Question: At a certain temperature, a 10.00 mL sample of liquid from a saturated solution of sodium tetraborate is completely neutralized by with 33.0 mL of

At a certain temperature, a 10.00 mL sample of liquid from a saturated solution of sodium tetraborate is completely neutralized by with 33.0 mL of a 0.0500 M HCL solution. Calculate the concentration of borate ions,B4O5(OH)4-2, in the 10.0 mL sample and calculate also for the salt.

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To solve this problem we need to understand the stoichiometry of the reaction between the borate ions and the hydrochloric acid Step 1 Write the balanced chemical equation The reaction between sodium tetraborate commonly written as Na2B4O710H2O or borax with hydrochloric acid can be represented as textB4textO5textOH42 2textHCl ightarrow 4textH3textBO3 2textCl Here textB4textO5textOH42 is the anion present in the solution and each molecule of borate ion ... View full answer

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