0.01M 50 mL Na2CO3 sodium carbonate solution with initial pH and 0.1 M HCl during titeration 1.and calculate the 2nd milestone pH values.Ka1= 1.8.10-6 Ka2= 4.3.10-11
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0.01M 50 mL Na2CO3 sodium carbonate solution with initial pH and 0.1 M HCl during titeration 1.and calculate the 2nd milestone pH values.Ka1= 1.8.10-6 Ka2= 4.3.10-11
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- Construct a curve for the titration of 20.00 mL 0.0500 N succinic acid (HO2CCH2CH2CO2H) by 0.1000 N NaOH solution. MS Excel® can be used. Titrant volumes: 15.00 mL, 20.00 mL, and 25.00 mL. (CH2)2(CO2H)2 ⇌ (CH2)2(CO2H)(CO2)^− + H^+ Ka1 = 6.21 × 10^-5; pKa1 = 4.207 (CH2)2(CO2H)(CO2)− ⇌ (CH2)2(CO2)2^2− + H^+ Ka2 = 2.31 × 10^-6; pKa2 = 5.636A 0.500-g sample containing BaBr2 (FM = 297.14) is dissolved in 50 mL of distilled water. Titrating with 0.0400 M AgNO3 requires 25.00 mL to reach the Mohr endpoint. A blank titration requires 0.50 mL to reach the same endpoint. Calculate the %w/w BaBr2 in the sample. Please provide a complete solution.Calculate the initial pH of 0.01M 50 mL Na2CO3 sodium carbonate solution and the pH values of the 1st and 2nd end points during titration with 0.1 M HCl. Ka1= 1.8.10-6Ka2= 4.3.10-11
- . 100 ml boiled cooled and filtered water sample takes 9.6 ml of M/50 EDTA in titration. The Permanent hardness of the water sample in terms of ppm of CaCO3 equivalent is100 mL water sample was subjected to DO analysis using the Winkler method. The initial reading of the titrant (0.025 M Na2SO3) in the buret was 2.51 mL. The endpoint was obtained and the final reading was 7.07 mL. A blank was also titrated and 0.75 mL of the titrant was consumed. Compute for the amount of DO (mg/L) in the sample.alculate the Ksp of a Ca(OH)2 solution using the data below: Titrated with 0.103MHCl Initial syringe value: 9.71 Final Syringe value: 1.53 Volume of Ca(OH)2 titrated 24.39 mL
- A Fajans titration of a 0.7908-g sample required 45.32 mL of 0.1046 M AgNO3 . Express the results of this analysis in terms of the percentage of BaCl2 * H2O. (Use a MW value in 4 decimal places)51 mL of 0.060 M NaF is mixed with 17 mL of 0.15 M Sr(NO3)2. Calculate the concentration of F- in the final solution. Assume volumes can be added. (Ksp for SrF2 = 2.0×10-10) 0.038 M 0.0075 M 0.045 M 0.015 M 0.00012 MA 0.045 0 M solution of HA is 0.60% dissociated. Find pKa for HA.
- Calculate the pH at 0, 50 and 100% for the titration of 100.0 mL of 0.05 M CH3NH2 with 0.05 M HCl. Kb (CH3NH2) = 4.35x 10-5 A 1.00-ml aliquot of fish oil was analyzed for N using the Kjeldahl method. After digestion, the distilled ammonia was collected in 100 ml of 0.0503M HCl. The excess HCl required 28.3 ml of 0.124 M NaOH for titration. Calculate the amount of N in the sample of fish oil as mg/mL.Write a balanced net ionic equation to show why the solubility of AlPO4 (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Ksp from textbook: 1.3*10^-20 Ka1 Phosphoric acid: 7.5*10^-3Construct a curve for the titration of 20.00 mL 0.500 N succinic acid (HO2CCH2CH2CO2H) by 0.1000 N NaOH solution. Use MS Excel for convenience. Titrant volumes: 0.00 mL, 5.00 mL, 10.00 mL, 15.00 mL, 20.00 mL, 25.00 mL, and 30.00 mL. (CH2)2(CO2H)2⇄(CH2)2(CO2H)(CO2)^- +H^+ Ka1= 6.21 x 10^-5; pKa1 =4.207 (CH2)2(CO2H)(CO2)^-⇄(CH2)2(CO2)2^2-+ H^+ Ka2= 2.31 x 10^-6; pKa2 =5.636