If a sample of solid KNO3 (MW 101.1 g/mol) is weighed and submitted to cation ex

Question

If a sample of solid KNO3 (MW 101.1 g/mol) is weighed and submitted to cation exchange, an aqueous solution of what substance (compund) will emerge from the bottom of the Amberlite resin column?

If 0.1230g of KNO3 were submitted to the procedures of this experiment, how many moles of the substance you identified above would emerge (elute) from the bottom of the column?

How many mL of a 0.1002 M NaOh solution would be required to titrate the moles of the substance eluted from the column in the previous question?

Explanation / Answer

1) HNO3 aqueous solution emerge out

     KNO3+ H-Resin ------> K+ - Resin   + HNO3

2) mole of KNO3 = 0.123g/ (101.1g/mol) = 1.216 x 10-3 moles

therefore 1.216x 10-3 moles of HNO3 is illuted out form the column

3) NaOH + HNO3 = H2O + NaNO3

     M1V1 = Moles

      V1 = 1.216x 10-3 moles/L / ( 0.1002 M) = 0.012 L = 12 ml

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