A 1.00g sample containing benzoic acid and gallic acid is titrated. Benzoic acid has MM=122g/mol and...
A 1.00g sample containing benzoic acid and gallic acid is titrated. Benzoic acid has MM=122g/mol and has 1 acidic hydrogen. Gallic aciid has MM=170g/mol and has 1 acidic hydrogen. The acid mixtures is dissolved and titrated with 0.500M NaOH solution. To reach the end point in the titration a total volume of 14.7mL of base was needed. What is the mass percent of benzoic and gallic acid?
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A 1.00g sample containing benzoic acid and gallic acid is
titrated. Benzoic acid has MM=122g/mol and...
3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water...
3. 0.7253 g sample containing an unknown weak acid HA was dissolved in 50 mL water and titrated against 0.1555 M NaOH, requiring 48.11 mL to of NaOH to reach the end-point. During the titration reaction, the pH of the solution is 3.77 when half of the HA is neutralized and the equivalence-point pH is 8.33. (a) State two ways to standardize the NaOH used in the titration. (b) Suggest and explain an indicator that can be used in the...
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A 0.258-g sample of a pure triprotic acid, H3A, (where A is the generic anion of...
A 0.258-g sample of a pure triprotic acid, H3A,
(where A is the generic anion of the acid), was dissolved in water
and titrated with 0.150 M barium hydroxide solution. The titration
required 13.9 mL of the base to reach the equivalence point. What
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Question 25 3.5 pts A 0.258-g sample of a pure triprotic acid, H3A, (where A is the generic anion of the acid), was dissolved in water and titrated...
| A 0.458 g sample of a diprotic acid is dissolved in water and titrated with...
| A 0.458 g sample of a diprotic acid is dissolved in water and titrated with 0.170 M NaOH. What is the molar mass of the acid if 37.4 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: g/mol
1.) 20.00 mL of 0.11 M benzoic acid (C6H5COOH, Ka = 6.3x10-5) is titrated with 0.25...
1.) 20.00 mL of 0.11 M benzoic acid (C6H5COOH, Ka = 6.3x10-5) is titrated with 0.25 M NaOH. What volume of base is required to reach the equivalence point in the titration? 2.) Calculate pH at each of the following points in the titration. a) 4.00 mL b) 8.80 mL
A 0.541 g sample of a diprotic acid is dissolved in water and titrated with 0.160...
A 0.541 g sample of a diprotic acid is dissolved in water and
titrated with 0.160 M NaOH. What is the molar mass of the acid if
30.6 mL of the NaOH solution is required to neutralize the sample?
Assume the volume of NaOH corresponds to the second equivalence
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A 0.521 g sample of a diprotic acid is dissolved in water and titrated with 0.160...
A 0.521 g sample of a diprotic acid is dissolved in water and titrated with 0.160 M NaOH. What is the molar mass of the acid if 40.4 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: g/mol
A 0.401 g sample of a diprotic acid is dissolved in water and titrated with 0.130...
A 0.401 g sample of a diprotic acid is dissolved in water and titrated with 0.130 M NaOH. What is the molar mass of the acid if 31.3 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: g/mol
A 0.824 g sample of a diprotic acid is dissolved in water and titrated with 0.200...
A 0.824 g sample of a diprotic acid is dissolved in water and titrated with 0.200 M NaOH. What is the molar mass of the acid if 37.2 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: g/mol
A 0.334 g sample of a diprotic acid is dissolved in water and titrated with 0.120...
A 0.334 g sample of a diprotic acid is dissolved in water and titrated with 0.120 M NaOH. What is the molar mass of the acid if 30.5 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: 91.25 g/mol
A 0.258-g sample of a pure triprotic acid, H3A,
(where A is the generic anion of the acid), was dissolved in water
and titrated with 0.150 M barium hydroxide solution. The titration
required 13.9 mL of the base to reach the equivalence point. What
is the molar mass of the acid ?
Question 25 3.5 pts A 0.258-g sample of a pure triprotic acid, H3A, (where A is the generic anion of the acid), was dissolved in water and titrated...
| A 0.458 g sample of a diprotic acid is dissolved in water and titrated with 0.170 M NaOH. What is the molar mass of the acid if 37.4 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: g/mol
A 0.541 g sample of a diprotic acid is dissolved in water and
titrated with 0.160 M NaOH. What is the molar mass of the acid if
30.6 mL of the NaOH solution is required to neutralize the sample?
Assume the volume of NaOH corresponds to the second equivalence
point.
molar mass: _____ g/mol
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A 0.401 g sample of a diprotic acid is dissolved in water and titrated with 0.130 M NaOH. What is the molar mass of the acid if 31.3 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: g/mol
A 0.824 g sample of a diprotic acid is dissolved in water and titrated with 0.200 M NaOH. What is the molar mass of the acid if 37.2 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: g/mol
A 0.334 g sample of a diprotic acid is dissolved in water and titrated with 0.120 M NaOH. What is the molar mass of the acid if 30.5 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. molar mass: 91.25 g/mol
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