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Concentrated aqueous HClO4 has a concentration of 14.8 M. Calculate the concentrations of all ions present in a solution prepared by pipetting 4.19 mL of concentrated HClO4 into a 1000. mL volumetric flask and filling to the mark.
Hydronium ion concentration?
Perchlorate ion concentration?
Hydroxide ion concentration? Kw = 1.0E-14.
What is the molarity of a solution prepared by adding 29.3 g of HNO3 to enough water to make 2 L of solution
A solution is 0.0100 M in Pb2+ ions. If 0.103 mol of solid NaI is added to 1.00L of this solution (with negligible volume change), what percent of the Pb2+ ions remain in solution?
Consider the reaction 2 Al2O3(s) → 4 Al(s) + 3 O2(g). ?H = +3339.6 kJ/mol What is ?H for the formation of one mole of Al2O3(s) from the elements
How many moles of copper atoms were lost? ii. The Faraday constant. iii. The charge of one electron. iv. The mass of one electron.
A rigid flask is initially filled with 4.00 atm of NO2(g) and no N2O4(g) at 100 C. After equilibrium is achieved, the pressure of NO2 is 1.56 atm.
You have 50 mL of 0.010 fully protonated histidine. how many milimoles of base must be added to bring histidine solution to pH equivalent to the pI of histidine.
A quantity of N2 occupies 62.2 L at a particular temperature and pressure. Its density is 0.900 g/L. How many moles of N2 are in the container?
a 93 L sample of dry air cools from 145 degrees C to -22 degrees C while the pressure is maintained at 2.85 atm. what is the final pressure?
Determine the empirical and molecular formula and draw the Lewis structure for a compound
How many neutrons and protons are contained in the nucleus of this isotope?
What is the molarity of each ion in a solution prepared by dissolving 0.550 g of Na2SO4, 1.192 g of Na3PO4, and 0.228 g of Li2SO4 in water and diluting to a volume of 100.00mL?
The following set of reactions can be used to produce nitric acid, HNO3. Calculate the mass of nitric acid produced from the reaction of 15.5 kg of nitrogen gas with excess hydrogen gas. Each reaction in turn has an excess of the second reactant a..
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