Question

Note:<br />Consider the reaction between Fe3+ and NCS ions. The equilibrium constant for this<br />reaction is 620.4. Calculate the equilibrium concentration of NCS ion in a solution that<br />contains 10.0mL of 0.05 M ferric nitrate in 1M HNO3, 2.0mL of 5.0*10-4 M NaNCS, and<br />8.0mL of distilled water. Assume that all the NCS is converted to FeNCS2+.<br />ㄷ<br />(A) 6.07x10-8 M<br />(B) 3.04x10M<br />(C) OM<br />(D) 1.00x10<br />E​

Answer 1

Answer:

Note:<br />Consider the reaction between Fe3+ and NCS ions. The equilibrium constant for this<br />reaction is 620.4. Calculate the equilibrium concentration of NCS ion in a solution that<br />contains 10.0mL of 0.05 M ferric nitrate in 1M HNO3, 2.0mL of 5.0*10-4 M NaNCS, and<br />8.0mL of distilled water. Assume that all the NCS is converted to FeNCS2+.<br />ㄷ<br />(A) 6.07x10-8 M<br />(B) 3.04x10M<br />(C) OM<br />(D) 1.00x10<br /