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17 Nov 2019
Please help! A 0.5250 sample containing only NaHCO_3 (MW = 84.01) and Na_2CO_3 (MW = 105.99) was dissolved in 30.0 mL of water. The solution was titrated with 0.2010 M HCI and the first equivalence point in the reaction was reached when 14.20 mL of acid had been added. Ka_1(H_2CO_3) = 4.3 times 10^-7 and Ka_2(H_2CO_3) = 4.8 times 10^-11. Determine the weight percent of Na_2CO_3 in the original sample. Determine the total volume of acid needed to reach the second equivalence point. Calculate the pH of the solution at the beginning of the titration.
Please help!
A 0.5250 sample containing only NaHCO_3 (MW = 84.01) and Na_2CO_3 (MW = 105.99) was dissolved in 30.0 mL of water. The solution was titrated with 0.2010 M HCI and the first equivalence point in the reaction was reached when 14.20 mL of acid had been added. Ka_1(H_2CO_3) = 4.3 times 10^-7 and Ka_2(H_2CO_3) = 4.8 times 10^-11. Determine the weight percent of Na_2CO_3 in the original sample. Determine the total volume of acid needed to reach the second equivalence point. Calculate the pH of the solution at the beginning of the titration.
Beverley SmithLv2
27 Sep 2019