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20mL of 6.0M NaOH was added to a 50mL beaker containing 2.719g Cu(NO3)2. Then merely enough NaOH was added to make the solution basic.
Utilize this formula
Cu(NO3)2(aq)+2NaOH(aq)-->Cu(OH)2(s)+2NaNO3(aq)
Explain which reactant is limiting, the copper(II) nitrate or the sodium hydroxide?
Compute the amount (grams) of copper(II) hydroxide that was prepared.
What is the concentration (M) of a compound with an absorbance of 0.55 and an extinction coefficient of 3.5 M-1cm-1 with a path length of 1cm
1. how many grams of solute are needed to prepare a910.0 ml of a 6.75 x 10-3nbspm potassium carbonate solution?2. 320 g
What mass of CaCO3 will produce 8.0 L of CO2, measured at standard temperature and pressure conditions? Molar mass of CaCO3 = 100. g per mole.
The overall formation constant for Cu(NH3)42+ is 1.1x1013 at 25oC. What is [Cu2+], in moles per litre, at equilibrium when 8.3 g Cu(NO3)2 is dissolved in 0.500 L of 1.00 mol/L NH3(aq)
The following table lists molar concentrations of several ions in seawater. Using a density of 1.022 g/mL for seawater
Arrange the molecules in order of decreasing boiling point. Rank the molecules from highest boiling point to lowest boiling point.
Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose that a can contains a residual amount of gas at a pressure of 765 mmHg and a temperature of 35*C.
Calculate the pH after adding 0, 10.0, 25.0 and 30.0 mL of titrant in the titration of 50.0 mL of 0.100M NaOH with HCl 0.200 M.
a gaseous mixture of o2 and n2 contains 30.8 percent nitrogen by mass. what is the partial pressure of oxygen in the
a compound x contains the elements carbon hydrogen and oxygen. after 35 g of x were burned in pure oxygen 59 g of
Calculate the experimental percent by mass of copper in the sample and the theoretical mass percent of copper in copper (II) acetate monohydrate.
Calculate the volume of carbon dioxide at 20.0 degrees C and 0.910 atm produced from the complete combustion of 5.00 methane. Compare your result with the volume of CO2 produced from the complete combustion of 5.00 kg of propane (C3H8).
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