Calcium hydrogen carbonate and nitric acid

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Revision Questions –StoicQ1. When alchemists gently heated mercury(II) oxide, a “mirror” of mercury condensed on the walls of the vessel. The equation for this is:2HgO(s) 2Hg(l) + O2(g)What mass of mercury(II) oxide must have reacted if a mirror containing 10.0g of mercury was produced?Q2. In the sealed environment of a space shuttle, canisters of the strong base lithium hydroxide are used to absorb carbon dioxide so that toxic levels do not build up. The reaction is shown in the following equation:2LiOH(s) + CO2(g) Li2CO3(s) + H2O(l)What mass of carbon dioxide can be absorbed by 200g of lithium hydroxide?Q3. A piece of copper wire of mass 2.25g completely dissolves on a solution of silver nitrate. The balanced equation for the metal displacement reaction is:Cu(s) + 2AgNO3(aq)Cu(NO3)2(aq) + 2Ag(s)(a)What mass of copper(II) nitrate will be produced?(b)What mass of crystals of pure silver crystals will be produced in this process?Q4. When a cake mixture containing bicarb soda, NaHCO3, isbaked, the sodium hydrogen carbonate decomposes according to the following equation:2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(l)The CO2gas produced rises through the mixture, causing the cake to rise. However, if too much bicarb soda is used, the cake will be spoilt because the sodium carbonate has a bitter, foul taste.If 0.60g of bicarb soda is used:(a)What mass of carbon dioxide gas will be produced?(b)What mass of sodium carbonate will be produced?(c)From your answers to parts a and b, deduce the mass of water vapourthat will produced, state your reasoning.Q5. When concentrated nitric acid is poured onto copper, a vigorous reaction occurs and a pungent brown gas is evolved. This is nitrogen dioxide gas, NO2. When the reaction has ceased, the remaining solution is blue. The balanced equation is:Cu(s) + 4HNO3(l) Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)(a)What mass of copper(II) nitrate will be produced when excess concentrated nitric acid is poured on to 3.85g of copper?(b)What mass of nitrogen dioxide gas will be produced in the process?
Q6. The combination of limestone country and a steady rainfall can lead to the formation of stunning underground caves. This is because even pure rain has a pH of 6, since carbon dioxide dissolves in it and produces carbonic acid, H2CO3, a weak acid. This acid acts on the limestone, CaCO3, and dissolves it in the form of soluble calcium hydrogen carbonate. The simplified equation for the solution process that creates a cave is:CaCO3(s) + H2CO3(aq) Ca(HCO3)2(aq)As the solution drips down from the ceiling of the cave, it decomposes:Ca(HCO3)2(aq) CaCO3(s) + CO2(g) + H2O(g)Thus solid limestone forms again, producing stalactites suspended from the ceiling and stalagmites that rise from the floor where the drips have landed.(a)What mass of solid limestone is formed when 1.00kg of calcium hydrogen carbonate completely decomposes?(b)What mass of carbon dioxide is returned to the air during this decomposition process?Q7. What must be the concentration of a solution of ammonium hydroxide, if a 20.00mL sample of the solution requires precisely 19.04 mL of hydrochloric acid of concentration 0.1058 mol/L to completely reaction with it? The full equation for the reaction is:HCl(aq) + NH4OH(aq) NH4Cl(aq) + H2O(l)Q8. What must be the concentration of a hydrochloric acid solution is a 20.00mL sample of the solution requires precisely 21.46mL of sodium carbonate solution of concentration 0.05129M to completely react with it?2HCl(aq) + Na2CO3(aq) 2NaCl(aq) + CO2(g) + H2O(l)Q9. Lactic acid HC3H5O3, is a weak, monoprotic acid that accumulates as a waste product in muscle tissue during exertion, leading to pain and a feeling of fatigue. What must be the concentration of a sample of lactic acid 20.00mL of sodium hydroxide of concentration 0.1426M requires 24.58mL of the acid for a complete reaction?HC3H5O3 (aq) + NaOH(aq) NaC3H5O3(aq) + H2O(l)Q10. (a)Write the balanced full equation for the neutralisation reaction of potassium hydroxide solution by nitric acid(b)What massof potassium nitrate would be produced by the addition of 19.50mL 0.1249M nitric acid to 20.00mL of 0.09878M potassium hydroxide solution.Q11.(a)Write the balanced full equation for the neutralisation of sodium hydroxide by sulphuric acid(b)What mass of water would be produced when 25.00mLof sulphuric acid of concentration 0.1510M is addedto exactly 20.00mL of sodium hydroxide of concentration 0.2485M?