Chemistry S-20 Week 1 Alkenes: Isomers and Nomenclature 1. There are 6 unique alkene isomers of the hydrocarbon C5H10. Draw each of these isomers‚ and provide a systematic name for each. 1-pentene (E)-2-pentene (Z)-2-pentene 2-methyl-1-butene 2-methyl-2-butene 3-methyl-1-butene 2. For the three alkenes above which are various isomers of pentene‚ rank them in order of stability. Explain your ranking. most stable (more subst. double bond) less stable (cis alkene is
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BaSO4 ‚ CaSO4 Carbonate All carbonate salt not dissolve in water except; Li2CO3 Na2CO3 ‚ K2CO3 ‚ (NH4)2CO3 Oxide All oxide not dissolve in water except; Na2O ‚ K2O ‚ CaO Hydroxide All hydroxide not dissolve in water except; NaOH‚ KOH‚ Ca(OH)2 ‚ Ba(OH)2 Formula to determine the heat change; Heat released/absorbed‚ H = mcӨ [unit = J or kJ] Symbol Description Unit m mass of solution 1cm3 = 1 g c specific heat capacity of solution 4.2 J g-1 oC-1 Ө temperature change oC
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3. Solubility Products (Ksp) BaSO4 1.5 ´ 10-9 CoS 5.0 ´ 10-22 PbSO4 1.3 ´ 10-8 AgBr 5.0 ´ 10-13 Which of the following compounds is the most soluble (in miles/liter)? A) BaSO4 B) CoS C) PbSO4 D) AgBr E) BaCO3 4. How many moles of Fe(OH)2 [Ksp = 1.8 10-15] will dissolve in 1.0 liter of water buffered at pH = 11.52? A) 1.6e–10 B) 3.3e–3 C) 1.1e–5 D) 6.1e9 E) 5.4e–13 5. You have two salts‚ AgX and AgY‚ with very similar Ksp values. You know that Ka for HX is much greater than
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powder reacts with potassium hydroxide to generate Al(OH)4- ions and release hydrogen. 2 Al(s) + 2 KOH(aq) + 6 H2O 2 K[Al(OH)4](aq) + 3 H2 (g) A gelatinous precipitate of aluminum hydroxide was created when sulfuric acid was added to the aqueous solution of Al(OH)4- ions. 2 K[Al(OH)4](aq) + H2SO4 (aq) 2 Al(OH)3 (s) + K2SO4 (aq) + 2 H2O Later‚ excessive addition of the acid causes the precipitate to dissolve in the solution. 2Al(OH)3 (s) + H2SO4 (aq) Al2(SO4)3 (aq) + 6 H2O Precipitation
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This might come off strong‚ I know I met you not long ago-oh-oh. (Mhmmm.) When I heard you sing‚ I thought you were the cutest thing‚ that I’d ever seen‚ that I’d ever seen-en-en-en. In a verse or two‚ you caught me staring over at you. & I thought of somethin’ funny to say‚ but I didn’t want to sound cliché-ay (Oh oh whoa oh oh.) & this is how I plan to break the ice-ce: Say something nice. But I had to go before I could‚ sittin’ here thinkin’ if I really should. But I’ll have some fun-un‚ take
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HPO4-2 + H2O ( PO4-3 + H3O+ Ka3 = [H3O+] [PO4-3] = 4.5e-13 [HPO4-2] Ka1> Ka2> Ka3 13B—Describing Polyfunctional Bases CO3-2 + H2O ( HCO3- + OH- Kb1 = [HCO3-] [OH-] = Kw = 2.13e-4 [CO3-2] Ka2 HCO3- + H2O ( H2CO3 + OH- Kb2 = [H2CO3] [OH-] = Kw = 6.7e-4 [HCO3-] Ka2 13C—Finding the pH of Solutions of Amphiprotic Salts -Amphiprotic salts are formed during neutralization titration of polyfunctional
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(also written [H3O+]‚ the equal concentration of hydronium ions)‚ measured in moles per litre (also known as molarity). Basic (Alkaline) substances have‚ instead of Hydrogen ions‚ a concentration of Hydroxide ions (OH-). So‚ similarly the formula for calculating pOH is : pOH = - log [OH-] The pH scale is logarithmic and as a result‚ each whole pH value below 7 is ten times more acidic than the next higher value. For example‚ pH 4 is ten times more acidic than pH 5 and 100 (10 times 10) more acidic
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Buffer solutions and common ion effect A buffer solution resists (or buffers) a change in its pH. That is‚ we can add a small amount of an acid or base to a buffer solution and the pH will change very little. How to calculate pH of buffer solution containing both acid and conjugate base? Dissociation constant definition 1.1 can be rearranged into or (note that due to sign change [A-] was moved to nominator). This is so called Henderson-Hasselbalch equation (or buffer equation)
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where they will live their lives in the freedom they desire. [Sea Wave Sound] - Oh my head! (bumps his head on the top of his crate) What the-- I’m in a box! Oh no! Not the box! Oh no‚ they can’t transfer ME! NOT ME! I can’t breathe‚ can’t breathe! Darkness creeping in. I can’t breathe. Walls closing in around me! So alone. So alone--- - Alex! Alex are you there? - Marty? - Yeah! Talk to me‚ buddy. - Oh‚ Marty! You’re here! - What’s going on? You OK? - This doesn’t look good. - Alex
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ion‚ by hydroxide‚ H2O2. The following reaction takes place: H2O + HO2- +2Fe2+ 2Fe3+ + 3OH- The OH- ion concentration of the solution is high enough so that some of the Fe3+ reacts with OH- to form ferric hydroxide(brown precipitate) as follows: Fe3+ + 3OH- Fe(OH)3 With the addition of more H2C2O4‚ the Fe(OH)3 dissolves and the soluble complex K3[fe(c2o4)3].3h20 is formed according to : 3k2C2O4 + 2Fe(OH)3 + 3H2C2O4 2K3[Fe(c2o4)3].3H20 + 3h2o Ethanol is added to the solution to cause the complex iron
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