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What is the pka of a protonated amide? (Being N protonated)
If 156 mL of wet H2 is collected over water at 24C and a barometric pressure of 736 torr, how many grams of Zn have been consumed?
Question- Calculate the pH for each of the following cases in the titration of 25.0 mL of 0.200 M pyridine, C5H5N(aq) with 0.200 M HBr(aq): 1) After addition of 25.0 mL of HBr
This provides an estimate of the equilibrium concentration of gasoline in contact with the plastic. What percent of the gasoline in the initially full 2 gallon container is lost in a year
Predict the physical state of ammonia at -95 degrees C (mp =-77degrees C, Bp =-33 degrees C) and normal atmospheric pressure.
When 2.150 g of AX (s) dissolves in 200.0 g of water in a coffee-cup calorimeter the temperature rises from 21.2 oC to 32.3 oC. Calculate the enthalpy change (in kJ/mol) for the solution process AX (s) --> A+ (aq) + X- (aq) Assumptions for this calcu..
The absorption spectrum of the complex ion [Rh(NH3)6]3+ has maximum absorbance at 295 nm. Calculate the crystal field splitting energy (in kJ/mol) for this ion.
A buffer with a pH of 4.06 contains 0.23 M of sodium benzoate and 0.32 M of benzoic acid. What is the concentration of [H ] in the solution after the addition of 0.054 mol of HCl to a final volume of 1.4 L?
Calculate the concentration of iodide ions in a saturated solution of lead(ll) iodide. The solubility product constant of PbI2 is 2.7* 10^-6
Suppose if a mineral has a density of 3.57g/cm3 and it adopts a cubic unit cell, with an edge length of 809 pm, Explain how many items of each type are in the unit cell
Cd2 forms two complexes with C2H3O2, with the following formation constants:(a) Find K2 for the reaction, (b) You prepare 1.00 L of solution containing 0.110 mol CH3CO2Na and 4.00 × 10-4 mol Cd(ClO4)2. Compute the fraction of cadmium in the form ..
For each of the half cells compare electrode potentials calculated from (1) concentration and (2) activity data. a) HCl (0.0200 M), Nacl (0.0300 M)|H2 (i.00 atm), Pt b) Fe(Clo4)2 (0.0111M), Fe(ClO4)3(0.0111M)|Pt
Suppose that 1.41 g of impure barium hydroxide is dissolved in enough water to produce 177.1 mL of solution and that 44.1 mL of this solution is titrated to the stoichiometric point
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