Question

Experiment TA Lab Team Members Finding Equilibrium Constants: The Solubility of Borax Report Sheet Part A: Titration of Room Temperature Borax: Kg Molarity of Standard HCl solution: 004 u Temperature of room temperature borate mixture (T); T. in 20.00 Tin 293.15 K Trial 1 LLLLLL Final buret reading HCl, mL Initial buret reading HCI, ml 135.26 12.40 110.48 11.052 Trial 3 Trial 2 (if done) 138.53 39.00 18.83 18.76 110.66 110. 36 1.000 1.040 Volume of HCl used in Titration, mL Moles HCI Moles Borate Molarity of Borate Molarity of Na Ki Average of Borax:

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Answer 1

Here is the Solution:

* Molarity of Standard HCl solutions 0.1004 M. Na2B4O7 • 10 H₂O + 2HCl - 2NaCl + H₂B4Oz + 10 H₂O Here 1 mol of borax reacts with a moles of HCL. · Average volume of HCl used (10.48 + 10.66 + 10.36 ml = 10.5 mL = 0.0105 L - Moles HCl = 2 moles borate = 0.1004 mol/xx 0.01056 = 0.001054 moles. 0.001054 mol = 0.000527 mol - 0.010L Molarity borate?= 0.000527 mol I =0.0 527 M * Molarity Nat = ax 0.0527 m = 0.1054 m Akspy = [Nat]². [ B40227 Ksp. = (0.105402 x (0.0527) Ksp = 0.000585 (Average), "Note: All above method calculations are for calculating average, use the same trial -1, trial 2 and trial-3.

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