This document provides instructions for an experiment to measure the amount of gas produced from the reaction of citric acid and sodium bicarbonate. It notes that using a balloon in previous experiments allowed gas to escape, making measurements inaccurate. To improve accuracy, it proposes using a syringe with measurement markings inserted through a stopper into a bottle. Detailed steps and materials are provided for setting up the syringe bottle system and carrying out three trials of the experiment. Students are asked to consider questions about the reaction and reasons for using a syringe over a balloon.
تقرير عن جرائم الإخفاء القسري بحق طلاب الجامعات والمعاهد المصرية - مدى الرصد ...مرصد طلاب حرية
تقرير | عن جرائم الإخفاء القسري بحق طلاب الجامعات والمعاهد المصرية
مدى الرصد : 850 يوم - من 3 يوليو 2013 إلى 1 نوفمبر 2015.
من إصدارات منظمة "طلاب حرية " للحقوق والحريات | ضمن سلسلة من التقارير عن الانتهاكات بحق الطلاب خلال 28 شهر تحت عنوان "طلاب مصر بين المطرقة والسندان".
Classic, mini chemistry experiments- some require materials typically found in a high school chemistry lab, while others are extremely simple. Very straightforward!
Lab 9 Chemical Reactions IIPre-lab Questions1. What is a limi.docxsmile790243
Lab 9: Chemical Reactions II
Pre-lab Questions
1. What is a limiting reagent?
2. A student used 7.15 g of CaCl2 and 9.25 g of K2CO3 to make CaCO3. The actual yield was 6.15 g of CaCO3. Calculate the limiting reagent and the percent yield.
Experiment: Synthesis of Garden Lime
Procedure
**Take photographs of your experiment set up and your results. Submit them with your laboratory report.**
1. Table 1 provides an example set of data for 1.0 g CaCl2.
2. For Trial 1, weigh into a 250 mL beaker the amount of calcium chloride (CaCl2) shown in Table 1. Record the exact mass you weigh out in the Trial 1 column of the Data section.
3. Measure 50.0 mL of distilled water into a 100 mL graduated cylinder. Pour the water into the 250 mL beaker with the calcium chloride.
4. Stir the solution with a stirring rod until all of the calcium chloride is dissolved.
5. Weigh out 2.5 g of potassium carbonate (K2CO3) in a 50 mL beaker. Record the exact mass in the Data section.
6. Measure 25.0 mL of distilled water into a 100 mL graduated cylinder. Add the water into the 50 mL beaker containing the potassium carbonate.
7. Stir the potassium carbonate in the distilled water with a stirring rod until it is all dissolved.
8. Pour the K2CO3 solution into the 250 mL beaker that has the CaCl2 solution. Rinse the beaker that contained the K2CO3 with a few mL of water and add this to the CaCl2 solution. Stir the mixture.
9. As soon as the reaction begins, record your observations in the Data section. Continue stirring until you see no more precipitate forming.
10. Set up the funnel in the Erlenmeyer flask as shown in Figure 2.
HINT: Do NOT begin filtering yet!
11. Zero the scale and weigh a piece of filter paper and a watch glass. Record the masses of both items in the Data section.
12. Prepare a filtering funnel as shown in Figure 2: fold a piece of filter paper in half twice to make quarters, and open the paper to make a small cone (three quarters are open on one side and one quarter is on the opposite side). Place the paper cone into the funnel and hold it in place with your fingers. Pour a small amount of distilled water through the paper to secure it inside the funnel.
13. Filter the mixture by pouring it into the filter paper in the funnel. Use the stirring rod and distilled water in a wash bottle to transfer the entire solid into the filter paper.
HINT: For best results, be sure to transfer all of the precipitate into the filter paper. Use a rubber policeman if it is available to help with the transfer.
14. Rinse the remaining solid in the filter paper twice with distilled water from a wash bottle to rinse off excess sodium chloride (NaCl). After all the liquid has filtered through, rinse the product with approximately 5 mL of ethanol to aid in its drying. Allow the ethanol to completely finish filtering through the paper.
15. Remove the filter paper carefully so as to not lose any product. Gently unfold the filter paper and lay it flat on the pre-weighed wat ...
تقرير عن جرائم الإخفاء القسري بحق طلاب الجامعات والمعاهد المصرية - مدى الرصد ...مرصد طلاب حرية
تقرير | عن جرائم الإخفاء القسري بحق طلاب الجامعات والمعاهد المصرية
مدى الرصد : 850 يوم - من 3 يوليو 2013 إلى 1 نوفمبر 2015.
من إصدارات منظمة "طلاب حرية " للحقوق والحريات | ضمن سلسلة من التقارير عن الانتهاكات بحق الطلاب خلال 28 شهر تحت عنوان "طلاب مصر بين المطرقة والسندان".
Classic, mini chemistry experiments- some require materials typically found in a high school chemistry lab, while others are extremely simple. Very straightforward!
Lab 9 Chemical Reactions IIPre-lab Questions1. What is a limi.docxsmile790243
Lab 9: Chemical Reactions II
Pre-lab Questions
1. What is a limiting reagent?
2. A student used 7.15 g of CaCl2 and 9.25 g of K2CO3 to make CaCO3. The actual yield was 6.15 g of CaCO3. Calculate the limiting reagent and the percent yield.
Experiment: Synthesis of Garden Lime
Procedure
**Take photographs of your experiment set up and your results. Submit them with your laboratory report.**
1. Table 1 provides an example set of data for 1.0 g CaCl2.
2. For Trial 1, weigh into a 250 mL beaker the amount of calcium chloride (CaCl2) shown in Table 1. Record the exact mass you weigh out in the Trial 1 column of the Data section.
3. Measure 50.0 mL of distilled water into a 100 mL graduated cylinder. Pour the water into the 250 mL beaker with the calcium chloride.
4. Stir the solution with a stirring rod until all of the calcium chloride is dissolved.
5. Weigh out 2.5 g of potassium carbonate (K2CO3) in a 50 mL beaker. Record the exact mass in the Data section.
6. Measure 25.0 mL of distilled water into a 100 mL graduated cylinder. Add the water into the 50 mL beaker containing the potassium carbonate.
7. Stir the potassium carbonate in the distilled water with a stirring rod until it is all dissolved.
8. Pour the K2CO3 solution into the 250 mL beaker that has the CaCl2 solution. Rinse the beaker that contained the K2CO3 with a few mL of water and add this to the CaCl2 solution. Stir the mixture.
9. As soon as the reaction begins, record your observations in the Data section. Continue stirring until you see no more precipitate forming.
10. Set up the funnel in the Erlenmeyer flask as shown in Figure 2.
HINT: Do NOT begin filtering yet!
11. Zero the scale and weigh a piece of filter paper and a watch glass. Record the masses of both items in the Data section.
12. Prepare a filtering funnel as shown in Figure 2: fold a piece of filter paper in half twice to make quarters, and open the paper to make a small cone (three quarters are open on one side and one quarter is on the opposite side). Place the paper cone into the funnel and hold it in place with your fingers. Pour a small amount of distilled water through the paper to secure it inside the funnel.
13. Filter the mixture by pouring it into the filter paper in the funnel. Use the stirring rod and distilled water in a wash bottle to transfer the entire solid into the filter paper.
HINT: For best results, be sure to transfer all of the precipitate into the filter paper. Use a rubber policeman if it is available to help with the transfer.
14. Rinse the remaining solid in the filter paper twice with distilled water from a wash bottle to rinse off excess sodium chloride (NaCl). After all the liquid has filtered through, rinse the product with approximately 5 mL of ethanol to aid in its drying. Allow the ethanol to completely finish filtering through the paper.
15. Remove the filter paper carefully so as to not lose any product. Gently unfold the filter paper and lay it flat on the pre-weighed wat ...
Operation “Blue Star” is the only event in the history of Independent India where the state went into war with its own people. Even after about 40 years it is not clear if it was culmination of states anger over people of the region, a political game of power or start of dictatorial chapter in the democratic setup.
The people of Punjab felt alienated from main stream due to denial of their just demands during a long democratic struggle since independence. As it happen all over the word, it led to militant struggle with great loss of lives of military, police and civilian personnel. Killing of Indira Gandhi and massacre of innocent Sikhs in Delhi and other India cities was also associated with this movement.
Welcome to TechSoup New Member Orientation and Q&A (May 2024).pdfTechSoup
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How Much Gas Lab?
1. How Much Gas? How much gas is created in the reaction of citric acid and sodium bicarbonate?
2. How can we make the gas collection more accurate? Problem- balloon allowed the gas to escape and not all of the gas from the experiment was collected and with other methods it might not give us specific answers Solution- let’s change a few instruments Instead of a balloon, let’s use a syringe with measurement markings on it Check it out on the next slide
3. Bottle & Syringe System To make this, you are going to use a syringe, a stopper and a glass bottle. The syringe stopper will go up as gas in the experiment is produced The syringe has measurement markers to keep it accurate
4. The materials for our lab: Jar of sodium bicarbonate Jar of citric acid 1 spoon, 2-mL Glass bottle #1 rubber stopper with hole 35-mL syringe water Protective eyewear I will have organized these into material cubbies for you to use in class, but make sure everything is returned to the cubby for clean-up Citric Acid Solution: we are going to use a citric acid solution of 2 mL of citric acid/100 mL of water to reduce lab error
5. Here is our lab procedure: Take a material cubby to your lab table. Put on protective eyewear. Put one level 2 mL spoon of sodium bicarbonate into the glass bottle. Put stopper in the opening of the glass bottle. Take up 5 mL of citric acid solution in the syringe. Insert the tip of the syringe into the hole of the stopper. Push the solution into the glass bottle using the syringe plunger. Don’t remove syringe. Observe and record results.
6. Last step… 8. Dump the used experiment into a sink and conduct two more trials. It is NOT necessary to wash out the bottle between trials.
7. To Prepare for Class: Write down the procedure for the lab, because we will not review this during class time. Create a data table to record your observations. It could look like this…
8. Be thinking about these things while completing the lab… What causes the syringe plunger to go up during the reaction between citric acid and sodium bicarbonate? Why is a syringe more useful than a balloon to conduct this experiment? What really causes this reaction the sodium bicarbonate or the citric acid?
