of which is a known concentration. We will record the initial and final reading of the NaOH while we record the pH of the titrated solution in the beaker. We will repeat this process with a solution of acetic acid which is a weak acid with NaOH and record the initial and final reading of NaOH and the pH of the solution in the beaker. Procedure Preview Calibrate the pH meter.
One mixture will contain vinegar, and the other will contain distilled water. What I expect to find it that the mixtures containing the vinegar’s pH will remain relatively constant, while the distilled water mixture will change drastically. Results and Observations: 1) The colors of the mixtures varied from drop to drop. One mixture turned blue, while the other turned a gold-ish color. Data Table 1: Add 0.1 M HCl| Drops|pH|Color| 0|6.0|Yellow| 1|6.0 |Yellow| 2|6.0|Yellow| 3|6.0|Yellow| 4|6.0|Yellow| 5|6.0|Yellow| 6|6.0 |Yellow| 7|6.0 |Yellow| 8|6.0 |Yellow| 9|6.0 |Yellow| 10|6.0 |Yellow| 11|6.0 |Yellow| 12|6.0 |Yellow| 13|6.0 |Yellow| 14|6.0 |Yellow| 15|6.0 |Yellow| Data Table 2: Add 0.1 M NaOH| Drops|pH|Color| 0|6.0|Yellow| 1|6.0|Yellow| 2|6.0|Yellow| 3|6.0|Yellow| 4|6.0|Yellow| 5|6.0|Yellow| 6|6.0|Yellow| 7|6.0|Yellow| 8|6.0|Yellow| 9|6.0|Yellow| 10|6.0|Yellow| 11|6.0|Yellow| 12|6.0|Yellow| 13|6.0|Yellow| 14|6.0|Yellow| 15|6.0|Yellow| Data Table 3: Add 6M HCl| Drops|pH|Color| 0|6.0|Yellow| 1|5.8|Yellow Orange| 2|5.6|Yellow Orange| 3|5.4|Light Orange| 4|5.0|Orange| 5|4.5|Orange| Data Table 4: Add 6M NaOH| Drops|pH|Color| 0|6.0 |Yellow| 1|6.2|Yellow Green| 2|6.4|Yellow Green|
The salts will be dissolved in distilled water by small quantities until the reaction reaches When ionic compounds dissolve in water, they either absorb energy from or release energy to the surroundings. If a chemical reaction absorbs heat from the surroundings, it is an endothermic reaction. If a solution releases heat to its surroundings, it is an exothermic reaction. The enthalpy of dissolution is the enthalpy change associated with the dissolution of a substance in a solvent at a constant pressure. The change in enthalpy relies on the concentration of the salt solution, because different concentrations will produce different enthalpies.
To understand the important role of the carbonic acid/bicarbonate ion buffer system in maintaining homeostasis, especially with regard to ventilation. Experiment was to show how the buffering agent minimized the change in pH (WCCC,2014) II. Introduction (Background info.) Homeostatsis is the maintenance of a relatively stable internal ennvironment. For Cells to survive, the composition of the surrounding fluids must remain relatively stable.