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A solution is prepared by dissolving 0.075 mol of cyanoacetic acid (Ka-3.37×10-3) and 0.030 mol of sodium cyanoacetate in water to a total solution volume of 1.00 L. First, calculate a pH for the solution by assuming that the concentrations of NCCH2CO2H and NCCH2CO2 are equal to the formal concentrations of the substances dissolved. 2.07 Computers answer now shown above. You are correct. Your receipt no. is 160-8794 () Previous Tries Next, calculate the pH for the solution based on the equilibrium concentrations of NCCH2CO2H and NCCH2CO2 2.33 Submit Answer Incorrect. Tries 2/5 Previous Tries Use the Henderson-Hasselbalch approximation to calculate the pH of a solution prepared by dissolving in water, to a final volume of 1.00 L, 0.140 mol of cyanoacetic acid, 0.040 mol of 2.47 sodium cyanoacetate, 0.050 mol of HNO3 and 0.050 mol of Ca(OH)2 Computers answer now shown above. You are correct. Your receipt no. is 160-2289 Previous Tries

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