1. A student who is performing this experiment pours an 8.50 mL sample of the saturated...

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1. A student who is performing this experiment pours an 8.50 mL sample of the saturated borax solution into a test tube after the borax solution. The student rinses the sample into a small beaker using distilled water, and then titrates the solution with a 0.550 M HCI solution. The student finds that 12.00 mL of the HCI solution is needed to reach the endpoint of the titration. Calculate the value of Ksp for borax. Here is a suggested procedure for doing this calculation: (a) (b) (C) (d) Calculate the number of moles of HCI that were added during the titration. Use reaction 2 in the lab manual to relate the number of moles of HCI to the number of moles of B4O5(OH)4 2- in the 8.50 mL sample. Calculate the concentration of B4O5(OH)4 2 in the 8.50 mL sample. Use equation 5 in the lab manual to calculate the equilibrium constant (Ksp). 1. A student who is performing this experiment pours an 8.50 mL sample of the saturated borax solution into a test tube after the borax solution. The student rinses the sample into a small beaker using distilled water, and then titrates the solution with a 0.550 M HCI solution. The student finds that 12.00 mL of the HCI solution is needed to reach the endpoint of the titration. Calculate the value of Ksp for borax. Here is a suggested procedure for doing this calculation: (a) (b) (C) (d) Calculate the number of moles of HCI that were added during the titration. Use reaction 2 in the lab manual to relate the number of moles of HCI to the number of moles of B4O5(OH)4 2- in the 8.50 mL sample. Calculate the concentration of B4O5(OH)4 2 in the 8.50 mL sample. Use equation 5 in the lab manual to calculate the equilibrium constant (Ksp).