Homework Answers
During titration of phosphoric acid, after just boiling the sample, it is kept as such for 5-10 minutes. This helps in expelling the carbon dioxide which otherwise interferes with the titration.
CO2 (g) + H2O (l) -----> H2CO3 (aq)
Carbon dioxide causes interference as it dissolves in water to produce carbonic acid which influences the end-point of acid-base titrations. The large amount of carbon dioxide in sample increases its acidity with time causing fading of pink color as the time passes by. This may lead to addition of more amount of titrant. A little amount added will influence the end-point result.
To prevent this solvents muct be kept covered. The complete absence of carbon dioxide can be confirmed by using an indicator such as phenolphthalein.
Consider the titration of 100mL of 0.296M H3PO4 with 2.39M NaOH. How many mL base will...
Consider the titration of 100mL of 0.296M H3PO4 with 2.39M NaOH. How many mL base will be needed for the weak acid to have a charge of -1? mL of base=
Calculate the Ka before adding the titrant (NaOH). Titration experiment between NaOH and H3PO4. B...
Calculate the Ka before adding the titrant (NaOH). Titration experiment between NaOH and H3PO4. Before adding the NaOH, the pH of the 10.00mL 0.15M H3PO4 and 20.0 mL DI water solution was 1.75. I'm stuck on how to calculate the Ka.
2. Balance the following equations: C5H12+ O2CO2 H20 Al2(CO3)3 + H3PO4 - AIPO4 CO2+H20o Ca(OH)2 +...
2. Balance the following equations: C5H12+ O2CO2 H20 Al2(CO3)3 + H3PO4 - AIPO4 CO2+H20o Ca(OH)2 + H3PO4 --> Ca3 (PO4)2 + H20 C2H6 + 02 -CO2+H20
In the titration of 250.0 mL of 0.20 M H3PO4 with 0.10 M NaOH, the pH...
In the titration of 250.0 mL of 0.20 M H3PO4 with 0.10 M NaOH, the pH of the solution after the addition of some NaOH is 4.66. Which of the following phosphate-containing species is present in the largest amount? For H3PO4, Ka1 = 7.5 × 10–3, Ka2 = 6.2 × 10–8, and Ka3 = 4.8 × 10–13.
Calculate the Ka before adding the titrant (NaOH). Titration experiment between NaOH and H3PO4. Before adding...
Calculate the Ka before adding the titrant (NaOH). Titration experiment between NaOH and H3PO4. Before adding the NaOH, the pH of the 10.00mL 0.15M H3PO4 and 20.0 mL DI water solution was 1.75. I'm stuck on how to calculate the Ka.
Table I. Summary of Titration Data for H3PO4 Acid Titration Point Volume of NaOH added 0.00...
Table I. Summary of Titration Data for H3PO4 Acid Titration Point Volume of NaOH added 0.00 2.60 5.20 7.40 8.60 pH 2.22 2.38 Initial First Eq. Pt. First Eq. Pt. Second 2 Eq. Pt. Second Eq. Pt.4.64 2.80 3.17
- n an acid-bade titration, 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL...
- n an acid-bade titration, 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 M KOH solution. What is the concentration of the H3PO4 solution (in M)? (3pts)
Calculating Ka from titration curve. We titrated H3PO4 with NaOH. We began with 40.0 mL 0.0970...
Calculating Ka from titration curve. We titrated H3PO4 with NaOH. We began with 40.0 mL 0.0970 MH3PO4, titrated with 0.2085 M NaOH. We reached first equivalence at 18.78 mL NaOH titrated, and second equivalence at 38.50 mL titrated. Calculate Ka1 for H3PO4 using the following data obtained from a titration curve: 1) From the initial pH = 1.97 2) From the pH value half way to the first equivalence point = 2.10 Calculate Ka2 for H3PO4 from the following data...
In a strong base/weak acid titration: titrant: NaOH analyte: H3PO4 solution There should be three equivalence...
In a strong base/weak acid titration: titrant: NaOH analyte: H3PO4 solution There should be three equivalence points since there are three protons transferred...why does my titration curve only show two?
Consider the titration of 100.0 mL of 0.0200 M H3PO4 with 0.121 M NaOH. Calculate the...
Consider the titration of 100.0 mL of 0.0200 M H3PO4 with 0.121 M NaOH. Calculate the milliliters of base that must be added to reach the first, second, and third equivalence points.
2. Balance the following equations: C5H12+ O2CO2 H20 Al2(CO3)3 + H3PO4 - AIPO4 CO2+H20o Ca(OH)2 + H3PO4 --> Ca3 (PO4)2 + H20 C2H6 + 02 -CO2+H20
Table I. Summary of Titration Data for H3PO4 Acid Titration Point Volume of NaOH added 0.00 2.60 5.20 7.40 8.60 pH 2.22 2.38 Initial First Eq. Pt. First Eq. Pt. Second 2 Eq. Pt. Second Eq. Pt.4.64 2.80 3.17
- n an acid-bade titration, 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 M KOH solution. What is the concentration of the H3PO4 solution (in M)? (3pts)
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