A worker at your facility is experiencing stomach discomfort. The company’s emergency medical technicians checked
out the worker and recommended that he be transported to their contracted occupational medical facility to be examined by a doctor. The worker was transported by his company safety representative. After examining the patient, the doctor determined that the illness was non-work related, and the doctor prescribed milk of magnesia, also known as magnesium hydroxide (Mg(OH)2), which is available over the counter at local pharmacies. Mg(OH)2, which produces a mild alkaline solution when mixed with water (only slightly soluble), is used to neutralize excess stomach (hydrochloric) acid that causes indigestion.
a. What is the balanced equation for the chemical reaction of magnesium hydroxide and hydrochloric acid?
b. What is the molar mass of milk of magnesia? If 30 grams of hydrochloric acid (molar mass of 36.5 g/mol) needs to be neutralized, how many grams of Mg(OH)2 are required to be ingested (disregard the solubility and dilution of the Mg(OH)2 in aqueous solution)?
c. What is the molarity of the solution (assuming Mg(OH)2 is soluble in aqueous solution), if 10 grams of Mg(OH)2 is dissolved in 150 ml of water?
d. Why is the proper management of potential work related injury and illness cases important?