• Shuffle
Toggle On
Toggle Off
• Alphabetize
Toggle On
Toggle Off
• Front First
Toggle On
Toggle Off
• Both Sides
Toggle On
Toggle Off
Toggle On
Toggle Off
Front

### How to study your flashcards.

Right/Left arrow keys: Navigate between flashcards.right arrow keyleft arrow key

Up/Down arrow keys: Flip the card between the front and back.down keyup key

H key: Show hint (3rd side).h key

A key: Read text to speech.a key

Play button

Play button

Progress

1/19

Click to flip

### 19 Cards in this Set

• Front
• Back
 Name the 7 strong acids HCl HBr HI HNO3 HClO3 HClO4 H2SO4 Arrhenius definitions of acids and bases Acids produce H+ Bases produce OH- Bronsted-Lowry definitions Acids transfer H+ Bases receive H+ Lewis definitions Acids are election pair acceptors Bases are electron pair donors Autoionization of water constant 1 * 10^-14 at 25 degrees Celsius Le Chatelier's Principle If a system at equilibrium is perturbed by a change in temperature, pressure, or concentration, the system will shift its equilibrium position so as to (partially) counteract the effect of perturbation. "If you push the universe, it pushes back." Common Ion Effect Extent of dissociation of a weak electrolyte is decreased by adding a strong electrolyte that has an ion in common with weak electrolyte. HA <--> H+ + A- MA <--> M+ + A- Common ion comes from both wk acid and soluble salt. Addition of salt suppresses dissociation of wk acid. "Ions just want to be alone." Calculations via ICE table: As a general rule, it quantity of x is more than ____ of initial value, it is better to use the quadratic formula. 5% Henderson-Hasselbach Equation pH = pKa + log[HA]/[A-] How do you calculate the pH of a buffer solution? HA <--> H+ + A- MA <--> M+ + A- pH = pKa + log[salt]/[acid] Blood is a _____ solution that needs to stay in the pH range of _____. buffered, 7.35-7.45 (usually 7.4) The buffer system in blood is made from ____ and ____ and has a high capacity to neutralize ____. carbonic acid and bicarbonate acids HF HCl HBr HI Acid strength is ______ CH4 NH3 H2O HF Acid strength is ______ increasing increasing Ideal gas law PV = nRT R = gas constant = 0.08206 L-atm/mol-K Converting Kp to Kc Kp = Kc (RT)^delta n Dalton's Law sum of partial pressures = total pressure OR partial pressure = (mole fraction X)(total pressure) X = moles gas / total moles Insoluble solids dissolve slightly in H2O, measured by Ksp, the ________. Solubility is measured in units of _____. Molar solubility is defined by ____. Solubility can be strongly influenced by _____, _____, and __. solubility product constant g of solute/L of soln moles of solute that dissolve to form 1 L of saturated soln common ion effect complex ion formation pH Complex ion formation Occurs when ion of an insoluble compound can form a soluble complex ion in solution--> increases solubility, determined by Kf Assembly of a metal ion and Lewis base Multiply Ksp and Kf (formation constant) together Amphiprotic Amphoteric oxides and bases any molecule that can gain or lose a proton more specific: insoluble in neutral H2O, dissolve in stg acid or base, can behave as acid or base ex. Al3+, Cr3+, Zn2+, Sn2+