A 25.00 mL solution of 0.08050 M NaI is titrated with 0.05000 M AgNO3 . Calculate pAg+ following the addition of the given volumes of AgNO3 . The ?sp of AgI is 8.3×10−17 . 35.80 mLpAg+= ?epAg+= 47.90 mLpAg+=
A 25.00 mL solution of 0.08050 M NaI is titrated with 0.05000 M AgNO3 . Calculate pAg+ following the addition of the giv...
A 25.00 mL solution of 0.08700 M NaI is titrated with 0.05140 M AgNO3 . Calculate pAg+ following the addition of the given volumes of AgNO3 . The
A 25.00 mL solution of 0.08610 M Nal is titrated with 0.05000 M AgNO . Calculate pAg+ following the addition of the given volumes of AgNO,. The Ksp of Agl is 8.3 x 10-'7. 37.40 mL pAgt = V pAgt = 47.90 mL pAgt =
The Ksp of AgI is 8.3× 10–17. You titrate 25.00 mL of 0.08160 M NaI with 0.05190 M AgNO3. Calculate pAg after the following volumes of AgNO3 are added: (a) at 35.10 mL (b) at Ve (volume at equilibrium) (c) at 47.10 mL
Consider the titration of 25.00 mL of 0.0925 M KI with 0.0695 M AgNO3. Calculate pAg+ at the following volumes of added AgNO3: (a) 30.00 mL; (b) Ve; (c) 35.27 mL. Ksp (AgI) = 8.3×10-17
The Ksp of AgI is 8.3× 10–17. You titrate 25.00 mL of 0.08870 M NaI with 0.05050 M AgNO3. Calculate pAg after the following volumes of AgNO3 are added: (a) 37.20 ml (b) Veq (c) 47.20 ml
Consider the titration of 25.00 mL of 0.07920 M KI with 0.05410 M AgNO3. Calculate pAg+ at a) 25.00 mL > ?? b) Ve > M1V1 = M2V2 (0.07920)(0.025)=(0.05410)(Ve) --------> Ve = 36.60 mL c) 45.00 mL > ?? of AgNO3 added (Ksp= 8.3*10-17). Show ALL work. pAg+ = -log[Ag]
A 25.00 mL solution of 0.03220 M Na2CO3 is titrated with 0.02510 M Ba(NO3)2 . Calculate pBa2+ following the addition of the given volumes of Ba(NO3)2 . The ?sp for BaCO3 is 5.0×10−9 . 13.90 mLpBa2+= ?epBa2+= 37.40 mLpBa2+=
A 25.00 mL solution of 0.03190 M Na2CO3 is titrated with 0.02660 M Ba(NO3)2 . Calculate pBa2+ following the addition of the given volumes of Ba(NO3)2 . The ?sp for BaCO3 is 5.0×10−9 . 15.50 mL pBa2+= ?ep Ba2+= 35.50 mL pBa2+
At 25 ∘C, a titration of 15.00mL of a 0.0360 M AgNO3 solution with a 0.0180 M NaI solution is conducted within the cell SCE || titration solution | Ag(s) For the cell as written, what is the potential after the addition of each volume of NaI solution? The reduction potential for the saturated calomel electrode is ?=0.241 V. The standard reduction potential for the reaction Ag+ + e− ⟶Ag(s) is ?∘=0.79993 V. The solubility constant of AgI is ?sp=8.3×10−17....
A 25.00 mL solution of 0.03060 M Na,Co, is titrated with 0.02550 M Ba(NO3), Calculate pBa?' following the addition of the given volumes of Ba(NO3), The Kep for Baco, is 5.0 x 10-. 14.90 mL pBa²+ = V. pBa²+ = 37.60 mL pBa2+ =