Welcome to StudyStack, where users create FlashCards and share them with others. Click on the large flashcard to flip it over. Then click the green, red, or yellow box to move the current card to that box. Below the flashcards are blue buttons for other activities that you can try to study the same information.
Reset Password Free Sign Up

Free flashcards for serious fun studying. Create your own or use sets shared by other students and teachers.

Remove Ads
Don't know (0)
Know (0)
remaining cards (0)
To flip the current card, click it or press the Spacebar key.  To move the current card to one of the three colored boxes, click on the box.  You may also press the UP ARROW key to move the card to the "Know" box, the DOWN ARROW key to move the card to the "Don't know" box, or the RIGHT ARROW key to move the card to the Remaining box.  You may also click on the card displayed in any of the three boxes to bring that card back to the center.

Pass complete!

"Know" box contains:
Time elapsed:
restart all cards

Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

  Normal Size     Small Size show me how



Does H+ ever exist on its own in water? NO --> always as hydronium
What is another name for hydration? solvation
How to calculate normality? Molarity of solution * number of H
molarity (M) mol solute / L of solution
molality (m) mol solute / kg of solvent
Calculate parts per million? X mg / kg = X mg / L
Ksp: MX2 Ksp = [M][2X]^2
What does solubility = for MX2? value of M
Common ion effect Less will dissolve in a solution where the species already exists
Acids are more soluble in _____. Bases are more soluble in ____. bases / acids
Complex ion metal cation bound to a Lewis base (charged or uncharged)
When a complex ion like M-Cl is formed, will more or less of AgCl dissolve? More --> Cl is taken out of solution, so more of AgCl should dissolve
Are complex ions soluble in water? YES --> charged species
lattice energy interionic forces in crystal
solvation energy strength of attraction btwn solvent and dissociated ions
Which part dissolves fastest? corners followed by edges and faces
What is a saturated solution? rate of dissociation = rate of precipitation
Supersaturated solution? solution is a suspension created at high temperature
An anion has more ___ than ____. A cation has more ____ than ____. -electrons / protons -protons / electrons
How to use spectroscopy to determine amount of dissolved salt? amount of absorbed light at a fixed wavelength depends on conc. of ions
Which cpds precipitate first? cpds with smallest value for x (molar solubility)
Ion exchange column precipitate out ion that forms less soluble salt and release more soluble ion into solution to replace it
What is a chelating agent? substance whose molecules form several bonds to a single metal ion
How to form a coordinate covalent bond? lewis base donates a pair of electrons to lewis acid
Do ionic / covalent solutions conduct electricity? ionic
What color solution does nickel create and why? green --> unfilled d-orbitals
What does Ksp describe? how much will dissolve in solution
How is a precipitate formed in relation to Ksp? exceed Ksp and form a precipitate
What is a metathesis reaction? double dispalcement
When you swallow something toxic, do you want it to be more or less soluble? less soluble
Does a smaller Ksp imply higher or lower solubility of cpd in water? lower solubility --> lower conc. of cation and anion in aq. solution
Polar substances dissolve in ____ solvents. polar solvents
salt made of +1 / -1 are soluble
nitrate (NO3-) salts are soluble
Sulfate (SO4 2-) with +1 cations are soluble (excludes transition metals)
Most salts with -2 or -3 anions are insoluble in water, excluding sulfate salts
Most oxide (O2-) and hydroxide (OH-) salts are only slightly water-soluble
KOH and NaOH are prett soluble
In ionic structures, are electrons shared? NO --> transferred btwn atoms -cation = deficiency , anion = abundance of electrons
salt nomenclature cation + anion -ium + -ide
lower solubility means? less dissolution in solution --> less ions
Magnesium hydroxide is most soluble in acid / base? acid
basic salts are most soluble in acid / base acid
NH4+ is acidic / basic acidic
What does a precipitate do to an ion? takes it out of solution
Created by: 507935299

bad sites Copyright ©2001-2015  StudyStack LLC   All rights reserved.