Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
25 Cards in this Set
- Front
- Back
|
= Solute + Solvent
Homogeneous mixture |
Solution
|
|
|
What is the solvent primarily made up of?
|
water H2O
|
|
|
Examples of solutions (2)
|
gas in liquid
solid in liquid |
|
|
what type of solution is carbonated beverages (such as O2 in water)
|
gas in liquid
|
|
|
what type of solution is the ocean
|
solid in liquid
|
|
|
What happens when an ionic compound dissolves in water?
|
the ions separate and water molecules surround the ions
|
|
|
why do ionic compounds dissolve
|
because of its polarity
|
|
|
what does hydrate mean
|
surrounded by water
|
|
|
what is an electrolyte
|
ionic compound
|
|
|
what conducts electricity?
|
ionic compound
|
|
|
what happens when methanol dissolves in water
|
no ions are formed and the molecules are unchanged
|
|
|
electrolyte dissociation:
KF=== NaNO3== CaCl2== Na3PO4== (NH4)2SO4== |
K^+ + F^-
Na^+ + NO3^- Ca^2+ + 2Cl^- 3Na^+ + PO4^-3 2NH4^+ + SO4^2- |
|
|
covalently bonded such as molecular solutes such as sugars and alcohol
|
non-electrolytes
|
|
|
solution formation (mixing of solvent and solute); (deltaH<0).
net energy decreases hot |
exothermic
|
|
|
solution formation is (deltaH>0).
net energy increases cold |
endothermic
|
|
|
what is the formula for the heat of the solution
|
lattice energy solute(+) + enthalpy hydration (-)=enthalpy of solution
(whatever number is greater determines the answer) |
|
|
add solvent to lower concentration
|
dilution
|
|
|
what is the formula for dilution
|
M1V1=M2V2
|
|
|
solute to solution or solvent ratio
|
concentration
|
|
|
what is the formula and unit for:
molarity(M) molality(m) mole fraction mass percent |
(mol solute / L solution) (mol / L)
(mol solute / kg solvent) (mol / kg) (moles / total moles) (none) (mass solute / mass sol’n * 100)(%) |
|
|
what measure always stays constant with temperature
|
molality
|
|
|
what measure solute stays the same while the solvent is increased which lowers the concentration
|
molarity
|
|
|
500 g of 0.90% saline solution, NaCl(aq), are needed. The density of the saline solution is 1.1 g/mL.
1) Mass NaCl needed? 2) Molarity of solution? 3) Molality of solution? 4) Mole fraction of NaCl? |
1. 4.5 g NaCl
2. .169392 3. (4.5/58.45 mol solute / 0.4955 kg solvent 4. (445.5/18) mol H2O |
|
|
25.0 g of Mg(NO3)2 added to 200. g water to make a solution with a volume of 205 mL.
% by mass Mg(NO3)2? M of Mg2+? M of NO3-? m of Mg2+? m of NO3-? mol fraction Mg(NO3)2? |
1. 25g Mg(NO3)2 / 225 g soln X 100=
2. (25g/148.3) mol Mg^2 / 0.205 L Soln= 3. (25g/148.3) mol Mg^2 / 0.205 L Soln X 2 4. ((25g/148.3) mol Mg2 / 0.2 kg H20)) 5. ((25g/148.3) mol Mg2 / 0.2 kg H20)X 2) 6. ( (25/148.3) mol Mg (NO3)2 / (25.148.3) mol Mg (NO3)2 + (200/18)(-)mol H20 |
|
|
A 12.4 M HCl(aq) solution has a density of 1.2 g/mL.
Molality of solution? Mass percent HCl? |
1. 12.4 mol HCl / 1.2 kg H2O
2. (? g HCL/1200g soln) X 100 |
