Calculations: Standardization of HCl Titrating Solution: Using your best two or three standardization titrations, calculate the concentration of the HCl titrating solution for each trial using the balanced equation between HCl and Na2CO3. What is the average concentration of your HCl solution? Ksp Determination at both temperatures Calculate the room temperature Ksp for borax. From the HCl volume used in each titration, calculate the concentration of borate in each room temperature aliquot using the equation between HCl and borate From the stoichiometric relationship between borate and sodium ion, calculate [Na+ ] in each aliquot. Calculate the room temperature Ksp for each titration using the following equation calculate the average Ksp value. Ice Bath Temperature Ksp Determination: Calculate Ksp for borax as you did for the room temperature system. Calculate the concentration of borate in each ice temperature aliquot. Calculate [Na+ ] for each ice temperature aliquot. Calculate each ice temperature Ksp and the average Ksp value. ΔHº Determination: Dissolving borax in water is an endothermic process shown by the equation: heat + borax (s) ↔ 2 Na+(aq) + borate (aq) + 8 H2O (l) Evaluate ΔH° for the dissolving of borax using the following equation, where Ksp2 is the borax solubility product at room temperature and T2 is room temperature in Kelvins, Ksp1 is the borax solubility product at ice temperature and T1 is the temperature of the borate solution in the ice-water bath. R = 8.314 J/mol·K. ΔGº Determination: Calculate ΔG° for each of the two temperatures using the equation: ΔSº Determination Calculate the entropy changes at the two temperatures using the equation: Discussion Discuss the relationship between enthalpy change and the solubility product Ksp. Standardisation of HCl – Titration results Trial I Trial II Mass of Na2CO3 (g) 0.15 0.17 Moles of Na2CO3 Moles of HCl used (from equation) Final mL of HCl 26 53 Initial mL of HCl 0 26 mL of HCl used (titre value) Molarity of HCl Ksp of Borax at room temperature (298 K) Titration with HCl: Trial I Trial II Final mL of HCl 14 30 Initial mL of HCl 0 14 mL of HCl used (titre value) Ksp of Borax (ice bath, 273 K) Titration with HCl: Trial I Trial II Final mL of HCl 5.6 9.9 Initial mL of HCl 0 5.6 mL of HCl used (titre value)

Calculations: Standardization of HCl Titrating Solution: Using your best two or three standardization titrations, calculate the concentration of the HCl titrating solution for each trial using the balanced equation between HCl and Na2CO3. What is the average concentration of your HCl solution? Ksp Determination at both temperatures Calculate the room temperature Ksp for borax. From the HCl volume used in each titration, calculate the concentration of borate in each room temperature aliquot using the equation between HCl and borate From the stoichiometric relationship between borate and sodium ion, calculate [Na+ ] in each aliquot. Calculate the room temperature Ksp for each titration using the following equation calculate the average Ksp value. Ice Bath Temperature Ksp Determination: Calculate Ksp for borax as you did for the room temperature system. Calculate the concentration of borate in each ice temperature aliquot. Calculate [Na+ ] for each ice temperature aliquot. Calculate each ice temperature Ksp and the average Ksp value. ΔHº Determination: Dissolving borax in water is an endothermic process shown by the equation: heat + borax (s) ↔ 2 Na+(aq) + borate (aq) + 8 H2O (l) Evaluate ΔH° for the dissolving of borax using the following equation, where Ksp2 is the borax solubility product at room temperature and T2 is room temperature in Kelvins, Ksp1 is the borax solubility product at ice temperature and T1 is the temperature of the borate solution in the ice-water bath. R = 8.314 J/mol·K. ΔGº Determination: Calculate ΔG° for each of the two temperatures using the equation: ΔSº Determination Calculate the entropy changes at the two temperatures using the equation: Discussion Discuss the relationship between enthalpy change and the solubility product Ksp. Standardisation of HCl – Titration results Trial I Trial II Mass of Na2CO3 (g) 0.15 0.17 Moles of Na2CO3 Moles of HCl used (from equation) Final mL of HCl 26 53 Initial mL of HCl 0 26 mL of HCl used (titre value) Molarity of HCl Ksp of Borax at room temperature (298 K) Titration with HCl: Trial I Trial II Final mL of HCl 14 30 Initial mL of HCl 0 14 mL of HCl used (titre value) Ksp of Borax (ice bath, 273 K) Titration with HCl: Trial I Trial II Final mL of HCl 5.6 9.9 Initial mL of HCl 0 5.6 mL of HCl used (titre value)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Calculations:

Standardization of HCl Titrating Solution: Using your best two or three standardization titrations, calculate the concentration of the HCl titrating solution for each trial using the balanced equation between HCl and Na₂CO₃.

What is the average concentration of your HCl solution?

Ksp Determination at both temperatures

Calculate the room temperature Ksp for borax.

From the HCl volume used in each titration, calculate the concentration of borate in each room temperature aliquot using the equation between HCl and borate
From the stoichiometric relationship between borate and sodium ion, calculate [Na+ ] in each aliquot.
Calculate the room temperature Ksp for each titration using the following equation calculate the average Ksp value.

Ice Bath Temperature Ksp Determination:

Calculate Ksp for borax as you did for the room temperature system.
Calculate the concentration of borate in each ice temperature aliquot.
Calculate [Na+ ] for each ice temperature aliquot.
Calculate each ice temperature Ksp and the average Ksp value.

ΔHº Determination: Dissolving borax in water is an endothermic process shown by the equation: heat + borax (s) ↔ 2 Na+(aq) + borate (aq) + 8 H2O (l)
Evaluate ΔH° for the dissolving of borax using the following equation, where Ksp2 is the borax solubility product at room temperature and T2 is room temperature in Kelvins, Ksp1 is the borax solubility product at ice temperature and T1 is the temperature of the borate solution in the ice-water bath. R = 8.314 J/mol·K.
ΔGº Determination: Calculate ΔG° for each of the two temperatures using the equation:

ΔSº Determination Calculate the entropy changes at the two temperatures using the equation:

Discussion

Discuss the relationship between enthalpy change and the solubility product Ksp.

Standardisation of HCl – Titration results

	Trial I	Trial II
Mass of Na₂CO₃ (g)	0.15	0.17
Moles of Na2CO3
Moles of HCl used (from equation)
Final mL of HCl	26	53
Initial mL of HCl	0	26
mL of HCl used (titre value)
Molarity of HCl

Ksp of Borax at room temperature (298 K)

Titration with HCl:

	Trial I	Trial II
Final mL of HCl	14	30
Initial mL of HCl	0	14
mL of HCl used (titre value)

Ksp of Borax (ice bath, 273 K)

Titration with HCl:

	Trial I	Trial II
Final mL of HCl	5.6	9.9
Initial mL of HCl	0	5.6
mL of HCl used (titre value)

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