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- Write the balanced NET ionic equation for the reaction when AgC₂H3O₂ and Ni(CIO4)2 are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.The aluminum in a 1.2 g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia. The precipitate was filtered and ignited at 1000 oC to give anhdrous Al2O3, which weighed 0.1798 g. Express the result of this analysis in terms of % NH4Al(SO4)2 and % Al2O3 (Molar mass of Al2O3 =101.96 g/mol, Molar mass of NH4Al(SO4)2= 237.15 g/mol)The powerful oxidizing agent Ce(IV) can be used to quantitatively determine the concentration of methylmalonic acid (MeMA) in a 500 mL beaker. The reaction proceeds as follows: CH3CH(COOH)2 + 6Ce(IV) + 2H₂O → CH3COOH + 6Ce(III) + 6H* + 2CO₂ If the initial concentration of Ce(IV) in the beaker was 0.3M, and 20.0 mL of 0.5 M Fe2+ was required to back-titrate the excess Ce(IV), what was the concentration of Me MA initially present? A. 0.047 M B. 0.28 M C. 0.020 M D. 0.023 M
- What are the main equilibria involved in the CO2–Carbonate system and what kind of equilibrium constant is associated with each (K?)?In which of the following solutions would PbBr₂ be the most soluble? O 0.10 M Pb(NO3)2 O 0.20 M KNO3 0 0.15 M NaBrWhat mass of NaOHNaOH is needed to precipitate the Cd2+ ions from 30.0mL of 0.500 M Cd(NO3)2 solution?
- When 15.11 ml of 0.102 M K2SO4 solution reacts with 35.00 ml of 0.114 M Pb(C2H3O2)2, predict the theoretical yield of the solid product.After preparing a sample of alum, K2SO4-Al2(SO4)3-24H2O, a student determined its purity gravimetrically in a sample of 1,2931 g, the aluminum precipitated as: Al(OH)3. The precipitate was collected by filtration, washed, and calcined to Al2O3, producing 0.1357 g. What is the purity of the alum preparation? [Answer: 97.7%]What is the concentration of Cl- ions in a solution of 0.30 M FeCl3 (aq) ?
- The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175mg CaCO3/L?Write a formula for the following precipitate and write a balanced net ionic equation for the reaction that occured between this precipitate and 3 M HNO3(aq). CO32- and 0.2M Pb(NO3)2Limestone consists mainly of the mineral calcite, CaCO3. The carbonate content of 0.5413 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel CO2: CaCO3(s, 100.087 g/mol) + 2 H+ → Ca2+ + CO2(g) + H2O The excess acid required 39.96 mL of 0.1004 M NaOH for complete titration to a phenolphthalein end point. Find the weight percent of calcite in the limestone.