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Calculate the reaction Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g) What mass of ZnCl2 (MW = 136.3 g/mol) can be prepared from the reaction of 3.27 grams of zinc (MW = 65.38 g/mol) with 3.00 grams HCl (MW = 36.46)?
Methylbenzene and 1,2-dimethylbenzene mix to form an ideal solution. At 90oC, the vapor pressure of pure methylbenzene is 400 Torr and that of pure 1,2-dimethylbenzene is 150 Torr.
A fluoridated water supply contains F- at a concentration of 8.9 ppm. What is the maximum concentration of Mg2+ that can exist in this water supply without causing precipitation.
500cm3 of 0.250M of Na2SO4 is added to an aqueous solution of 15.0g of BaCl2 resulting in a white precipitate of insoluble BaSO4.
A gas was enclosed in a rigid-walled container. The initial temperature and pressure were 52°C and 0.55 atm, respectively. If the final pressure were 2.41 atm.
suppose you wanted to dissolve 106 g of Na2CO3 in enough H2O to make 6.00L of solution what is the molar mass of Na2CO3.
What is the pH at the half-stoichiometric point (half-way to the endpoint) for the titration of 0.22 M HNO2(aq) with 0.10 M KOH(aq)?
The minimum frequency of light needed to eject electrons from a metal is called the threshold and find the minimum energy needed to eject electrons from a metal with a threshold frequency of 3.27*10^14s^-1.
Zinc chloride (ZnCl2) is 52.02% chlorine by mass. What mass of chlorine is contained in 66.0 g of ZnCl2?
Consider two solutions. One solution is 0.1115 M Ca(OH)(2). The other is 0.1050 M HClO(4). a) Write a balanced equation for the reaction between the two solutions.
A sample of laughing gas occupies 500.0Ml at a standard temperature and pressure . what volume will the gas occupy at 95.0oC and 525 torr.
At 25 c the ion product of water, Kw is 1.9 x 10^-14. What is the concentration of hydroxide ions in a solution where the concentration of hydrogen is found to be 5.0 x 10^-15 mol dm^-3.
Calculate the concentration of a solution of FeCl3 was prepared by dissolving 13.86 gm of FeCl3 in 2.5L of water.
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