Draw the expected product for each of the following reaction: 1) MeMgBr (excess) 2) H₂O NaOH H₂O ? H₂O* H₂O (excess) Chemical Formula: C5H₁₁NO ABCD 0000 1) LiAlH4 (excess) 2) H₂O H₂O+ CH₂OH (excess) Et₂N (base) SOCI₂ EtOH Py (base) A B с D NH OH NH2 OH Et₂CuLi MCPBA NH NH2

Predict two products for the following reaction.

What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. HC1O4+ H2O — NH/ + H2O -» HCOr + OH" —

HCl (excess) H₂O₂

Q4

Ph NaOH / H2O Compound C

NaHCO3 can deprotonate benzoic acid but cannot deprotonate phenol. On the other hand, NaOH can deprotonate both benzoic acid and phenol. Given this information, rank the molecules numbered I to V in order of decreasing acidity. COH cOH он H,0 H,CO, IV CH3 II I II (A) V > II >I > III > IV (В) II > 1 > V > III IV (C) II > V >I > IV > II

Explain why using one or two equivalents of NaH results in differentproducts in the following reactions.

Draw a full arrow pushing mechanism for the following three reactions: 2 Acidic Conditions OH Acidic Conditions H 2 H 2 Acidic Conditions

The amount of tartaric acid is responsible for the tartness of wine and controls the acidity of the wine.  Tartaric acid also plays a very significant role in the overall taste, feel and color of a wine.   Tartaric acid is a diprotic organic acid The chemical formula for tartaric acid is C4H6O6 and its structural formula is HO2CCH(OH)CH(OH)CO2H.   A 50.00 mL sample of a white dinner wine required 21.48 mL of 0.03776 M NaOH to achieve a faint pink color.  Express the acidity of the wine in terms of grams of tartaric acid, H2C4H4O6 (M. M.  =  150.10) per 100 mL of wine.  Assume that the two acidic hydrogens are titrated at the end point. MM H2C4H4O6 = 150.10 MM NaOH = 40.00 Below is the balanced chemical equation for this titration.