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Write expressions for the equilibrium constants for the following reactions: Formulate these expressions in terms of the degree of dissociation.
0.375 g of a monoprotic acid (mm = 245 g/mol) is dissolved in water to produce 25.0 mL of a solution with pH = 3.28. Determine the ionization constant of the acid.
When a 6.00-g sample of KCN is dissolved in water in a calorimeter that has a total heat capacity of 3.850 kJ·K-1, the temperature decreases by 0.280 K. Calculate the molar heat of solutio
How do you who that both ZnS and CuS will precipitate at pH8. 2) Show that only CuS will precipitate when (H3O+) = 0.3M.
Lindane, a powerful insecticide, is a member of this group. The molar mass of lindane is 290.8. How many atoms of carbon does a molecule of lindane contain?
A buffer was prepared by adding 2.4 g of ammonium nitrate to 100.0 mL of 0.30 M ammonia (Kb = 1.8 × 10-5). To this solution was then added 10.0 mL of 0.30 M sodium hydroxide, what is the pH
During a structure fire, the pump runs for 30 minutes. How many pounds of water are used to extinguish the fire? The density of water is 1.0 grams per milliliter.
What is the remaining Ag+ ion concentration and is precipitation complete? The solubility product constant of AgBr is 5.0 × 10-13.
Assuming 91% efficiency for conversion of potential to electrical energy, and 8% loss of the resulting power in transmission, what is the mass flowrate of water required to power a 200-watt light
A gas has the equation of state PV=RT+a(T)P. Show that for a reversible expansion between T1 and T2 at constant pressure P, the work done is.
The final temperature was 27.1oC exactly. The specific heat capacity of water is Cp=4.1855 J/g oC. What is the specific heat capacity of the solid?
A buffer solution contains 0.17 mol of propionic acid and 0.24 mol of sodium propionate in 1.50 L. What is the pH of the buffer after the addition of 0.01 mol of HI?
A typical amount would be 7.6 * 10^(-5) of Kl per gram of NaCl. What is the concentration of potassium iodide in terms of part per million (ppm)?
How many quartz of ethylene glycol, C2H6O2 (density = 1.116 g/mL). Will have to be added to 5 gal of water (density = 1 g/mL) to protect an automobile radiator down to a temperature of-10oF?
Describe the points of rutherford's model for the nuclear atom and how he tested this model. based on his expiriments, how did ruthford envision the structure of an atom?
Draw the Newman projections for the anti and gauche forms of 1,2-dibromoethane. The molecule has a dipole moment of 1.0 D.
What mass of salt would have to be added to 1000.0 mL of water in order to raise the boiling point of the solution by 0.5 C? Assume the ideal van't Hoff factor for NaCl.
The osmotic pressure of the solution is measured to be 8E-4 bar at 25 C. What is the calculated molar mass of the protein?
What molal concentration of salt is needed to lower the freezing point to -3.97 C? Assume that the solution is ideal, and that the van't Hoff factor for NaCl is the expected (ideal) value.
The rate constant for the equation is 0.0406 M-1 s-1. We start with 0.236 mol C2F4in a 3.00-liter container, with no C4F8initially present. What will be the concentration of C2F4after 3.00 hours?
When a nucleus of 240^Pu undergoes fission, it breaks into two smaller, more tightly bound fragments. Calculate the binding energy per nucleon for 240^Pu.
What will be the pressure of the gas if the temperature rises to 94 degrees Celsius and while the volume decreases to 12 liters?
If a particular alloy is prepared by mixing 11.2 moles of copper with 1.5 moles of nickel, what is the mass percentage of nickel in the alloy?
What is the value of Kf for acetic acid, given that its freezing temperature is 16.6 C and its density is 1.049 g/mL? Experiments show that a solution prepared by dissolving 5.00 grams of water.
If the work function for a metal is 1.8 eV, what would be the stopping potential for light having a wavelength of 400 nm? What would be the maximum velocity of the emitted photoelectrons at the meta