23. Milk of magnesia is often used as an antacid to neutralize acid stomach. It has...
milk of magnesia is a common liquid antacid that contains magnesium hydroxide. since magnesium hydroxide isnt highly soluble in water milk of magnesia is sold as a suspension (thick liquid) where the solute isnt dissolve it stays as a small solid particles homogeneously mixed throughout the liquid; it is estimated that 1.00 ml of milk of magnesia contains 80.0 mg of magnesium hydroxide . assuming that our stomach acid has a concentration of 0.166M HCL how much milk of magnesia...
Integrated Problems #13 Milk of magnesia (Mg(OH)2)is often taken to reduce the discomfort associated with acid stomach or heartburn. The recommended dose is 1 teaspoon (5 mL) which contains 4.00 X 10-mg of Mg(OH)2. 1) Magnesium hydroxide is a slightly soluble salt. Write a balanced equilibrium reaction for this process. 2) The Ksp for Magnesium hydroxide is 2.06 X 10-13, what is the pH of the recommended dose of milk of magnesia? 3) If we assume that stomach acid is...
Milk of magnesia, an over-the-counter antacid liquid, is a suspension of magnesium hydroxide in water. It neutralizes the hydrochloric acid in the stomach to alleviate some stomach symptoms associated with excess acid. In a laboratory, 1.11 g Mg(OH)2 is added to 231.8 mL of 0.1731 M HCl in water. They react according to the following equation. Mg(OH)2 + 2 HCl → MgCl2 + 2 H2O (a) What is the limiting reagent in this reaction? (b) How much magnesium chloride is...
"Milk of magnesia" antacid has a pH of 10.25. What is the [H+] in this solution? A. 5.6 × 10-11 B. 1.8 × 1011 C. 1.8 × 10-4 D. 3.75 E. 1.8
Antacids are used to neutralize excessive hydrochloric acid (HCl) that may be present in the stomach during digestive process. Milk of Magnesia is a common over the counter medication used to neutralize the HCI excess, the base present in Milk of Magnesia is called magnesium hydroxide (Mg(OH)_2). Tell which of the compounds (HCI or Mg(OH)_2) is an ionic compound, and which compound is a covalent compound. Next, explain in a very clear way how you conclude which compound is ionic...
Magnesium hydroxide, the active ingredient in milk of magnesia, neutralizes stomach acid, primarily HCl, according to the reaction Mg(OH)2 (aq) + 2HCl(aq) + 2H2O(1) + MgCl2 (aq) What mass of HCl, in grams, is neutralized by a dose of milk of magnesia containing 3.26 g of Mg(OH)2 ? Express the mass in grams to three significant figures. IVO ADD + R o 2 ? mass of HCl = g Submit Request Answer
An average human has about 1.64 L of 0.157 M HCl in the stomach. At some point, you might have acid reflux and consumed an antacid such as milk of magnesia as the active ingredient at a concentration of about 1.317 M. How much milk of magnesia would you need to consume in ml if you wanted to neutralize all of the stomach acids? 2HCl(aq)+Mg(OH)2(aq)>2H2O(l)+MgCl2(aq)
Milk of magnesia is often taken to reduce the discomfort associated with heartburn. The recommended dose is one teaspoon, which contains 165 mg of Mg(OH)2. If the stomach contains 354 mL of pH 1.3 solution, what percent of the acid will be neutralized?
Magnesium hydroxide, the active ingredient in milk of magnesia, neutralizes stomach acid, primarily HCl, according to the reaction Mg(OH)2(aq) + 2HCl(aq) + 2H2O(1) + MgCl2(aq) What mass of HCI, in grams, is neutralized by a dose of milk of magnesia containing 3.26 g of Mg(OH)2? The balanced chemical equation for the combustion of propane is C3H3(g) + 502(g) +3CO2(g) + 4H2O(g) Which statement is correct about the complete combustion of 3.00 mole of propane, C3H8?
7) Magnesium hydroxide, Mg(OH)2, as "Milk of Magnesia" can be used to neutralize excess stomach acid, represented by HCl(ag) according to the chemical equation below. Mg(OH)2(s)+2HCI (ag)-MgCl2(ag)+ 2H20( When 5.00 g of HCl are combined with an excess of Mg(OH)2, what mass of MgCl2 can be produced? [Molar masses: H, 1.01 g/mol; O, 16.00 g/mol; Mg, 24.31 g/mol; Cl, 35.45 g/mol] A) 2.50 g E) 70.5 g D) 6.53 g C) 0.957 g B) 13.1 g 8) What is the...