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Please explain which of the following aqueous solutions has the strongest ion-dipole attractions: 0.3 M Na3PO4 .1 M NiF2 .2 M Rb2CO3 0.01 M Sr(OH)2 and .03 M ScBr3.
Don't worry about the concentrations of reagents or the colors resulting precipitates (if any). You don't have to precipitate all ions, just separate them
If the pH probe was miscalibrated and reports the pH and reports the pH to be 1 unit higher than the true pH of the solution it is in, would the molar mass you report for the solid acid be higher th
If your absent minded lab partner spilled deionized water into your NaOH solution, diluting it, would the Ka value you determine for the solid weak acid be greater than
Draw a complete electronic mechanism of the aldol product between benzaldehyde and acetophenone.
An unknown gas that occupies 1.00 L at a pressure of 534 torr and a temperature of 295.7 K weighs 0.9847 g. What is the molecular mass of this gas
Explain which of the following aqueous solutions has the strongest ion-dipole attractions:0.3 M Na3PO4, 0.1 M NiF2,0.2 M Rb2CO3, 0.01 M Sr(OH)2 , 0.03 M ScBr3.
Automobile airbags contain solid sodium azide, NaN3, that reacts to produce nitrogen gas when heated, thus inflating the bag. Calculate the value of w (work) for the following system if 11.8 g of Na
If a system has 2.50 × 102 kcal of work done to it, and releases 5.00 × 102 kJ of heat into its surroundings, what is the change in internal energy of the system
aqueous solutions has the strongest ion-dipole attractions: 0.3 M FeBr3, 0.6 M CaCl2, 0.5 M Ba(NO3)2, 0.2 M (NH4)2SO4, 0.9 M KOH.
Explain for which of the following species resonance is an important property: HONO, HONO2, N3-, NO2-, NO2.
Calculate the wavelength at which this vibration will be found in the anti-Stokes scattering from a nitrogen laser(337nm).
If Ka is 1.85 x 10-5 for actetic acid, calculate the pH at one-half the equivalence point and at the equivalence point for a titration of 50 mL of 0.100 M acetic acid with 0.100 M NaOH
Calculate the pH of a solution prepared by mixing 10.0 mL of 0.500 M NaOH and 20.0 mL of 1.50 M benzoic acid solution. (Benzoic acid is monoprotic: it's ionization constant is 6.7 x 10-5)
Why isn't the pH at the equivalence point always equal to 7 in a neutralization titration? When would it be 7?
Complete and balance the following equations, and identify the oxidizing and reducing agents. Recall that the O atoms in hydrogen peroxide, H2O2, have an a typical oxidation state.
If 27.5 mL of 0.1000 M NaOH are required to neutralize 1.22 g of an unknown acid, HA, what is the molecular weight of the unknown acid? NaOH + HA --> NaA + H2O
If 2.5 mol of ethylene oxide is decomposed at 93 degrees celcius what will be the final temperature of the products? The heat capacity of the products is 110.13J/mol C
Type the electron configuration for the following ions according to the rules in your text. Use the format {He} 2s2 2p2 for carbon. Pay attention to the spaces.
The BF3 molecule has one A'1, one A"2 and tow E' vibrations. Does this representation account for all of the normal mode fundamental vibrations for this molecule
Calculate E cell for the following balanced redox reaction O2(g)+2H2O(l)+4Ag(s)=4OH^-(aq)+4Ag^+(aq)
Calculate the pH of a formic acid solution that contains 1.39% formic acid by mass. (Assume a density of 1.01 for the solution.)
what is the value for deltaS if 20g of a substance (MW=78.0g/mol) is boiled at 50 degrees C
Propose a reasonable reaction mechanism for the sodium hypochlorite oxidation of 3-heptanol. Give the IUPAC name of the expected product. What other oxidizing agents may be used to carry out this ox
Identify the reagents you would need to make the following substance via Grignard synthesis, and briefly describe your synthetic strategy.