Calcium carbonate is a common ingredient in antacids that reduces the discomfort associated with acidic stomach or heartburn. Stomach acid is hydrocholoric acid, HCl.HCl.
What volume in milliliters (mL) of an HClHCl solution with a pH of 1.581.58 can be neutralized by 20.0 mg20.0 mg of CaCO3?
If the stomach contains 24.3 mL24.3 mL of pH 1.58pH 1.58 solution, will all of the acid be neutralized?
yes
no
What percentage of the acid is neutralized? If all of the acid is neutralized enter 100%.
Answer:-
This question is solved by using the simple concept of stoichiometry. Firstly a balanced chemical equation is written then volume is calculated.
The answer is given in the image,
Calcium carbonate is a common ingredient in antacids that reduces the discomfort associated with acidic stomach...
Calcium carbonate is a common ingredient in antacids that reduces the discomfort associated with acidic stomach or heartburn. Stomach acid is hydrocholoric acid, HCI. What volume in milliliters (mL) of an HCl solution with a pH of 1.71 can be neutralized by 29.0 mg of CaCO,? volume: mL If the stomach contains 45.0 mL of pH 1.71 solution, will all of the acid be neutralized? O yes no What percentage of the acid is neutralized? If all of the acid...
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?
Calcium carbonate is used in many antacids to neutralize stomach acid, as depicted by the following chemical equation: CaCO3(s) + 2 HCl(aq) → CaCl2 + H2O(l) + CO2(g) If 250. mg of calcium carbonate reacts with 5.64 g of hydrochloric acid, how much hydrochloric acid will remain? Provide your answer in g.
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Calcium carbonate, CaCO3, reacts with stomach acid, (HCI, hydrochloric acid) according to the following equation: CaCO3(s) + 2HCl(aq)-CO2(g) + H2O(1) +CaCl2(aq) Tums, an antacid, contains CaCO3. If Tums is added to 20.0 mL of a 0.400 M HCl solution, how many grams of CO2 gas are produced?
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A common base found at home is milk of magnesia (antacids are bases). The active ingredient of milk of magnesia is magnesium hydroxide, a weak base. Magnesium hydroxide is used to neutralize excess stomach acid which is primarily HCl. How much HCl (in mg) could be neutralized from a normal dose of milk of magnesia if that dose contains 400 mg of Mg(OH)2? The correct answer is 500 mg but could you show your work so i understand how to...
Calcium carbonate (CaCO3) reacts with stomach acid (HCl, hydrochloric acid) according to the following equation: CaCO3(s) + 2HCl(aq) + CO2(g) + H2O(l) + CaCl2(aq) A typical antacid contains CaCO3. If such an antacid is added to 25.0 mL of a solution that is 0.300 M in HCl, how many grams of CO2 gas are produced? Express the mass to three significant figures and include the appropriate units. TI MÃ + + + a ? Value Units MCO: = Submit Previous...
Calcium carbonate (CaCO3) reacts with stomach acid (HCl, hydrochloric acid) according to the following equation: CaCO3(s)+2HCl(aq)⟶CO2(g)+H2O(l)+CaCl2(aq) Tums, an antacid, contains CaCO3. If Tums is added to 10.0 mL of a solution that is 0.400 M in HCl, how many grams of CO2 gas are produced?
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