Apr 22- Ions in Solutions

On thursday's class we learned about ions in solutions.

- The formation of a solution depends on the ability of the solute to dissolve in the solvent.
- Solvation is the interacting between solutes and solvent.
- Ionic solds are crystals made up of ions (salts)
- Molecular solids are crystals made up of neutral molecules.

- Dissolving ionic solutions produces ions in a process called dissociation
Ex. NaCl(s) --(H2O)--> Na+(aq) + Cl-(aq)
- Ionization is the break up of a neutral molecule into charged particles
Ex. CH3COOH ----> CH3COO(-) + H(+)

- Determining concentrations is relatively easy.
Ex. What is the [Cl-] in a solution of 0.50M
AgCl3 ----> Ag+(aq) + 3Cl-(aq)

What is the [NO3-] in a solution of 0.82M Fe(NO3)2?
Fe(NO)3 ----> 2Fe 2+(aq) + 2NO3-(aq)
0.83M --(X2)--> 1.64M

What is the [Cr2O7 2-] and [K+] when 3.5g is dissolved in 40mL of water?
K2Cr2O7 ----> 2K(+) + Cr2O7(2-)
294.2g/mol 3.5g divided by 294.2g/mol = 0.0119mol divided by 0.04L = 0.297M

What is the [NO3-] when 100mL of 0.6M AgNO3 is mixed with 200mL of 0.40M Mg(NO3)2?"
AgNo3 ----> A3(+) + NO3(-)
0.600M 0.600M 0.600M