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Problem- You carefully weigh out 19.00g of CaCO3 powder and add it to 76.95g of HCl solution. You notice bubbles as a reaction takes place. You then weigh the resulting solution and find that it has a mass of 88.16g. The relevant equation is
CaCO3(s)+2HCl(aq)?H2O(l)+CO2(g)+CaCl2(aq) Assuming no other reactions take place, what mass of CO2 was produced in this reaction?
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In a test tube, 10 mL of 0.100 M KI and 10 mL of 0.100 M Na2CO3 are mixed. Next, 0.10 M lead nitrate is added drop wise. What will be the concentration of CO3 2- when PbI2 first starts to precipitate? Ksp (PbCO3) = 1.5 x 10^-13 Ksp (PbI2) = 8.7 x 1..
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