I've posted this question now three times and no one has responded. I first posted it Sunday 2/11 at 1 pm. Meanwhile, other questions are being answered. Can someone please help...
Al^3+ forms a complex ALSO4+ in the presence of sulfate...
Al^3+ + SO4^2- = AlSO4+
with Kstab = 10^3.01
How many ppm Al(total) would be in equilibrium with gibbsite at pH 4 and 25 degrees celsius in the presence of 10^3- m
SO4^2- (consider only this one complex and assume activities = concentrations)
Am having a tough time with complexes, hope you can help. Thanks.
why not look again at the phase diagram and stop cheating by trying to get someone to do your coursework for you
I'm sorry to hear that your question hasn't been answered yet. It can be frustrating to not get a response. However, I'm here to help you understand the problem and guide you in finding the answer.
First, let's break down the problem step-by-step:
1. We are given that Al^3+ forms a complex AlSO4+ in the presence of sulfate (SO4^2-).
2. The equilibrium reaction between Al^3+ and SO4^2- is: Al^3+ + SO4^2- ⇌ AlSO4+
3. The equilibrium constant for this reaction, known as the stability constant (Kstab), is given as 10^3.01.
4. We need to calculate the concentration of total aluminum (Al(total)) in parts per million (ppm) at equilibrium with gibbsite at pH 4 and 25 degrees Celsius.
Now, let's understand some key concepts:
1. Gibbsite is an aluminum hydroxide mineral (Al(OH)3).
2. The pH value (4) tells us that the solution is acidic.
To solve the problem and find the concentration of Al(total) in ppm, we need additional information. Unfortunately, the information provided is incomplete as we don't have the initial concentration of Al^3+.
Here's what you can try to find the answer:
1. Check if there is any additional information provided that might have been missed in the question.
2. If there is no additional information, you can try searching for the solubility product constant (Ksp) of gibbsite at pH 4 and 25 degrees Celsius. This information can help you determine the initial concentration of Al^3+.
3. Once you have the initial concentration of Al^3+, you can set up an ICE (Initial, Change, Equilibrium) table and use the stability constant (Kstab) to calculate the equilibrium concentration of AlSO4+.
4. Finally, convert the equilibrium concentration of AlSO4+ to Al(total) in ppm by using the molar mass and multiplying by the appropriate conversion factors.
Remember, understanding complexation reactions and equilibrium calculations requires knowledge of chemistry principles. By reviewing your course materials and consulting textbooks or online resources, you can further enhance your understanding and tackle similar problems successfully.
I hope this explanation helps you approach the problem and find the answer you're looking for. If you have any further questions, feel free to ask.