According to The Aldol Addition and Condensation: The Effect of Conditions on Reaction Pathways for 3-Hydroxy-3-(4-nitrophenyl)-1-(2-pyridyl)-1-propanone, Answer this Q/

Q: 112 microliters of 2-acetylpyridine (121.14 g/mol, 1.08 g/mL) was reacted with 145 mg of 4-nitrobenzaldehyde (151.12 g/mol) and 35 mg of sodium carbonate (105.99 g/mol). What is the theoretical yield, in milligrams (mg), of the aldol addition product (254.25 g/mol)? Enter your answer as digits only (no units), using the proper number of significant figures.

1. The densities of crystalline Cl2 and H2S at 160 K are 2.02 and 0.95 g/cm3, respectively. Calculate their molar volumes.

2. The fluorocarbon compound C2Cl3F3 has a normal boiling point of 47.6 ∘C. The specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J/g⋅K and 0.67 J/g⋅K, respectively. The heat of vaporization for the compound is 27.49 kJ/mol.

Calculate the heat required to convert 73.0 g of C2Cl3F3 from a liquid at 13.90 ∘C to a gas at 99.80 ∘C.

Express your answer using two significant figures.

Calculate the enthalpy chamge when 75.0g of ethanol goes from 87.0 C to -15.0 C, given the following information for ethanol: c ethanol = 2.44j/g*C, Delta Hfusion=5.02 kj/mol, delta Hvap=38.56 kj/mol.

For a particular redox reaction NO is oxidized to NO3– and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in basic solution. Phases are optional.

NO + Cu²⁺ ----> NO₃^- + Cu⁺

I know how to do it for an acidic solution, please show work for a basic solution. Thanks.

What are the units for molarity? Rearrange the molarity equation to solve for volume

question 1

The Friedel-Crafts reaction to form BHA forms both isomers equally while the BHT

synthesis only forms on regioisomer (where the t-Bu are ortho to the alcohol). Why is the

selectivity for one regioisomer so much higher in the reaction to form BHT?

explain ir data for 7-Methoxy-1H-indol-6-yl propiolate

IR
(KBr): 3392 (NH), 3259 (C≡CH), 2941, 2810, 2123 (C≡C),
1732 (C═O), (1600, 1500, 1338, 1242, 1200, 1057, 750 cm1)==== specialy

Calculate the concentrations of all species contained in 0.15 M solution of carbonic acid at 25 degrees celsius. ka1= 4.2 x10^-7, ka2= 4.8 x 10^-11 .

The number of different bond angles for PBr2F3 with Br’s axial and equatorial is?

9) A 12.39 kg sample of phosphorus reacts with 52.54 kg of chlorine to form only phosphorus trichloride (PCl3).

a) If it is the only product, what mass of PCl3 is formed?

b) Assuming ideal behavior, calculate the stoichiometric volume of chlorine gas needed at 1.1 atm and 25 °C. 4

c) Calculate the stoichiometric mass of chlorine required.

d) In a similar process, the chlorine is introduced to the reactor in the form of a carbon tetrachloride solution. What volume of a 4.5 M solution is required to deliver for the stoichiometric amount of chlorine?

What is the pH and the equilibrium concentration of PO₄^3- in a 0.511 M solution of H₃PO₄(aq)? Ka1=7.5*10^-3, Ka2=6.2*10^-8, Ka3=4.8*10^-13

0.5 L of a buffer solution contains 0.44 M acetic acid and 0.44 M NaCH3COO, and has a pH of 4.74. What will the pH be if 0.20 mol of HCL is added to the solution?

Learning Goal:

To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects of acid or base addition on pH.

A buffer is a mixture of a conjugate acid-base pair. In other words, it is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an acetic acid buffer consists of acetic acid, CH₃COOH, and its conjugate base, the acetate ion CH₃COO^-. Because ions cannot simply be added to a solution, the conjugate base is added in a salt form (e.g., sodium acetate NaCH₃COO).

Buffers work because the conjugate acid-base pair work together to neutralize the addition of H⁺ or OH^- ions. Thus, for example, if H⁺ ions are added to the acetate buffer described above, they will be largely removed from solution by the reaction of H⁺ with the conjugate base:

H⁺+CH₃COO^--->CH₃COOH

Similarly, any added OH? ions will be neutralized by a reaction with the conjugate acid:

OH^-+CH₃COOH --> CH₃COO^-+H₂O

This buffer system is described by the Henderson-Hasselbalch equation

pH=pKa+log[conjugate base]/[conjugate acid]   

A beaker with 125mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 5.00mL of a 0.380M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.760.

Express your answer numerically to two decimal places. Use a minus (-) sign if the pH has decreased.

A buffer solution is prepared by dissolving 1.50 g each of sodium benzoate, C6H5COONa, and benzoic acid, C6H5COOH (Ka = 6.45 × 10-5), in 150.0 mL of solution. The molar mass of benzoic acid is 122.12 g/mol and that of sodium benzoate is 144.10 g/mol.

a) What is the pH of this buffer solution?

b) Which buffer component must be added to change the pH to 4.00? What mass of that component is required?

c) What volume of 2.0 M NaOH or 2.0 M HCl must be added to the original buffer in part a to change the pH to 4.00?

The vapor pressure of solid benzene is 299 Pa at -30ºC and 3270 Pa at 0ºC. The vapor pressure of liquid benzene is 6170 Pa at 10ºC, and 15,800 Pa at 30ºC. (a) Calculate the triple point of benzene (temperature and pressure at which solid, liquid, and vapor all coexist). This is obtained by using the Clausius-Clapeyron equation first to determine ∆vapH for the solid and the liquid, and then to give equations for the curves defining the solid-vapor equilibrium and the liquidvapor equilibrium, and solving both the latter equations simultaneously. (b) Calculate the enthalpy of fusion at the triple point, ∆fusH = Hliq – Hsol.