# ion

1. ### What would Chlorine Ion React With?

If I had a box that had inside it a UV light an equal quantity of ozone (O3), and H3O+, which would be broken down because of the UV light to O, and O2, as well as H2O, and H+ because that is what the H3O+ would be broken down into. If I introduced one hypochlorite Ion (ClO−) or a chloride Ion...
2. ### Maintaining fluoride ion concentration

This is the problem: Fluoridation is done by continuously adding sodium fluoride to water drawn from a reservoir. Assume you are responsible for the fluoridation of your city's water. How many tons of sodium fluoride must you add to the water supply each year (365 days) to maintain a fluoride...
3. ### Molarity and Ion concentration question

I finally got to the last page of my assignment, and there is a problem I can't figure out how to do. It is this: Given the reaction below, if 52.2mL of 0.771M Ba(NO3)2 reacts with 65.9mL of 1.11M NaF, calculate the concentration of all ions in solution after the reaction. Ba(NO3)2 (aq) + 2NaF...
4. ### Redox Equation - Chlorate Ion

Dear Colleagues, I have been attempting to balance the redox oxidation of the chlorate ion to the perchlorate ion, but I cannot balance it correctly - any help would be appreciated with both balancing the equation and the no of charges on both sides of the equation ( using H and H2O atoms )...
5. ### Question about the common ion effect

A bit of theory to refresh your mind about the solubility product: Ks = the given solubility constant example: Ks = [Pb2+].[I-]^2 7,1*10^(-3) = [Pb2+].[I-]^2 -> The solubility of this compound is then: S= (Ks/4)^1/3 = 1,2 mol/L Now my question: What is the solubility of Ag2SO4 (Ks...
6. ### General Chemistry: Complex Ion Formation Question?

So the problem states: Treating one mole of Ag2O(s) with 1M (NH4)2SO4 gives as main Ag-containing products: Answer: 1 mole [Ag(NH3)2]+(aq) and 0.5 moles Ag2(SO4)(s) My question is: how do I get to this conclusion? How can a solid precipitate form from sulfate and silver ion in water...
7. ### AP Chemistry ion concentration help?

You mix 275mL of 1.20M lead II nitrate, Pb(NO3)2, with 300mL of 1.75M potassium iodide (KI). The lead II iodide is insoluble. Calculate the final concentration of Pb (lead II) ions, NO3 (nitrate) ions, and K (potassium) ions. I wrote the reaction forumla to be Pb(NO3)2 + 2KI --> PbI2 + 2KNO3...
8. ### Common Ion Effect

What mass of Mg(OH)2 will dissolve in 1.0 L of 0.050 mol/L solution of MgSo4(aq)? Here is my work I just want to know if my calculations are correct. Mg(OH)2 <--> Mg^2+ + 2(OH-) Ksp= [Mg^2+][OH-]^2 = 5.6X10^-12 ICE Molar Solubility | [Mg^2+] | [OH-]^2 Initial...
9. ### finding ion concentrations of solution in equilibrium

An excess amount of silver chloride is added to a beaker of 2 M sodium cyanide. Calculate the concentration of all ions, other than OH- and H+, that are in solution once the system reaches equilibrium. (Hint, there should be 5 other ions present) Please explain through your answer!! I'm really...
10. ### Ion dipole?

Is the interaction between the hydrogen on the water molecule and the iodine a weak ion-dipole interaction?? I know they are insoluble in water.
11. ### Put the following ion pairs in order of increasing force between them, using Coulomb’

Put the following ion pairs in order of increasing force between them, using Coulomb’s Law. (a) Fe3+, OH- separated by 1.1 nm (b) Ca2+, O2- separated by 1.3 nm (c) Mg2+, Cl- separated by 0.9 nm (d) Ba2+, N3- separated by 1.6 nm Final answer is (d) < (b) < (c) < (a) The notes that the teacher...
12. ### Calculating pH from deltaG° and Ion Concentrations

I've been working on this one for a few days, and I just cant seem to get the right answer. Consider the reaction I2(s) --> I- (aq) + IO3- (aq) Balanced= 3I2 + 6OH- --> 5I- + IO3- + 3H2O deltaG°= -153.8 kJ/mol The question: What pH is required for the reaction to be at equilibrium at 298 K...