# Andrew H

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2. ## Need someone to check my work for finding # of ions in 1 pound of pure potassium.

That's weird I can see them now. When I first checked them it said they had been removed because the poster didn't have permission to link. I also found this 0:08 / 16:07 Week 8 - Potassium Sources (ENR 5270) that answers my K2O question and how to calculate the potassium content.

5. ## Need someone to check my work for finding # of ions in 1 pound of pure potassium.

I also am trying to figure out how many pounds of KCl I could need to get 1.25767 x 1029 atoms of potassium. I have sat here for 30 minutes thinking and I'm not coming up with numbers that makes sense. I first tried to find the number of atoms in 1lb. of KCl: [(grams in one pound)/(molar mass of KCl)] (6.02214 x1023) (atomic mass of Cl/molar mass KCl) = 1.742443813x1024 atoms of K in 1lb. KCl. Then I set up an equation to find how many pounds of KCl I need to get 1.25767 x 1029 atoms of potassium: (atoms of K in 1lb. of KCl)(X lbs.) = (atoms of K 1lb. of K2O) (1.742443813x1024 )(X lbs.) = (1.25767 x 1029 ) X = 72178.64459 This can't be correct. Thank you
6. ## Need someone to check my work for finding # of ions in 1 pound of pure potassium.

I'm back with another question. I looked and the MSDS for the product I plan to use again and noticed that potassium is listed as K2O. When I first read it and saw that it contained 10% K2O I just thought potassium. I didn't take the formula into consideration. This would change the amount of potassium atoms in a pound of material calculated by studiot, correct? So I could [(molar mass of K)(2)/(atomic mass of Oxygen)] ( molar mass of K2O) (6.02214 x1023) (453.592 grams) = 1.25767 x 1029, atoms of K in 1lb. of K2O? Before I did the math I thought I would have less potassium but I actually should have more. Same mass of glauconite double the atoms of potassium makes sense to me. I hope my calculation is correct. However, I'm not sure they actually measured or tested for K2O because no other other elements on the chemical composition report are given as oxides and I know there are iron oxides present in this mineral. Although, iron is what the report shows. I'm have no logical explanation other than that. Maybe the answer is buried in the depths of chemistry I am still learning. I have seen this with several mineral and rock fertilizer chemical composition reports, like limestone and dolomite. For example one lists Ca 38.4%, Mg 1.3%, CaO 48.7%, MgO 4%, CaCO3 87% and MgCO3 8.5%. Which I still need to learn why these are given and do not total 100%. I also don't understand why they given Ca and CaO content. It's limestone made of CaCO3 almost completely. Ca doesn't exist in this mineral without being bonded to something. I appreciate any input. Thank you
7. ## Need someone to check my work for finding # of ions in 1 pound of pure potassium.

Dear Strange, I completely understand. I would much rather have someone teach me how to problem solve so I can figure things out on my own.I have problem of getting excited by the idea of some of the advanced concepts I have a hard time sitting though months of review step by step like I should or I would have remembered Avogadro's number. You really can't do much in chemistry if you don't have a firm grasp on the basics, the math isn't hard it's learning to think like a chemistry that's challenging. In closing, I really appreciate a place like this to come and ask for help, get help, and a little wisdom on the side. Thank you
8. ## Need someone to check my work for finding # of ions in 1 pound of pure potassium.

Yea not home work I am learning independently. That makes total sense. Thanks for working it out so I could see it. I need practice. Thank you again.
9. ## Any Soil Scientists Out There?

Hello, thank you for your interest in helping. 1. How would I determine the quantity of KS04 to add to 5 pounds of clay with a CEC of 100 meq./100g in order to provided double the potassium ions in solution as there exchanges sites. I want to saturate a clay sample with potassium? Are there any tricks to getting ions moving other than adding more ions or creating movement in the water like using specific salts of potassium or maybe a third wheel ion like Na that would add to the pressure I am trying to push out the exchangeable aluminum from the clay before I use them in an aquarium soil where it could cause problems for a long time. 2. How do I use the ion exchange reaction models like the Beckett - Q/I Relationships to predict K, Ca, and Mg ions interactions in solution? I have some basic chemistry knowledge but skipping from what I am familiar with and remember from ten years ago to what some of those models are designed to do is a massive leap for me. I understand the concepts of thermodynamics and equilibrium but I am not up to speed with the nomenclature and I thought I would ask here to see if anyone can help me learn to use these ion exchange models by myself. I appreciate your time. Thank You
10. ## Need someone to check my work for finding # of ions in 1 pound of pure potassium.

I know this is simple but I would like to make sure I've used the right procedure to determine number of ions by knowing the total weight of mineral and % of an element of interest. I want to find number of atoms in one pound of pure potassium. So I took the molecular weight of potassium 38.963706 g/mol x 10+15 lb.-mol = 0 .003963706 kg/mol x 10+15 lb.-mol = 38,963,706,000,000 atoms in one pound of potassium. Thank you for your time!
11. ## Calcium carbonate vs. Magnesium Carbonate reaction with acid.

I have few more questions and one is about Dolomite. How does CaMg(CO3)2 disassociate and behave in slightly acidic water? I know from gardening that limestone powder raises pH faster that dolomite powder especially when watered into the acidic soil. Does means that Ca CO3 reacts faster with acids in solution than MgCO3? If reaction time with acids is significantly faster in CaCO3 this could be a useful tool to help maintain elevated CO2 levels. Because magnesium is bonded to the carbonate ion stronger than calcium is I think predicting how carbonate rocks with different Ca:Mg ratios will act over time can be done. Thank you for your time.
12. ## Calcium carbonate vs. Magnesium Carbonate reaction with acid.

I am trying to engineer an aquarium system that will maintain CO2 levels much higher than what is present if the atmosphere. I have many ideas to create these conditions. However, the avenue of producing CO2 through a chemical reaction is one that is giving me most trouble. I know how it works and understand the equations. Although I don't know how to quantify the CO2 release for this reaction do you quantify the about of CO2 being released in these two First of all I would like to learn reaction produced more CO2. I am asking this because I read some where that MgCO3 produced a lot more CO2 than CaCO3 does under the same conditions but it didn't explain why. I hadn't though about this much before but the amount CO2 produced by MgCO3 was so much greater it really had me wondering if it was true. If someone knows the answer and is willing to explain it to me I would appreciate it. CaCO3 + HCL > CaCl2 + CO2 + H20 or MgCO3 + HCL > MgCL2 + CO2 + H2O
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