Perform the calculations
needed to generate a titration
curve for 50.00 ml of a 0.0500
M NaCl solution titrated with
0.1000 M AgNO3 . Note for
AgCl the Ksp = 1.82×10-10
.
(i) Calculate pAg when 10.00 ml of
AgNO3 is added.
(ii) Calculate pAg when 25.00 ml of
AgNO3 is added.
(iii) Calculate pAg when 26.00 ml of
AgNO3 is added.
Given the solubility products
above, show (by calculation)
which of the two compounds
concerned has the greater
solubility in water.
Ksp(AgCl) = 1.78x10-10
Ksp(Ag2CrO4) = 2.45x10-12
Perform the calculations needed to generate a titration curve for 50.00 ml of a 0.0500 M...
6A. Construct the titration curve for a 20.00 m, mixture solution of 0.0800 M in I and 0.0800M in Cl titrated with 0.1000 M AgNO3. Calculate the pAg values of the titration solution atter addition of 6.00mL, 16.00 mL, and 26.00 mL of 0.1000 M AgNO solution. 18) Kp AgCl = 1.77 × 10-10ー[Ag+][Cl] Ksp Agl 8.3 x 101-AgI
Construct a curve for the titration of 50.00 mL of a 0.1000 M solution of compound A with a 0.2000 M solution of compound B in the following table. For each titration, calculate the pH after the addition of 0.00, 12.50, 20.00, 24.00, 25.00, 26.00, 37.50, 45.00, 49.00, 50.00, 51.00, and 60.00 mL of com- pound B. A (a) H2SO3 (b) ethylenediamine (c) H2SO4 B NaOH HCl NaOH
A 50.00 ml aliquot of 0.1000 M NaOH is titrated with 0.1000 M HCL. Calculate the pH of the solution after the addition of 0.00, 10.00, 25.00, 40.00, 45.00, 49.00, 50.00, 51.00, 55.00, and 60.00 ml of acid and prepare a titration curve from the data.
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]
In the titration of 50.00 mL of 0.1000 M sodium formate (NaCO2H, whose conjugate acid is HCO2H, and Kb of CO2H- = 1.8 x 10-5) with 0.1000 M HCl at 25.0 C, calculate the pH of the solution when the 25.00 mL of HCl has been added.
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
Calculate the hypothetical pH AFTER addition of 15.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with 0.1000 M HCl at 25°C. QUESTION 7 10 poir Calculate the hypothetical pH AFTER addition of 40.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with 0.1000 M HCl at 25°C. Calculate the hypothetical pH AFTER addition of 46.00 mL of reagent for the titration of 50.00 mL of 0.0800 M NaOH with...
Calculate the hypothetical pH AFTER addition of 40.00 mL of reagent for the titration of 50.00 mL of 0.0800 M HCl with 0.1000 M NaOH at 25°C. Auranmaa Calculate the hypothetical pH BEFORE acid is added for the titration of 50.00 mL of 0.0800 M NaOH with 0.1000 M HCl at 25°C.
Calculate the hypothetical pH BEFORE acid is added for the titration of 50.00 mL of 0.0800 M Formic Acid (HCOOH, Ka= 1.80x104) with 0.1000 M NaOH at 25°C. Calculate the hypothetical pH AFTER addition of 15.00 mL of reagent for the titration of 50.00 mL of 0.0800 M Formic Acid (HCOOH, Ka= 1.80x10-4) with 0.1000 M NaOH at 25°C. Calculate the hypothetical pH AFTER addition of 40.50 mL of reagent for the titration of 50.00 mL of 0.0800 M Formic...
Calculate the hypothetical pH AFTER addition of 10.00 mL of reagent for the titration of 50.00 mL of 0.0800 M HCl with 0.1000 M NaOH at 25°C.