Solubility Equilibrium is an equilibrium constant for a solid dissolving in an aqueous solution. When there is a solid before the equilibrium sign and dissolved products after the equilibrium sign, it is talking about the solubility product. Also, referred to as Ksp. To solve Ksp you need the concentration of the two dissolved products. The equation of Ksp is... aA(s)⇌cC(aq)+dD(aq) Ksp= [C]ᶜ[D]ᵈ As, you can see pure solids and liquids are not included in the Ksp equation because they are already accounted for in the equilibrium constant. A Ksp with a large value has a lot of dissolved ions causing it to have …show more content…
Also, it had provided enough trials to find an accurate volume of Ca(OH)₂. The data collected gave enough information to find the mol of H⁺ ions which equaled the mol of OH⁻ ions because of neutralization. Furthermore, this helped to find the concentration of OH⁻, which helped find the concentration of Ca²⁺ because every 2 OH⁻ ions have one Ca²⁺ ion. That is why the concentration of Ca²⁺ was half of the concentration of OH⁻. With these two concentrations the Ksp was found which was 2.92 x 10^⁻⁵. The actual Ksp is 5.5 x 10^⁻⁶, therefore, there is a big difference. In fact, the percentage error is 431%. This could of happened because of some sources of errors in the …show more content…
(2013, October 2). Solubility Product Constant, Ksp. Retrieved November 18, 2015, from http://chemwiki.ucdavis.edu/Physical_Chemistry/Equilibria/Solubilty/Solubility_Product_Constant,_Ksp No Author. (n.d.). Acid-Base Indicators. Retrieved November 18, 2015, from http://www2.ucdsb.on.ca/tiss/stretton/Database/indicators.htm Xavier, L. (2014, November 23). Titration Fundamentals. Retrieved November 18, 2015, from http://chemwiki.ucdavis.edu/Analytical_Chemistry/Quantitative_Analysis/Titration/Titration_Fundamentals Clark, J. (2013, November 1). Acid-base indicators. Retrieved November 18, 2015, from
The lab utilized a spectrophotometer to figure out the absorbance of the five different Potassium phosphate solution and the absorbance of an unknown concentration solution. The absorbance of the unknown solution was used
Discussion: The percent of errors is 59.62%. Several errors could have happened during the experiment. Weak techniques may occur.
The equation shows how 1 mol of Na2CO3 reacts with 1 mol of H2SO4, so
Solutions have three different stages that the solutes can be classified in: isotonic, hypertonic, and hypotonic. Isotonic is when the solutions have equal amounts of solutes. Like equilibrium, there is no net change in the amount of water in either solution. When the solutions have different concentration of solutes then the one with less solute is hypotonic and the one with more solute is hypertonic. Hypotonic takes in the solute from the hypertonic side that gives away the solute.
The molar volume of the H2 in our experiment is very close to the theoretical molar volume, but I think that the deviation lies in the temperature of the H2O: in the first trial it is too high and in the second one too low.
Solubility is defined as the maximum amount of a substance that will dissolve in a given amount of another substance at constant temperature and pressure. Solubility is typically expressed in terms of maximum volume or mass of the solute that dissolve in a given volume or mass of a solvent. Traditionally the equilibrium solubility at a given pH and temperature is determined by the shake flask method. According to this method the compound is added in surplus to a certain medium and shaken at a predetermined time. The saturation is confirmed by observation of the presence of un-dissolved material. Saturation can also be reached if the solvent and excess solute is heated and then allowed to cool to the given temperature. After filtration of the
The purpose of this lab was to calculate the percent composition by mass of oxygen in potassium chlorate.
Extraction is a separation method that is often used in the laboratory to separate one or more components from a mixture. Sucrose was separated at the beginning because it is the most immiscible and it’s strongly insoluble. Next Acetylsalicylic Acid was separated which left Acetanilide alone. Variety steps could have led to errors occurring. For example the step of separation, when dichloromethane layer was supposed to be drained out, it could be possible some aqueous layer was drained with it. Which could make the end result not as accurate. Also errors could have occurred if possibly some dichloromethane was not drained out. Both way could interfere with end result of figuring the amount of each component in the mixture. The solids percentage were 22.1% more than the original. That suggests that solids weren’t separated completely which clarifies the reason the melting points that were recorded were a slightly lower than the actual component’s melting point. The melting point for Acetylsalicylic Acid is 136 C but that range that was recorded during the experiment was around 105 C to 118 C. The melting points were slightly lower than the literature value. Sucrose was the purest among all component due to its higher melting point which follows the chemical rule that the higher the melting point the more pure the component
This question refers to the example data given below. Using the rate law and the experimental values given below, calculate k.
There is also the potential of human error within this experiment for example finding the meniscus is important to get an accurate amount using the graduated pipettes and burettes. There is a possibility that at one point in the experiment a chemical was measured inaccurately affecting the results. To resolve this, the experiment should have been repeated three times.
Compared to the 0.5 M hydrochloric acid that was less concentrated, the more concentrated 2 M hydrochloric acid c...
A kurtosis value near zero indicates a shape close to normal. A negative value indicates a distribution which is more peaked than normal, and a positive kurtosis indicates a shape flatter than normal. An extreme positive kurtosis indicates a distribution where more of the values are located in the tails of the distribution rather than around the mean (Grad pad, 2013). A kurtosis value of +/-1 is considered very good for most psychometric uses, but +/-2 is also usually acceptable (Grad pad, 2013). The above graph shows GPA with a kurtosis of -.811; awhile the final kurtosis is -33.2.
At approximately 548 degrees Celsius all of the compound has been absorb by the solution (this is a recognised appropriate temperature in chemistry).
The Solubility of Potassium Nitrate Aim To investigate how the solubility of Potassium Nitrate is affected by Temperature. Background Knowledge Potassium Nitrate (KNO3) is an ionic compound. The strong ionic bonds hold the compound in an ionic lattice which gives KNO3 its crystalline structure. These ionic bonds also have other properties which will affect my investigation, I must be aware of these properties for greater accuracy in my method.
Firstly, we need to keep the chemical at a constant concentration. So, in this experiment we have chosen to keep hydrochloric acid at a constant concentration (5cm3). We could have, however, used Sodium Thiosulphate as a constant, but we had chosen to use Hydrochloric acid. Next, we must make sure that the solution is kept at a constant volume throughout the experiment. If the volume is different, then it could give different results if it was at a constant volume.