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Suppose that you have 0.500 L of each of the following solutions, and an unlimited supply of water. (Note: C9H7NHBr is a salt containing the ions C9H7NH+ and Br? and C9H7N is quinoline, an organic base with pKb = 6.24 at 298 K. If you like, you may represent C9H7NH+ as HB+ and C9H7N as B.) 0.113 mol L?1 C9H7NHBr (aq) 0.104 mol L?1 HBr(aq) 0.122 mol L?1 NaOH(aq) (a)Provide simple instructions for preparing 1.00 L of a solution having pH = 7.00 at 298 K. Your instructions should include the volumes of the solutions required. (b) What is the buffer capacity of the resulting solution? (The buffer capacity is the number of moles of NaOH that must be added to 1.0 L of solution to raise the pH by one unit.)
when 8.00g of NaOH is added to a calorimeter filled with 75.0mL of HCl the temperature of the solution increases for 25.0 C to 33.5 C. calculate the molar heat of neutralization for the NaOH. (assume that the density of the solution is 1.00gmL)
If 3.8kcal of energy is released when 1 gram of glucose is combusted, how many kcals are released when 0.689 moles of glucose are combusted
How many resonance forms are required to represent the bicarbonate ion HOCO21
What is the energy per photon of the lowest frequency of electromagnetic radiation that can be used to observe a gold atom with a diameter of 280 picometers.
Suppose Joule encountered the waterfall at Niagara Falls. Calculate the height if the temperature difference between the top and bottom of the waterfall is 0.20° F.
You are expected to design a car that works with photovoltaic panels. Assume that the driver is 75kg and the expected speed is 50km/hr.
Calculate the partial pressure of each gas in the container. Express the pressure values numerically in atmospheres, separated by commas.
What is the concentration (in M) of the nitrate ion when 17.3 mL of a 0.633 M solution of potassium nitrate is combined with 15.3 mL of a 0.662 M solution of aluminum nitrate to a final volume of 48.1 mL
Consider the malate dehydrogenase reaction from the citric acid cycle. Given the following concentrations, calculate the free energy change for this reaction at 37.0 °C (310 K). ?G°\' for the reaction is 29.7 kJ/mol.
At 50 degrees C, the value of pKw (the dissociation constant for water) is 13.262. Calculate the pH of water at this temperature.
The equilibrium constant for the elctrochemical reaction 2Fe+Cu3(PO4)2 = 2FePO4 + 3Cu occuring in aqueous solution
At 7914 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP = 0.726. If the initial pressure of NO is 0.00366 atm, what are the equilibrium partial pressures of NO, N2, and O2? p(NO) = . p(N2) = . p(O2) = .
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