Titration Worksheet Pdf
Charise Scrivner
We use Eventbrite to manage event bookings. If you view or interact with this content, Eventbrite may store cookies on your device for functional, analytical or targeting purposes. Please accept cookies to book your place, or visit the event listing at Eventbrite.
This content is provided by " + networkList[key] + ". If you view or interact with this content " + networkList[key] + " may store cookies on your device for functional, analytical or targeting purposes. Please accept cookies to use this content.
The accompanying activity requires learners to name, describe the purpose and draw a simple diagram of each piece of apparatus, with follow-up questions on how to use the equipment and accuracy of measurements.
Each reading you take from a burette has an accuracy of 0.05 cm3. When you take two readings, this accuracy is doubled. Because the volume delivered by the burette is variable, this accuracy has a bigger impact when you measure smaller volumes. This is clear when the accuracy is expressed as a percentage.
In titration, the end point is a complete reaction between the reactant solutions in the burette and the conical flask. You will often use an indicator to give a colour change, but some titrations are self-indicating.
A friend that I work with teaches chemistry in a school within a school. She was trying to find a lab to help students review at the end of the semester. After a little brainstorming together we decided to use an idea from Bob Worley. Last May, I wrote a blog about a titration lab. Bob had posted a comment and proposed an idea that really stuck in my head. He suggested that instead of doing a formal acid base titration, why not do it through mass instead of volume? See the video below. Apparantly, back in the day, scientists believed that once instrumentation improved, gravimetric titrations would provide better results. Since scales were not that great at the time they turned to using volumes for analysis. Using volumes works well, but why not give gravimetric analysis a try? Maybe we could also turn this into a great review of the semester content.
I started by standardizing a sodium hydroxide solution of about 0.15 M with KHP. I then used the standardized sodium hydroxide solution to standardize two solutions of HCl. The two acidic solutions were about 0.20 and 0.10 M. I made 250 mL of each solution. I estimated that students could run multiple trials of titrations with these solution and I would have enough for about the next 5 years of class. Next, I made the "stand" for the berel pipette. I bought some really cheap plastic cardboard that is used for yard and election signs. I made a rectangle with a small open area in the bottom middle. I cut two slits in the rectangle and took another approximately two inch by twenty four inch piece that I bent and placed each end in the slits. This created a tripod type of stand (see figure 1). Above the cut out in the rectangle I poked some holes for plactic zip ties. I was able to slide the pipette into the ties. I also ordered some inexpenive "Hoffman clamps" to place on the fat end of the pipette (see figure 2). These clamps allow a student to carefully dial in the drops. The end of the pipette was pulled tight and then cut off. This made the drops much smaller. The smaller ends and the "Hoffman clamps" allows for students to carefully dial in extremely small amounts of liquid.
Students were instructed to obtain a small vial and put in a few drops of phenolpthalein. They were to find the mass of the vial and its contents. They then had to fill the vial about one third full with one of the two acids and record the new mass. Students then obtained the base. They filled the pipette with the special tip with the basic solution. They placed the pipette in the apparatus, added the Hoffman clamp and carefully added base to the acid until they saw the first permanant change of color. They recorded the mass of the vial and repeated the procedure for a second trial. Watch the video below to see exactly how the lab is set up.
There are many ways teachers can direct students to analyze the data from this activity and use it to review the material covered over the entire semester. Here are some questions that a teacher could ask.
ChemEd X invites practitioners in the chemistry education community to share their experiences, knowledge and the resources they use in their classroom and laboratory. ChemEd X includes teachers and faculty from many diverse educational settings and who serve all students. We encourage contributions that demonstrate the particular opportunities found in teaching chemistry to diverse audiences from the entire breadth of learning environments.
In this thermometric titration instructional activity, students titrate hydrochloric acid with sodium hydroxide to determine the concentration of hydrochloric acid. They measure the change in temperature of the solution, plot their data and use the graph to find the concentration of hydrochloric acid.
Teach your high school students how titrations are used for volumetric analysis by completing using this 4 page worksheet and PowerPoint with theory, example calculations and simple acid-base lab. Answers are included.
We want to add exactly the right amount of acid - not too much and not too little. This might be because we need to get rid of the alkali, or it might be because the neutralisation reaction makes a useful salt.
3. Add a few drops of indicator to the alkali. A good indicator to use is phenolphthalein. This is pink in alkali, and colourless in acid. Since it only has two colours, it changes sharply, so we know when neutralisation has happened.
4. Fill a burette with acid. A burette is a long cylinder with a tap at the bottom, and a measuring scale along it. Clamp the burette above the conical flask, and record the volume of acid in the burette at the start of the experiment. The setup should look like this:
6. The indicator will change colour suddenly. This is called the endpoint because it is when the alkali is completely neutralised. When this happens, close the tap. Record the amount of acid left in the burette.
6. Add the rest of the acid, very slowly - drop by drop, swirling all the time. Just before you reach the end point, you will see pink and colourless regions in the flask at the same time, a bit like in this beaker:
The titration method has lots of steps - the key to learning them is to remember that we are trying to find out how much acid it takes to neutralise this particular alkali; that we need to measure this very accurately and precisely (so we add the acid very slowly); and that we need to be safe (so we wear goggles, and put the alkali in the flask).
We hope you've enjoyed trying some of our activities. We're here to help each child succeed. Get started for free to track progress, measure results and access thousands of educational activities in English, maths and science.
Beer's Law states that there is a linear relationship between concentration of a colored compound in solution and the light absorption of the solution. This fact can be used to calculate the concentration of unknown solutions, given their absorption readings. First, a series of solutions of known concentration are tested for their absorption level. Next, a scatter plot is made of this empirical data.
In this next part of the tutorial, we will work with another set of data. In this case, it is the titration of a strong acid with a strong base (see Figure 10 for the final plot). With this titration, a strong base (NaOH) of known concentration is added to a strong acid, HCl (also of known concentration, in this case). As the strong base is added to solution, its OH- ions bind with the free H+ ions of the acid. An equivalence point is reached when there are an equal number of free OH- & H+ ions in the solution (pH = 7). This equivalence point can be found with a color indicator in the solution or through a pH titration curve. This part of the tutorial will show you how to do the latter.
All of the points of the titration data can be connected to form a smooth curve. With this approach, the curve is guaranteed to go through all of the data points. This option can be used if you have only one pH reading per amount of NaOH added. If you have multiple pH readings for each amount added on the scatter plot, you will not end up with a smooth curve. To add lines to the scatter plot (Figure 9):
Titration and pendulation are important concepts in somatic therapy that involve working with the nervous system to regulate emotions and release tension. This Somatic Therapy Titration and Pendulation Worksheet will help you work with your therapist to navigate the process of titration and pendulation and help you express your thoughts throughout the process. TherapyPatron.com helps you streamline the therapeutic process so that your clients can be their best selves. Our editable, fillable, printable PDFs are perfect for counselors, psychologists, psychiatrists, social workers, therapists, and other mental health professionals.
Q. I'm the new and only lab tech at my job (Chemist fired). I have been tasked with figuring out how much of what to add to bring this tank back to life.
I have a 790 gal hard coat anodize tank which we would like to decant but still maintain a 6 g/L Aluminum content. My free sulfuric acid content would like to be at 160 g/L but the range is 140-190 g/L.
My last titration results are as follows:
261.66 total acid
152.88 free acid
19.98 g/L Al (range is 3-20)
2.11% b.v. AANF
I know that we figure 19 gal/inch and 3.79 L/gal, but after that I'm lost
I've read many of your answers/explanations and was hoping you could help me? You [ed. note: Tina is addressin Rachel Macintosh] seem to not just answer but explain the why's and how's and it just makes sense when I read your interpretation.
Thank you!
TinaMarie