50.0 ml of 0.100mol/L silver nitrate solution is titrated by 0.0900mol/L ammonium thiocyanate solution. Calculate : pSCN and pAg after addition of 50.0 ml of titrant.

To calculate the pSCN and pAg after the addition of 50.0 ml of titrant, we need to follow these steps:1. Calculate the moles of silver nitrate (AgNO3) in the 50.0 ml solution.2. Calculate the moles of ammonium thiocyanate (NH4SCN) in the 50.0 ml solution.3. Determine the reaction between AgNO3 and NH4SCN.4. Calculate the remaining moles of AgNO3 and NH4SCN after the reaction.5. Calculate the concentrations of Ag+ and SCN- in the final solution.6. Calculate the pAg and pSCN values.Let's go through these steps:1. Moles of AgNO3: Moles of AgNO3 = Volume (L) x Concentration (mol/L) Moles of AgNO3 = 0.050 L x 0.100 mol/L = 0.005 mol2. Moles of NH4SCN: Moles of NH4SCN = Volume (L) x Concentration (mol/L) Moles of NH4SCN = 0.050 L x 0.0900 mol/L = 0.0045 mol3. Reaction between AgNO3 and NH4SCN: AgNO3 + NH4SCN → AgSCN + NH4NO3 The reaction is a 1:1 stoichiometric reaction.4. Remaining moles after the reaction: Since the reaction is 1:1, the limiting reagent is NH4SCN. Remaining moles of AgNO3 = 0.005 mol - 0.0045 mol = 0.0005 mol Remaining moles of NH4SCN = 0 mol5. Concentrations in the final solution: Total volume after mixing = 50.0 ml + 50.0 ml = 100.0 ml = 0.100 L [Ag+] = Remaining moles / Total volume = 0.0005 mol / 0.100 L = 0.005 mol/L [SCN-] = 0 mol/L (since all NH4SCN has reacted)6. pAg and pSCN values: pAg = -log[Ag+] = -log(0.005) ≈ 2.30 pSCN = -log[SCN-] = -log(0) = undefined (since [SCN-] is 0)Therefore, the pAg value is approximately 2.30, and the pSCN value is undefined.