First, two grams on an unknown white compound were given. The possible compounds the known could be were CaCO3, KNO3, NH4Cl, CaCl2, K2SO4, (NH4)2SO2, Ca(NO3)2, NaC2H2O2, K2CO3, MgCl2, Na2CO3, 0.1 M AgNO3, MgSO4, NaCl, 0.2 M BaCl2, KCl, NaSO4, Mg(s), HCl, HNO3, NaOH, HC2H3O2, H2SO4, and KOH. The solubility test required using a scale to measure .575 of our unknown white compound. The unknown compound was measured in a 100 mL beaker. Next, a 100 mL graduated cylinder was used to measure 60 mL of distilled water. The water was added to the compound and stirred with a glass-stirring rod until dissolved. Next, The flame test required the solution made during the solubility test. The experiment needed a metal wire that was dipped into the solution …show more content…
interface which plugged into a computer and Logger Pro opened. To calibrate the probe, Experiment-Set Up Sensors-Showed All Interfaces was selected and then Calibrate Now was on. The probe was cleaned in distilled water and dried. Then the probe was placed into a buffer solution. There was two buffer solutions, one with a pH of 4.00 and the other with a pH of 7.00. Each buffer was measured in a 100 mL graduated cylinder and contained in a 40 mL beaker. Once the reading of the buffer was stabilized, the program entered into reading 1. The probe was cleaned with distilled water and dried before being placed into the second buffer for reading 2. Once the second calibration was completed the pH probe was cleaned again. Next the probe was placed into the unknown solution. The unknown solution contained 20+ -0.05 mL of the unknown in a 40 mL beaker. A 10 mL graduated cylinder was used to accurately measure. The pH value of the unknown was recorded, and then the probe was removed again and cleaned. Last, the pH probe was placed into potassium nitrate. The potassium nitrate was contained in a 40 mL beaker, .520+ -.0005g of KNO3 dissolved in 20+ -0.5 mL. A 10 mL graduated cylinder was used to accurately measure. The pH of potassium nitrate was recorded and the probe was removed and …show more content…
The probe was cleaned with distilled water and dried before placing into the unknown solution. The solution was .500+-.0005g of the unknown compound dissolved in 20+-0.5mL of water contained in a 40 mL beaker. A 10 mL graduated cylinder was used to measure accurately. The conductivity of the unknown compound was recorded and then the probe was removed and cleaned. Next, the probe was placed in potassium nitrate solution. The solution contained .500+-.0005g of KNO3 dissolved in 20+-.5 mL of water in a 40 mL beaker. The probe recorded the conductivity of potassium
A hot plate was placed under the ring stand. 50 mL of 3.0 M NaOH in a 250 mL beaker and a stir bar was placed in the beaker. The beaker with NaOH was placed on the hot plate and 3.75 grams of NaAlO2*5H2O was placed in the beaker. The temperature probe was placed in the beaker with the solution, not touching the bottom of the beaker. The solution was heated and stirred till the solution dissolved.
The temperature probe was kept in the calorimeter until the temperature had been stabilized and was calibrated. A beaker was placed on a hot plate with dial turned between three and four. Another 100.00 ml of deionized water was added while the beaker is heating up. Using the temperature probe, the beaker was measured
To do the temperature and dissolved oxygen tests, stick the probe in the water, and it will show numbers. One will be the dissolved oxygen in ppm (parts per million) and the other will be the temperature of the water. To do the pH test, stick the pH paper in the water and compare the color it turns to the scale. To test nitrates, put clear water in a container and dirty water in another, and put powder in them. Shake them and then compare the color they turn to the scale.
Poisonous Animals The cane toad is an invasive species that came from Hawaii to Australia to eat the cane beetles. The cane beetles were causing a big problem as they were eating Australia’s sugar cane. Once introduced to Australia, the cane toad multiplied until its numbers reached up to 200 million. The toad eats snakes and lizards.
”Conducting. Solutions” purpose is to use different examples to explain conductivity. To explain, the evidence states, “A vinegar solution also contains only a few ions and conducts only a little electricity. But when these solutions are mixed, the ammonia reacts with the acid in vinegar (acetic acid), and they form a lot of ions. This is why the mixture of ammonia and vinegar conducts electricity very well.
This data gave the following calibration curve: To obtain the concentration of caffeine in the soda sample, the absorbance measured was plugged in as y to
Next, a 10 mL beaker is filled with 3 mL of HCl and measure 10 mL of ionized water into a 140 mL beaker. Carefully turn on laboratory burner and start cleaning the Nichrome wire by dipping it into concentrated HCl acid. Hold the Nichrome wire on top of the flame and repeat the step until the wire doesn 't show any color. When the wire is clean, dip the wire again with some of the acid and dip it into the solution with the unknown compound in it. Place the wire back into the flame again and observe the color of the flame.
Electrical conductivity (EC, mS.cm-1) were measured by Coductometer (YSI Model 35 yellow spring, OH, USA).
There are three separate forces that passively affect how potassium moves through cell channels. One way that affects it is the chemical gradient that occurs and pushes the element out of the cell to re-balance the chemical concentration. When the ions are then pushed out of the cell, automatically, they are drawn back to the cell. The molecule's positive charge is attracted to the negative charge of the proteins inside the cell, where therefore creates the chemical gradient. A second way is when the chemical and electrical gradients go up against one another because they urge the potassium ions to move in opposite direction, this therefore creates an electrochemical gradient.
They measure how much potassium is present; then
Then, the boiling tubes were left in a water bath at 45°C. After 5minutes, the boiling tub, labelled A, was withdrawn from the water bath. 4) The sample was filtered using a Buchner funnel, collected in a sample vile, labelled A, and positioned securely to dry and crystallise in an oven at 65°C. 5) After 45minutes, the boiling tube, labelled
For a general salt, AmBn, the equation would be: The equilibrium constant for such a salt would be: The solubility product expression matches the coefficients in the equilibrium equation, and that the solid is not included in the Ksp equation. In this experiment, you will determine the Ksp for the sparingly soluble salt potassium hydrogen tartrate (also called acid tartarate or bitartrate). It dissolves in water to give potassium ions and hydrogentartrate ions according to the following equation: KHC4H4O6 K+ + HC4H4O6-
3.1.1 Physical-chemical parameters The temperature of the reactor was stable at about 30 (±5)°C. Immediately after filling the reactor the pH was 5.5 and after one day the pH increased to 6.3 due to the addition of methanogenic leachate of pH 7. Afterwards the pH decreased progressively from 6.2 to 5.5 during the first 200 days. After day 200, pH increased steadily up to 7.3 at day 400 and remained steady until the end of the experiment at day 700. Conductivity increased from 22mS cm-1 to 36mS cm-1 due to the dissolution of salts into the leachate.
The purpose of the analysis of Module 9, is to find the Dissolved Oxygen concentrate (mg/l) by using a HACH HQ40d portable multi-meter (field instrument method) and a HACH Digital titrator (method 8215 or known as Winkler method) for a tap water sample and its duplicate drawn from the Churn splitter as a main source. Further, we analyzed the sample and its duplicate for (pH, Temperature, Conductivity, and TDS) by using (Oakton PCS tester 35 series). The obtained results compared to its precision by using the equation (1) below and compared within the EPA standard limits: 1. Precision (as RPD) %=
That caused a new initial reading of NaOH on the burette (see Table1 & 2). The drops were caused because the burette was not tightened enough at the bottom to avoid it from being hard to release the basic solution for titrating the acid. The volume of the acid used for each titration was 25ml. The volume of the solution was then calculated by subtracting the initial volume from the final volume. We then calculated the average volume at each temperature.