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Calculate the pH of a solution containing 0.085M nitrous acid (ka = 4.5 x 10-4) and 0.100M KNO2.
Calculate the [Zn2+] in a solution of ZnC2O4 held at a pH of 3.00. Remember C2O4^2- is a weak base so you must consider other equilibria.
What will be the final concentrations of NH3,N2, and H2 after equilibrium is established. I know the answers are suppose to be H2=.170M, NH3=.0424M, N2=.0568M, but I don't know how to get them.
The pH of a solution of ammonia, NH3, is measured at equilibrium and found to be 11.48. Given that Kb for NH3 is 1.8 X 10?5, what was the initial (before equilibrium) concentration of NH3
Supercooled (metastable) water vapor commonly occurs in the atmosphere if dust particles are not present to begin condensation of the liquid.Sometimes small particles,such as tiny crystals of silver iodide
A 75.0-mL volume of 0.200 NH3 is titrated with 0.500 M HNO3 . Calculate the pH after the addition of 19.0 mL of HNO3
Suppose you have the following reagents available under standard conditions. (i.e., P = 1 atm for all gases; t = 25 oC; C = 1 mol L-1 for all aqueous species, including H+.) Co(s), Ag+(aq), Cl-(aq), Cr(s), BrO3-(aq), I2(s), F-(aq) (a) Which is the..
The higher heating value (HHV) of a fuel is its standard heat of combustion at 25 C with liquid water as a product; the lower heating value (LHV) is for water vapor as product.
Marble (calcium carbonate) reacts with hydrochloric acid solution to form calcium chloride solution, water, and carbon dioxide.
The volume of a sample of ethane, C2H6, is 2.66 L at 447 torr and 30 °C. What volume will it occupy at standard temperature and pressure (STP)
Calculate the heat of the reaction. (Use the equation Q = s . m .?T where s is the specific heat, m is the mass of solution and ?T is the change in temperature)
How the concentration on Cl- was calculated from a solution of 0.0167M CdCl2. It gives the value [Cl-]=0.0334
The bromocresolgreen end point of the titration was reached after the addition of 30.00 mL of hydrochloric acid solution. Calculate the concentration of the acid solution.
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