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Part b and C What volume of 0.110 M HCI is required for the complete neutralization of 1.10 g of Na2 CO3 (sodium carbonate)? Express your answer to three significant figures and include the appropriate units. A sample of NaOH (sodium hydroxide) contains a small amount of Na2 CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.110 g of this sample requires 23.98 mL of 0.100 M HCI. Ar additional 0.700 mL of 0.100 M HCI is required to reach the methyl orange endpoint. What is the percentage of NaCO; by mass in the sample? Express your answer to three significant figures and include the appropriate units.

Part b and C What volume of 0.110 M HCI is required for the complete neutralization of 1.10 g of Na2 CO3 (sodium carbonate)? Express your answer to three significant figures and include the appropriate units. A sample of NaOH (sodium hydroxide) contains a small amount of Na2 CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.110 g of this sample requires 23.98 mL of 0.100 M HCI. Ar additional 0.700 mL of 0.100 M HCI is required to reach the methyl orange endpoint. What is the percentage of NaCO; by mass in the sample? Express your answer to three significant figures and include the appropriate units.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section: Chapter Questions
Problem 27PS: Phenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water...
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Part b and C What volume of 0.110 M HCI is required for the complete neutralization of 1.10 g of Na2 CO3 (sodium carbonate)? Express your answer to three significant figures and include the appropriate units. A sample of NaOH (sodium hydroxide) contains a small amount of Na2 CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.110 g of this sample requires 23.98 mL of 0.100 M HCI. Ar additional 0.700 mL of 0.100 M HCI is required to reach the methyl orange endpoint. What is the percentage of NaCO; by mass in the sample? Express your answer to three significant figures and include the appropriate units.
Carbonic acid (H₂CO3) is a weak diprotic acid with Kal = 4.43 x 10-7 and Ka2 = 4.73 x 10-¹1. When sodium bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it acts as a weak base according to the equation NaHCO3(aq) + HCl(aq) →H₂CO3(aq) + NaCl(aq) Suitable indicators are those that change color within the pH range for the equivalence point of a specific titration. The expected pH at the equivalence point can be calculated using pKa values. Suitable indicators for use in titrating carbonic acid or carbonate solutions are methyl orange and phenolphthalein. Part B What volume of 0.110 MHCl is required for the complete neutralization of 1.10 g of Na2CO3 (sodium carbonate)? Express your answer to three significant figures and include the appropriate units. ▾ View Available Hint(s) ▶ Hint 1. Identify the mole ratio at the equivalence point Hint 2. Determine the amount of sodium carbonate present Hint 3. Complete previous hint(s)
Transcribed Image Text:Carbonic acid (H₂CO3) is a weak diprotic acid with Kal = 4.43 x 10-7 and Ka2 = 4.73 x 10-¹1. When sodium bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it acts as a weak base according to the equation NaHCO3(aq) + HCl(aq) →H₂CO3(aq) + NaCl(aq) Suitable indicators are those that change color within the pH range for the equivalence point of a specific titration. The expected pH at the equivalence point can be calculated using pKa values. Suitable indicators for use in titrating carbonic acid or carbonate solutions are methyl orange and phenolphthalein. Part B What volume of 0.110 MHCl is required for the complete neutralization of 1.10 g of Na2CO3 (sodium carbonate)? Express your answer to three significant figures and include the appropriate units. ▾ View Available Hint(s) ▶ Hint 1. Identify the mole ratio at the equivalence point Hint 2. Determine the amount of sodium carbonate present Hint 3. Complete previous hint(s)
Carbonic acid (H₂CO3) is a weak diprotic acid with Kal = 4.43 x 10-7 and Ka2 = 4.73 x 10-¹¹. When sodium bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it acts as a weak base according to the equation NaHCO3(aq) + HCl(aq) →H₂CO3(aq) + NaCl(aq) Suitable indicators are those that change color within the pH range for the equivalence point of a specific titration. The expected pH at the equivalence point can be calculated using pKa values. Suitable indicators for use in titrating carbonic acid or carbonate solutions are methyl orange and phenolphthalein. A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.110 g of this sample requires 23.98 mL of 0.100 M HCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample? Express your answer to three significant figures and include the appropriate units. ▾ View Available Hint(s) Hint 1. How to approach the problem The phenolphthalein endpoint of the titration occurs when the HCI has neutralized all of the NaOH in the sample. Additional HCl is then needed to neutralize the Na2CO3 and reach the methyl orange endpoint. The amount of HCl needed to get from the first to the second endpoint will allow you to determine the mass of Na₂CO3 in the sample. The percentage by mass of any component is a ratio of the mass of that component to the total mass of the sample, as shown in the equation percentage of Na₂CO3 = The total mass of the sample is given in the problem mass of Na₂CO3 mass of sample as 0.110 g. x 100%
Transcribed Image Text:Carbonic acid (H₂CO3) is a weak diprotic acid with Kal = 4.43 x 10-7 and Ka2 = 4.73 x 10-¹¹. When sodium bicarbonate (NaHCO3) is titrated with hydrochloric acid (HCl), it acts as a weak base according to the equation NaHCO3(aq) + HCl(aq) →H₂CO3(aq) + NaCl(aq) Suitable indicators are those that change color within the pH range for the equivalence point of a specific titration. The expected pH at the equivalence point can be calculated using pKa values. Suitable indicators for use in titrating carbonic acid or carbonate solutions are methyl orange and phenolphthalein. A sample of NaOH (sodium hydroxide) contains a small amount of Na2CO3 (sodium carbonate). For titration to the phenolphthalein endpoint, 0.110 g of this sample requires 23.98 mL of 0.100 M HCl. An additional 0.700 mL of 0.100 M HCl is required to reach the methyl orange endpoint. What is the percentage of Na2CO3 by mass in the sample? Express your answer to three significant figures and include the appropriate units. ▾ View Available Hint(s) Hint 1. How to approach the problem The phenolphthalein endpoint of the titration occurs when the HCI has neutralized all of the NaOH in the sample. Additional HCl is then needed to neutralize the Na2CO3 and reach the methyl orange endpoint. The amount of HCl needed to get from the first to the second endpoint will allow you to determine the mass of Na₂CO3 in the sample. The percentage by mass of any component is a ratio of the mass of that component to the total mass of the sample, as shown in the equation percentage of Na₂CO3 = The total mass of the sample is given in the problem mass of Na₂CO3 mass of sample as 0.110 g. x 100%
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