test 2 for chem

what is the forward reaction?

HF (+) H2O--> F- (+) H3O-

to name aromatic

# from lowest number attached to the geometric (circle w/circle in middle) only to get the first name--> add either bromine, toluene,aniline,phenol in ending. NO SPACES ex.)3-ethylphenol; 4-ethyltoluene; 4-bromoaniline

what is a Mass percent

*(% m/m)* -concentration by mass of solute in a solution -mass of solute in grams for exactly 100g of solutions -mass of solute and solution MUST be the SAME

what is Mass/ volume percent?

*(% m/v)* -percent *mass (g)* of solute to *volume (mL)* of solution

what is Volume Percent

*(% v/v)* percent volume (mL) of solute (liquid) to volume *(mL)* - *units* must *all be the same* throughout the problem -assume that there is 100 mL of every solution unless otherwise noted.

what is the Equation for Mass percent?

*(m/m)= g of solute/ (g of solute + g of solvent)--> x100%* -*if given mass %= g solute/ 100g solution* refer back to notes for the actual details of equation and book for more details, Pg. 296 chpter 9

what is the Equation for Mass/Volume Percent?

*(m/v)% = g solute/ mL solution --> x100%* or *(m/v)% =g solute/100 m/L solute--> x100%*

What is Molarity?

*(molarity of solute/liter of solution)*

what is the equation for volume percent?

*(v/v)%= mL solute/ (mL solute +mL solvent)--> 100%* *solute+ solvent= solution* a.) first solve the solution b.) plug the numbers into the equation to get the final answer (v/v)% = mL solute/ 100mL solution

what is the equation for Solute Concentration?

*C1V1=C2V2* *C*= *concentration* *V*= *volume*

what happends in a *solution with ionic solute*? ex.) NaCl

*Ionic solutions will BOND w/ OPPOSITE ATTRACTIONS; undergo HYDRATION to form solution* if NaCl crystal placed in water 1.) partially *negative oxygen* atom in water molecule -->*attract Positive Na+ ions* 2.)Partially *positive hydrogen atom* in *other water molecule*--> attract *negative Cl- ions* 3.)when *form Solution* -undergo *hydration* *(water molecule surround Each ion & Pull it into Solution)* *Equation:* NaCl(s)--> Na(+)(aq) + Cl (-)(aq) [top of arrow is the *formula H2O: indicating water needed for dissociation process but NOT REACTANT *]

What is the equation for *dissociation of water?

*Kw= [H3O+][HO-]* *Kw=1 .0X10(-14 exponent)* @25degrees rearranged: Kw/ [H3O+]= [HO-] Kw/[HO-]= [H3O+]

what is the equation of Molarity?

*M= mol/L* steps: 1.)*find* the *molar mass* of the given elements a.)*find atomic mass* of *each element* in the compound b.)*add/ multiply* to *get the TOTAL Molar mass (g of the given compounds)* 2.)Set equation: a.)put the *given (g first) w/ the given comound* b.)*multiply* by *either 1mol of the given compound or by 1 gram of the given over the molar mass of the given compound*. 3.) Find the M a.) M= take answer from the mol of the #2 -mol b.) divide by the given liters= final answer EQUATION: given equation w/the given compound X 1mol with the given equation /molar mass (g) given compound= answer in mol M=answer from mol/ given from problem of liter=answer in M

*naming ether*

*O in middle of skeleton*

chapter 12: functional groups Alcohol Phenol Thiol Ether

*OH=>hydroxyl group benzene w/ OH (CH3) SH group c-o-c*

what is the formula for *calculating the [H3O+]* for solution

*[H3O+]=10(-PH)* to write it: *[H3O+]=1X10(-pH)*

alkene: cis/trans

*cis: hydrogen are next to each other* *trans: hydrogen are opposite from one another in a double bond*

alkyne

*count where tripple bond is* *name: ending "yne" *alphabetical order*

*hydration* for alkene

*double bond breaks into SINGLE bond* *where double bond was attached, one carbon GETS OH to fewest (C-OH), the other carbon gets an H to mostest C (C-H)* on *top of arrow* SO4,HCL,H2*

*hydrogenation* for alkene

*double bond from the carbon-broken.* *becomes single bond, add H where the double bond used to be* *needs pt, nd,NI to break. written on top of arrow*

what is Solubility?

-*MAX amount* of solute that can dissolve in a specific amount of solvent at given temp equation: g solute/ 100g H2O

what is Saturated solutions?

-*Max* amount of solute is in solution -May *see undisolved solute in Container - Solute + Solvent (equilibrium sign) saturated solution

what happens in NH3 in a Bronsted-Lowry Base in the reaction of ammonia and water?

-*NH3* base that *accept H+* -*H2O* base that *DONATE H+* ex.) NH3+H2O--> NH4+ (+) HO-

chpter12: *Naming thiol*

-*SH* -start counting where the SH located. -in the end of naming the main skeleton; number name-add thiol

what is a typical organic compound?

-*covalent bond* -*low* melting point/ boiling point -*flammable* -*soluble* in *non polar solvent* -*NOT soluble in H2O* -C3H8--> propane

How does temperature affect on solubility?

-*depend* on *temp* -Most *solid* are *More soluble* at *higher temp* -*Gases* *LESS* soluble at higher temp

what are Strong electrolytes?

-*dissociate 100% in water* a.)fully *breaks into ions* Na2SO4---> 2Na+ (+) SO4 {charge of 2-; polyatomic} -forms solutions that conduct strong *electric current* -addition info for ionic compounds: NaCl, KBr, MgCl2, NaNo3; bases like: NaOH, KOH acids like: HCl, HBr, HI, HNO3, HClO4, H2SO4

what are Nonelectrolytes?

-*dissolve as molecules* in H2O -Do *NOT* *break* into *ions* = no conduction of electricity in H2O -addition info: carbon compound like: CHOH(methanol), C2H5OH(ethanol), C12H22O11(sucrose), CH4N2O(urea)

based on Le Chatelier's Principle; given the *equilibrium reaction*, *adding more* of a *substance*, what will happen

-*increase* in reaction rate (change) a.)shift in direction of products

where do *strong bases* form from?

-*metals in group 1 and 2* HU- = strong base

what are alkanes? where do you start counting?

-*organic* molecule -*single bond* -name *ends with "-ane* when counting: # by *longest chain*

what is Arrhenius bases?

-*produce HO-* in H2O -dissociate from metal -*Bitter/Chalky* taste -electrolytes -*soapy/Slippery* feeling -neutralize acid *has OH-*

how many bonds can a carbon with more than 1 can have ?

-4 single bonds -tetrahedral shape

what is dilution?

-H2O added -volume increases -concentration can decrease -*MASS of solute* *remain SAME*

what is the definition for Solute

-Homogenous mixture of 2 or More substances -form when there are *Sufficient attraction between Solute & Solvent * -object being dissolved

what is the definition for Solution

-Liquids, gases, solid -spread evenly through the solution -solute mix with solvent= *Same physical state* -Cannot filter out; Unless Solvent is evaporated -*Cannot see Solute in solution* -*might* see color changes

what are buffers?

-buffer solutions help maintain a pH -absorb any addition acid or base -blood pH=7.4

what is Unsaturated?

-contain *LESS* than maximum amount of solute -*More solute* can *dissolve*

what are *weak acid*?

-dissociate slightly -few ions -strong conjugate base

In a *weak acid what does weak acid do in water*?

-dissociate slightly to form *few ions* in aqueous solutions -*poor acceptor of hydrogen -will have a double arrow

what are *weak* *bases*?

-few ions in solution -ex.) NH3

what is organic compound?

-high melting point/boiling point -soluble in H2O

what happen when you add acid to pure water?

-increase [H3O+] -cause [H3O+] exceed 1.0X10(-7) M -decreases [OH-] -solution acidic

what is an organic compound?

-made from carbon -1 or more carbon -lots of hydrogen -could have o,s,n, halogens

what happend when equilibrium is reached?

-no changes in concentration of reactant and product - rate of forward reaction=to rate reverse reaction -Product and reactant concentration NOT have to be SAME equilibirum

what is Arrhenius acid?

-produce H+ (proton) ions in H2O HCl---->(top of arrow is H2O) H+ (+) Cl- -electrolytes -*Sour taste* -blue litmus paper *turn red* -*neutralizer base* *has H*

What is Henry's law states?

-solubility of gas in liquid is directly related to the pressure of gas above the liquid -HIGHER pressure= gas MORE soluble in Liquid -LESS pressure= LESS soluble

what is *water* in terms in solute or solvent?

-universal *solvent* (most common in nature) -*polar molecule* -can form H-bonds -strongest bond is H2O

what is happening in an equilibrium reaction?

2 reaction taking place -one forward direction -one reverse direction

how to Name Acid?

1.) Acids w/ *H* & *nonmetal* -*prefix hydro* -*end* with *ic acid* ex.) HCl--> Hydrochloric acid 2.)Acid with *H* and *polyatomic ion* - *"ate"*---> *ic acid* ex.) ClO3- (chlorate)-->HClO3 =chloric acid -polyatomic end w/ *"ite"*--> *ous acid* ex.)ClO2- (chlorite)---> HClO2 =Chlorous acid

how to name Bases?

1.) base with *OH- ions* -*hydroxide ending* of formula name -in *metal periodic table* ex.) NaOH--> sodium hydroxide KOH--> potassium hydroxide Ba(OH2)--> barium hydroxide Al(OH)3--> aluminum hydroxide Fe(OH)3--> iron(III) hydroxide

to write benzene

1.) name what ever is group of extra carbon attached no spaces; write benzene as ending

what does the pH solution indicate? -what are its values?

1.)acidity 2.) 1-->14 3.)below 7.0 acidic 4.)7.0 neutral 5.)7.0 basic

what does *strong acid* do in aqueous solutions*? -what its opposite conjugate? 2.)what are the strong acid formulas?

1.)completely ionizes 100% -will have one arrow only 2.) weak conjugate base 2a.)HCl=hydrochloric acid H2SO4=sulfuric acid HNO3=nitric acid HBr=hydrobromic acid HI=Hyrdroiodic acid

Sample Problem #1: Sea water contains roughly 28.0 g of NaCl per liter. What is the molarity of sodium chloride in sea water?

1.00 L) = 28.0 g / 58.443 g mol¯1 x = 0.4790993 M to three significant figures, 0.479 M

Sample problems: KF is a strong electrolyte and HF is a weak electrolyte. How is the solution of KF different from that of HF?

9.7 answers: KF solutions will dissociate in water to produce ionizations to conduct electricity vs. HF being a weak electrolyte which will separate into molecules; will dissociate slightly in water [in solution of KF, only ions of K+ and F- are present in the solvent. In an HF solution, only a few ions of H+ and F- present but mostly dissolved HF molecules]

Sample problem: write a balance equation for the dissociation of each of the following strong electrolytes in water: a.)KCl b.)CaCl2 c.)K3PO4 d.)Fe(NO3)3

9.9 answers: a.) ---> (H20 on top of arrow) K+(aq) (+) Cl-(aq) b.)--> (H2O top of arrow) Ca2+(aq) (+) 2Cl-(aq) c.)--->(H2O top of arrow) 3K+(aq) (+) PO4[3- charge](aq) d.)---> (H2O top of arrow) Fe3+-(aq) (+) 3NO3[-charge](aq)

What happens in solution with Polar Solutes?

Are *Polar molecules* (covalent molecule) 1.) Polar Solute *require Polar solvent* for *solution to Form* EX: CH3OH methanol 1.) CH3---OH (soluble in water b/c *methanol has POLAR --OH group to form with hydrogen bond with water)*

what is the reverse reaction?

F- (+) H3O+ --> -HF (+) H2O

Sample Problem: Describe the formation of an aqueous KI solution, when solid KI dissolves in water

K has a Positive charge, while I has a negative charge; therefore the charges will attract, will undergo hydration to form solution

In terms of sizes; what is Solvent

Larger amount

sample problem: Problem #1: If you dilute 175 mL of a 1.6 M solution of LiCl to 1.0 L, determine the new concentration of the solution.

M1V1 = M2V2 (1.6 mol/L) (175 mL) = (x) (1000 mL) x = 0.28 M Note that 1000 mL was used rather than 1.0 L. Remember to keep the volume units consistent.

Problem #2: You need to make 10.0 L of 1.2 M KNO3. What molarity would the potassium nitrate solution need to be if you were to use only 2.5 L of it?

M1V1 = M2V2 (x) (2.5 L) = (1.2 mol/L) (10.0 L) x = 4.8 M Please note how I use the molarity unit, mol/L, in the calculation rather than the molarity symbol, M.

In terms of sizes; What is Solute

Smaller amount

Sample problem: Write the dissociation equations for the following that emphasize their behavior as Arrhenius acids: a) HI b) HBrO c) HCN d) HClO2

Solution a) HI(aq) H+(aq) + I-(aq) b) HBrO(aq) H+(aq) + BrO-(aq) +- +- c) HCN(aq) H (aq) + CN (aq) d) HClO2(aq) H (aq) + ClO2 (aq)

Problem #6: To 2.00 L of 0.445 M HCl, you add 3.88 L of a second HCl solution of an unknown concentration. The resulting solution is 0.974 M. Assuming the volumes are additive, calculate the molarity

Solution 1: M1V1 + M2V2 = M3V3 (0.445) (2.00) + (x) (3.88) = (0.974) (2.00 + 3.88) x = 0.125 M Calculate moles HCl in 0.445 M solution: (0.445 mol/L) (2.00 L) = 0.890 moles 2) Set up expression for moles of HCl in second solution: (x) (3.88 L) = moles HCl in unknown solution 3) Calculate moles of HCl in final solution: (0.974 mol/L) (5.88 L) = 5.73 moles 4) Moles of HCl in two mixed solutions = moles of HCl in final solution: 0.890 moles + [(x) (3.88 L)] = 5.73 moles x = 1.25 M (to three sig figs)

special groups of benzene

Toluene-CH3 Aniline-NH2 Phenol-OH

Sample problem: identify the Solute and Solvent in the each solution composed of the following: a.) 10.0 g of NaCl and 100.0 g of H2O b.) 50.0 mL of ethanol, C2H5OH and 10 mL of H20 c.)0.20 L of O2 and 0.80 L of N2

a.)10.0 g of NaCl=> solute 100.0 g of H2O=> Solvent b.)50.0 mL of ethanol=> solvent 100.0 g of H2O=>solute c.)0.20 L of O2=>solute 0.80 L of N2=>solvent

Sample problem: identify the Solute and Solvent in each solution composed of the following: a.) 10.0 mL of acetic acid and 200 mL of water b.)100.0 mL of water amd 5.0 g of sugar c.)1.0 g of Br2 and 50.0 mL of methylene chloride

a.)10.0 mL of acetic acid=> solute 200 mL of water=> solvent b.)100.0 mL of water=> solvent 5.0 g of sugar => solute c. 1.0 g of Br2=>solute 50.0 mL of methylene chloride=> solvent

sample problem: 9.33 pg. 301 calculate the mass percent (m/m) for the solute in each of the following: a.)25g of KCl and 125g of H2O b.)12g of sucrose in 225g of tea solution c.)8.0g of CaCl2 in 80.0g of CaCl2 solution

a.)17%KCl solution b.)5.3%sucrose solution c.)10.0% CaCl2 solution

Sample problem: water is solvent and carbon tetrachloride (CCl4) is a nonpolar solvent. In which solvent is each of the following more likely to be soluble? a.) NaNO3, ionic b.) sucrose (table sugar), polar c.)gasoline, nonpolar d.)gasoline, nonpolar

a.)water b.)CCl4 c.)water d.CCl4

what is the Bronsted- Lowry Acids and Bases

acid *Donate H+* *Bases ACCEPT* H+

what is the Concentration of a solution expressed as?

amount/amount of solution -Units: a.)mass %= (m/m) mass/ volume % (m/v) b.)volume %= (v/v) molarity (mol of solute/ L of solution)

what can water act as based on ionization of water?

amphoteric: act as a base or acid

sample problem: pg.335 10.23 use Le Chatelier's principle to predict whether each of the following changes causes the system to shift in the direction of products or reactants: HCHO2(aq) (+) H2O(l) --><--- CHO2-(aq) (+) H3O+(aq) a.)adding some CHO2-(aq) b.)removing some HCHO2(aq) c.)removing some H3O+(aq) d.)adding some HCHO2(aq)

answer: a.

sample problem: 10.13 pg.328 identify thr Bronsted-Lowry acid-base pairs in each of the following basses: a.) H2CO3(+) H2O--><-- HCO3- (+) H3O+ b.)NH4+ (+) H2O --><--H2O--><-- NH3 (+) H3O+ c.)HCN (+) NO2---><---CN- (+) HNO2

answer: a. conjugate acid -base pair are H2CO3/HCO3- and H3O+/H2O b.conjugate acid-base pair NH4+/NH3 and H3O+/H2O c.conjugate acid-base pair are HCN/CN- and HNO2/NO2-

sample problem: 10.9 pg.328 write the formula for the conjugate base for each of the following acids: a.)HF b.)H2O c.)H2CO3 d.)HSO4-

answer: a.F- b.OH- c.HCO3 d.SO4(2-)

sample problem: 10.11 pg.328 write the formula for the conjugate acid for each of the following bases: a.)CO3(2-) b.)H2O c.)H2PO4- d.)Br-

answer: a.HCO3- b.H3O+ c.H3PO4 d.HBr

sample problem:10.4 a.) Al (OH)3 b.) HBr c.) H2SO4 d.)KOH e.)HNO2 f.)HClO2

answers:

Sample problem: 10.3 pg. 328 Name each of the following acids: 1.) Hbr 2.) H2CO3 3.)HC2H3O2

answers: 1.) hydrobromic acid 2.) carbonic acid 3.)acetic acid

sample problem: 10.3 pg.328 Name each of the following acids or bases: a.)HCl b.)Ca(OH)2 c.)H2CO3 d.)HNO3 e.)H2SO3 f.)HBrO2

answers: a.)hydrochloric acid b.)calcium hydroxide d.)nitric acid c.)carbonic acid d.)nitric acid e.)sulfurous acid f.)bromous acid

aromatics

are *Benzene*

what do Buffers contain?

combination of acid-base conjugate pairs -acetic acid & sodium acetate -or weak base & conj.acid ex.)-weak acid and its "salt"--> conj.base HC2H3O2=acid NaC2H3O2=conj.base

what happens with *solutions with nonpolar solutes*

compounds that have non-polar molecules like iodine (I2), oil, grease, do not dissolve in water because of *no attractions between particles of non-polar solute and polar solvent.

based on Le Chatelier's Principle, given the equilibrium, *removing a substance* what will happen? -what happens when you add a product/ remove a product more explanation on table pg334

decrease reactant a.)shift direction of reactants -*add a product*-->*increase* reverse reaction rate=>*shift* direction in *reactant* -*remove product*-->*decrease* reverse reaction rate=> *shift* direction in *product*

what are Weak electrolytes

dissociate *slightly in H2O* in solution -*few ions* -*mostly full molecules* -ex. of an *aqueous solution of *weak*electrolyte HF HF--> H+ (+) F- -addition info of weak electrolytes: HF, H2O, NH3, HC2H3O2(acetic acid)

alkane

ends with "ane" -number by the lowest with extra carbon *alphabetize*

alkene

ends with *"ene* *double bond* numbering: start *counting where closest to double bond* *alphabetize* *has Cis/Trans* if *has cis; to name:* 1.) put either cis or trans first 2.)number that the double bond located 3.)the total number of carbons

sample problem: 9.39 pg. 301 a mouthwash contains 22.5% (v/v) alcohol. If the the bottle of mouthwash contains 355mL, what is the volume, in milliliters, of alcohol?

given: 22.5%; 355mL equation to use: (% v/v)= mL solute/100mL 22.5%=355/100 final answer= 79.9 m/l

Calculate the molarity of 25.0 grams of KBr dissolved in 750.0 mL.

http://www.chemteam.info/Solutions/Molarity-example5-answer.GIF

Sample Problem: NaOH is a strong electrolyte and CH3OH is a nonelectrolyte. How is the solution NaOH different from that of CH3OH?

in solution of NaOH, only ions of Na+ and OH- are present in the solvent. In solution of CH3OH will dissolve as molecules in H20

what happens when you add base to pure water?

increase OH- causing 1.0X0(-7) to exceed decrease the [H3O+] -solution basic

Number base on its prefixes: 1,2,3,4,5,6,7,8,9,10

meth=1 eht=2 prop=3 but=4 pent=5 hexane=6 hexxane=7 octane=nonane dec=10

what is the function of a weak acid in buffer?

neutralize base - acetate ion produced in the neutralization reaction add to concentration of

what is the equation for finding pH?

pH=-log[H3O+] if the Ph value is given and ask for the log #--> answer will be 1.0X10(- whatever the given #)

in terms of " like solutions dissolving with what", -polar dissolving with what? -nonpolar dissolving with what?

polar dissolves with polar solutions nonpolar dissolves with nonpolar solutions *just determine base on polar or nonpolar*

what happens when stress is put upon an equilibrium?

reaction will CHANGE to relieve stress (reestablish equilibrium)

name an alcohol:

start counting where the OH group is. *drop* "e" *add* *ol*

what is Le Chatelier's Principle?

when *alter concentration* of *reactant or product of system at equilibrium*-->rate of *forward & reverse reaction NOT equal* -stress placed on equilibrium

combustion

x+CO2+H20 balance the equation