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Calculate the molality of a solution formed by dissolving 27.8 g of LiI in 500.0 mL of water.  (Report answer with correct units to 3 decimal places)

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10-4 M O2 at 25°C. The Henry’s law constant for oxygen in water at 25°C is 1.3 × 10-3 M/atm.  (report you answer WITH UNITS to the second decimal place.)

Please explain why homeostasis is important to a properly functioning body and provide and example of homeostasis.   Define the following terms or use the in an example to provide evidence of student comprehension:   Effector, Receptor, Balance, Imbalance, Afferent, Stimulus, Efferent Control Center. 

Find the percent ionization of 0.337 M HF solution. The Ka for HF is  3.5 X 10-4.

Consider a reaction that has a positive ΔH and a positive ΔS. Which of the following statements is TRUE?

What is the conjugate acid of HCO3-?

Determine the solubility of N2 in water exposed to air at 25 °C is the atmospheric pressure is 1.2 atm. Assume that the mole fraction of nitrogen is 0.78 in air and the Henry’s law constant for nitrogen in water at this temperature is 6.1 X 10-4 M/atm.

The overall order of the following reaction is ______.   (**Just give the whole number i.e. 1 for 1st, 2 for 2nd, 3 for 3rd ect….) 2X + 3Y à 2Z                               Rate = k[BLANK-1][BLANK-2]2

Balance the following redox reaction if it occurs in an acidic solution. What are the coefficients in front of H2C2O4 and H2O in the balanced reaction? MnO4- (aq) + H2C2O4 (aq) à Mn2+ (aq) + CO2 (g)

The equilibrium constant is given for one of the reactions below.  Determine the value of the missing equilibrium constant. N2O4 (g) ⇌ 2NO2 (g)                 Kc = 1.46                                                      6NO2 (g) ⇌ 3 N2O4 (g)       Kc  = ?