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12 Dec 2019

Question 3 (8 marks) Borax (Na2B4O7·10H2O, MW 381.367) can be used to standardise HNO3. Titration of 0.2347 g borax required 19.25 mL HNO3 solution. What is the molarity of the nitric acid solution? Borax reacts in the following way: B4O72- + 2 H+ + 5H2O → 4B(OH)3

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Trinidad Tremblay
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13 Dec 2019

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Related questions

Using the following information, calculate the number of moles of HCl, Moles of Borate, Concentration of Borate, Ksp, Average Ksp, ΔG (kJ/mol), ΔH (kJ/mol), and ΔS (J/mol*K):

Na2B4O7 • 10H2O(s) -><- 2Na+(aq) + B4O5(OH)42−(aq) + 8H2O(l)

Titration: B4O5(OH)42-(aq) + 2HCl(aq) + 3H2O(l) → 4 B(OH)3(aq) + 2 Cl− (aq)

Molar Mass of B: 10.81g/mol, Molar Mass of O: 16.00g/mol, Molar Mass of H: 1.008g/mol, Molar Mass of Cl: 35.45g/mol

K = [Na+]2 [B4O5(OH)42-]

Ksp = 4 [B4O5(OH)42-]3

ΔG = −RT ln Ksp

ΔG = ΔH – TΔS

−RT ln Ksp = = ΔH – TΔS

a)Titration 1: Temperature: 28.0 degrees C, Concentration of HCl: 0.251 M, Volume of Borax solution (mL): 5.00, Volume of HCl titrated: 2.00 mL

Please do not post the lab that this question comes from because it is hard for me to understand. Please show each individual step and use units along the way to the answer. Thanks!

Nitric acid (HNO3), a strong acid, is formed in the following reaction.

2 NO(g) + 3/2 O2(g) + H2O(g) → 2 HNO3(g).

Assume a volume of 22.4 mL of NO gas (at STP = 1 atm, 273 K) completely reacts with
excess of oxygen and water. If all of the acid that is formed is dissolved into 50. mL of
water, what should be the pH of the solution? (pH = - log[H+])?
A) 1.0
B) 1.7
C) 2.0
D) 3.0
E) 2.3

1. Let’s separate the different data pieces of the HNO3 solution into solute, solvent and solution. Using the density of nitric acid solution (1.09 g/mL) and the molarity you calculated above (0.1532M) and the volume used (14.92ml), calculate the following in the table below.

Volume of original nitric acid solution: _______________

Grams & Moles of Nitric Acid? ___________________

Grams of Water? ________________

Total Solution? __________________

In another titration, a student uses 1.023 M HCl solution to standardize a sodium hydroxide solution. Assuming 1.00 L of HCl solution and its density of 1.02 g/mL, calculate the mass percent and molality of the HCl solution.

mass percent:_________________

molality: ___________________

3. Draw the expanded structure of ethanoic acid (acetic acid) in the provided box.

4. What is the solute in the vinegar solution?

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