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A 0.223 molar solution of the weak acid, HA, with a pKa of 3.954 is titrated with a 0.142 molar solution of NaOH.
What is the solubility of aluminum hydroxide in water at 25 degrees Celsius if the Ksp is 3 x 10^-34? What is the concentration of Hydroxide at equilibrium?
A 12.0-L container holds these gases at equilibrium. What is the value of Kc for this reaction if there are 1.036 g NO2Cl, 5.962 g NO2, and 4.578 g.
What will be the concentrations of Ca2+ and Mg2+ ions just as the most soluble flouride starts to precipitate?
In the reaction of ammonium chloride (as a solid) dissociating to produce ammonia and hydrogen chloride (both as gases), the equilibrium concentration.
Determiniation of the Molar Mass and Ionization Constant of a Weak Monoprotic Acid.
The hemoglobin molecule carries O2 in the blood from the lungs to the cells, where the O2 is released for metabolic processes.
When 2.0 mol of carbon disulfide and 4.0 mol of chlorine are placed in a 1.0 Liter flask and the system allowed to come to equilibrium, the flask.
Calculate the value of the equilibrium constant for each of the following reactions ( we abbreviate citric acid as H3Cit) using the Ka values for citric acid.
Calcium sulfate is sometimes added to wine both to clarity and to percipitate dissolved lead.
Heat is liberated in the dissolving process. Does the tendency toward minimum energy favour the separated pure substances, or the solution.
Consider a solution that is 0.10 M in a weak triprotic acid that is represented by the general formula H3A with the following ionization constants.
What is the concentration of free Zn+2 in a solution of 3M NH3 (total ammonia) buffered to a pH of 9.0 if the total zinc concentration is 0.1M?
What is the partial pressure of NO under these conditions if the partial pressures of nitrogen and oxygen are 3.0 atm and 0.013 atm, respectively?
Why is it important to study chemical equilibrium? In what industries might such knowledge be particularly useful? Explain your answer.
The following data were collected for the rate of disappearance of NO in the reaction 2NO(g)+O2(g)-----> 2NO2(g)
Given that the standard free energy of formation (?Gof) of NH3 (g) is -111 kJ/mol at 335 K, calculate the equilibrium constant, K, at this temperature.
If a change is made in the gas temperature which causes the volume of the gas sample to become 620 ml at 1.00 atm, what is the new temperature?
Assuming the volumes are additive, calculate the molar concentration of Ba2+ (aq) and CrO4 (aq) in the 1.00 L solution.
Calculate the maximum mass , in grams , of Ag2CrO4 that can dissolve in 100ml of water at 25°C.
Write the equilibrium constant expression for the ionization of the HOBr in water, then calculate the concentration of the HOBR(aq).
Will a precipitate form when 250 ml of 0.33 M Na2CrO4 are added to 250 ml 0.12 M AgNO3?
Assuming the reaction is at equilibrium, classify each of the following actions by whether it causes a leftward shift, a rightward shift.
For each of the equilibria in problem #1 predict (1) how Ke is affected by an increase in temperature, (2) predict how the equilibrium.
A 120.0ml sample fo a solution that is 2.8x10^-3M in AgNO3 is mixed with a 225ml sample of a solution that is .1M in NaCN.