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159 Cards in this Set
- Front
- Back
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What do most chemical reactions in cells take place among?
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dissolved substances
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What is a solution?
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homogeneous mixture with a solute dissolved in a solvent
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What are water-based solutions?
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aqueous
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What does homogeneous mean?
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uniform in composition throughout
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What do solubility curves show? |
points where solution will become saturated at given temperatures
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What are multivalent elements and what are three examples?
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elements capable of forming more than one ion iron, tin, and lead |
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How are monoatomic anions named?
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-ide
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What ion(s) does scandium form? |
Sc 3+
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What ion(s) does yttrium form? |
Y 3+
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What ion(s) does iron form? |
Fe 2+ Fe 3+ |
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What ion(s) does copper form? |
Cu+ Cu 2+ |
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What ion(s) does silver form? |
Ag+
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What ion(s) does zinc form? |
Zn 2+
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What ion(s) does cadmium form? |
Cd 2+
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What is nitrate?
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NO3 -1
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What is sulfate? |
SO4 -2
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What is carbonate? |
CO3 -2
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What is hydroxide? |
OH -
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What is phosphate? |
PO4 -3
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What is acetate? |
C2H3O2 -1 CH3COO -1 |
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What is bicarbonate? |
HCO3 -1
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What is hydrogen carbonate? |
HCO3 -1
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What is chlorate? |
ClO3 -1
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What is ammonium? |
NH4 +1
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What is the difference between -ate and -ite polyatomic ions? |
-ate has one more oxygen no charge difference |
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What is ClO4 -1 called?
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perchlorate per is short for hyper |
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What is ClO -1 called? |
hypochlorite
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When does solution formation take place?
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when molecules of the solute can interact with molecules of the solvent
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How is each ion solvated in water?
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surrounded by water molecules
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How does water arrange around ions? |
hydrogens towards anions, oxygens toward cations
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What is solvation known as in water? |
hydration
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What is a hydration shell? |
surrounding group of water molecules around dissolved ion or molecule
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What is the hydration number? |
number of water molecules surrounding a dissolved ion
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How do nonpolar solutes dissolve in nonpolar solvents? |
London dispersion forces
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What is an electrolyte?
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compound that dissolves in water to form ions
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Does electrolyte strength depend on the identity of the ions? Why or why not? |
No, it depends on the number of ions produced.
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Are sodium salts electrolytes? |
yes, strong
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What ionic compounds are always soluble in water?
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compounds with group 1 metals or ammonium ions
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Are compounds containing nitrate soluble or insoluble in water?
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soluble
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Are compounds containing Cl-, Br-, and I- soluble or insoluble in water? |
soluble, unless with silver, lead (II), or mercury (II)
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Are compounds containing SO4 soluble or insoluble in water?
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soluble, unless with calcium, strontium, barium, or lead(II)
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Are oxides soluble or insoluble in water?
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insoluble, unless with a group 1 metal or ammonium
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Are hydroxides soluble or insoluble in water? |
insoluble, unless with a group 1 metal, ammonium, calcium, strontium, or barium
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Are compounds of the ions carbonate, phosphate, and sulfide soluble or insoluble in water? |
insoluble, unless with group 1 metal or ammonium
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Why does H+ attach to a water molecule?
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charge density is too high by itself
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Is the solubility of solids affected by pressure?
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no
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When are gases more soluble?
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lower temperatures, higher pressures (Henry's Law)
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What is molality? |
number of moles of solute per kilogram of solvent
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What is the advantage of using molality? |
does not vary with temperature, volume changes (molarity) but mass does not (molality)
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What is the dilution equation? |
M1V1 = M2V2
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What exists for an insoluble ionic compound? |
equilibrium between the solid and the dissolved ions
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How is a solubility constant determined and what is its symbol? |
same way as Keq, ignoring solids Ksp |
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What does a small value of Ksp represent?
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less solubility
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What is the common ion effect? |
If ion is already present in solution, solubility will decrease and the reaction will shift away from that ion.
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How is the following situation dealt with: 9*10^-13 = x*(x+0.1)?
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Ignore x in (x+0.1), it is negligibly small.
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What is a complex ion?
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ion that contains a metal cation bonded to one or more small molecules
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What are ions or molecules surrounding the metal cation of a complex ion? |
ligands
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Are complex ions soluble in aqueous solutions? Why or why not?
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Yes, charged
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How many ligands typically surround the central metal of a complex ion?
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charge + 1
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What is indicated when the addition of a ligand causes an insoluble compound of a metal to redissolve? |
complex ion formation
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Are particles in a colloid attracted to or repelled by the molecules in the medium in which they are dispersed? |
either/or
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What are the three types of mixtures? |
solution colloid suspension |
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What type(s) of mixtures can be separated by filtration? |
suspensions
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What type(s) of mixtures show the Tyndall effect?
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colloids suspensions |
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What type(s) of mixtures are homogeneous?
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solutions colloids |
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What type(s) of mixtures separate via gravity?
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suspensions
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What type of mixture is salt water?
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solution
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What type of mixture is muddy water? |
suspension
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What often react with carbonates or bicarbonates to produce carbon dioxide gas? |
acids
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What do metals react with acids to form?
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hydrogen gas
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What is a Brønsted-Lowry acid?
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donates a hydrogen ion (or proton)
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What is a Brønsted-Lowry base? |
accepts a hydrogen ion
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What is an amphoteric substance?
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can act as an acid or a base
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How do conjugate acid-base pairs differ?
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by one hydrogen
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What are three examples of amphoteric species?
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water bicarbonate (HCO3 -) bisulfate (HSO4 -) |
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What does the Lewis theory of acids and bases describe all acid-base reactions in terms of? |
donating and accepting of electron pairs
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Why must an increase in hydronium ion concentration be accompanied by a decrease in hydroxide concentration? |
Kw is constant at a given temperature
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What is the equation for pH?
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pH = -log[H+]
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What is log x^n?
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n*log(x)
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What is log 10^x?
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x
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How does [H+] relate to pH without log?
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[H+] = 10^-pH
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What is the pH if [H+] is of the form 1*10^-x and why?
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x because log(1) = 0
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What is the pH if [H+] is 3*10^-7? |
between 6 and 7
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What is a strong acid/base?
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dissociates 100% in water
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What is any compound for which the number of oxygen atoms exceeds the number of hydrogen atoms by two or more?
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strong acid
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What are six strong acids?
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HI HCl HBr H2SO4 (sulfuric acid) HNO3 (nitric acid) HClO4 (perchloric acid) |
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What are six strong bases?
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LiOH NaOH KOH Mg(OH)2 Ca(OH)2 Ba(OH)2 |
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What is an example of a triprotic acid and is it strong or weak?
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H3PO4, weak
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What is an acid or base's normality and its symbol?
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molarity times number of hydrogen or hydroxide ions it can contribute to a reaction N |
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What is the mass of an acid or base that contributes 1 mole of either hydrogen or hydroxide ions?
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equivalent weight
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What do all weak acids and bases exist in?
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equilibrium between the ionized and non-ionized forms
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What are binary acids?
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non-oxygen containing
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What's the relationship between the conjugate base and acid strength?
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the more stable the anion formed, the stronger the acid
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Rank H-halogens by acid strength and explain why.
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HF < HCl < HBr < HI Increased electronegativity results in a stronger bond. |
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Rank H2-oxygen group elements by acid strength.
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H2O < H2S < H2Se < H2Te
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Rank Cl-oxoacids by acid strength and explain why.
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HClO < HClO2 < HClO3 < HClO4 Negative charge can spread across more oxygen atoms. |
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What is a salt?
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ionic compound formed from the reaction of an acid and a base
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What does a salt consist of?
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positive and negative ion
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Where does the positive ion in a salt come from?
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base
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Where does the negative ion in a salt come from? |
acid
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What is hydrolysis?
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reaction of a salt with water to form acids or bases
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When is a salt neutral?
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strong acid + strong base
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When is a salt acidic?
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weak base + strong acid
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When is a salt basic?
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weak acid + strong base
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What is the salt of a weak acid and weak base?
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acidic if Ka > Kb basic if Ka < Kb |
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Do ions of strong acids or bases react with water?
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No, they become spectator ions.
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Do ions of weak acids or bases react with water?
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yes
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What is a buffer?
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combination of a weak acid and a salt of that weak acid or a weak base and a salt of that weak base that resists a change in pH
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What happens when a base is added to the following buffer: HF <-> F- + H+?
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It reacts with H+ and shifts the reaction to the right, maintaining pH.
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What happens when HCl is added to the following buffer: HF <-> F- + H+?
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It introduces additional H+ and shifts the reaction to the left, maintaining pH.
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What is the Henderson-Hasselbalch equation and what is it used for?
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pH = pKa + log(base/acid) "buffer recipe" to create a solution with a desired pH |
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What is the equation for pKa?
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-log(Ka)
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When will the point of maximum buffering occur in reference to the Henderson-Hasselbalch equation?
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when the pH of a solution is approximately equal to the pKa
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How does adding water affect pH?
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It doesn't, acid and base ratios both decline at the same rate.
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What are neutralization reactions?
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acid + base -> salt + water
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What salt does ammonia form?
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ammonium salt
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What is the equivalence point on a titration curve?
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midpoint of the nearly vertical area where the number of moles of acid exactly equal the moles of base
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What is true at the half-equivalence point of a titration curve?
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pH = pKa and the solution has its maximum buffering ability, the concentration of the acid and its salt are equal
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What equation is used in titrations?
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Va*Na = Vb*Nb N= normalities |
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When is Va*Na = Vb*Nb used?
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When you don't explicitly know how many moles were used.
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Is equivalence point always at pH = 7?
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No, only when a strong base is added to a strong acid. When a strong base is added to a weak acid, pH > 7. When a weak base is added to a strong acid, pH < 7.
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What is an indicator usually?
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weak acid whose conjugate base is a different color
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How does the following litmus indicator work: HLit (red) <-> H+ + Lit- (blue)?
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When acid is added, the reaction shifts left and appears red. When base is added, it raises the pH, the concentration of hydroxide ion increases, and the concentration of H+ decreases, shifting the equilibrium to the right.
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What is the best indicator for an acid-base titration?
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one that undergoes a color change at the equivalence point
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How is a redox titration monitored?
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with either a potentiometer or a redox indicator
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What is a system in which electrodes are submerged in electrolytes, and in which a chemical reaction either results in or is a result of an electric current?
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electrochemical cell
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What are electrochemical cells that generate current?
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voltaic or galvanic cells
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What is an electrochemical cell in which the reaction is driven by the application of electrical current?
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electrolytic cell
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In an electrolytic cell, where does oxidation take place? Reduction?
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anode cathode |
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negatively charged electrode
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cathode
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positive electrode
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anode
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What is the charge on one mole of electrons known as?
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1 Faraday
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How many coulombs of charge is 1 Faraday?
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96,500
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How does electric charge relate to current? Describe using units as well.
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Electric charge = electric current * time current flows Coulombs = Amperes * seconds |
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What does a voltaic or galvanic cell consist of?
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two half-cells electrically connected to each other, each is an oxidation or reduction reaction
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What convert electrical energy into chemical energy?
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electrolytic cells
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What is an example of how a half-cell can be made?
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placing a zinc strip in a zinc+ion solution
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Why are two half-cells connected through a salt bridge in a galvanic cell?
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to allow an electric current to flow between the two electrodes without the solutions mixing
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What does a salt bridge consist of?
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a gel with an ionic compound dissolved in it
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Why does a flow of electrons (current) result in a voltaic or galvanic cell?
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one metal has a greater tendency to lose electrons than the other
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Where do electrons flow from in a galvanic cell?
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anode to cathode
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Does the mass of the cathode increase or decrease? Why?
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increase, metal is formed
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Does the mass of the anode increase or decrease? Why?
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decrease, ions exit
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What is the shorthand notation for a galvanic cell?
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anode (s)|anode ion (aq)||cathode ion (aq)|cathode (s) |
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How do electrons move according to electric potential?
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from a higher electric potential to a lower electric potential
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What is potential difference measured in?
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Volts
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What is the equation for electrical work?
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charge*potential difference
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What is the equation for the maximum work that an electrical cell can do?
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W = -nFE W = ΔG n = number of moles of electrons F = Faraday constant E = cell potential/voltage |
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What is a measure of the chemical force of an electrochemical cell's (redox) reaction?
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electromotive force (emf)
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What measures the tendency of an oxidized species to gain electrons and become reduced?
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reduction potential
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What is the equation for Ecell (emf)?
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E(cathode) - E(anode)
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If a half-reaction must be doubled to be balanced, what happens to its voltage?
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no change, don't double
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What is a property that is independent of the amount of material?
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intensive property
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Does cell voltage or emf depended on the amount of material in the cell?
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no
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What is hydrogen's reduction potential at standard conditions?
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0
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Will the more negative reduction potential be at the cathode or the anode?
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anode
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How does cell voltage relate to spontaneity?
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positive = spontaneous negative = nonspontaneous |
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What kind of cell has a positive voltage? Negative?
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galvanic electrolytic |
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What allows the cell emf to be calculated when concentrations are not standard?
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Nernst equation
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