A certain dose of Tums contains 750.0 mg of calcium carbonate, CACO,, in each tablet. In this problem, you will follow the steps to calculate how many grams of stomach acid, HCI, are neutralized by one tablet of Tums. Balance the chemical equation for the reaction of HCl with CaCO,. chemical equation: HCI + CaCO, CaCl, + CO, + H,0 Using the balanced equation, determine how many moles of HCI will react with 1 mol of CaCO,. moles of HCl: mol Calculate how many moles 750.0 mg CaCO, is. 750.0 mg CaCO, = mol CaCO, Using your answers from the first two questions, calculate how many moles of HCI are neutralized when 750.0 mg CACO, reacts. moles of HCI: mol

A certain dose of Tums contains 750.0 mg of calcium carbonate, CACO,, in each tablet. In this problem, you will follow the steps to calculate how many grams of stomach acid, HCI, are neutralized by one tablet of Tums. Balance the chemical equation for the reaction of HCl with CaCO,. chemical equation: HCI + CaCO, CaCl, + CO, + H,0 Using the balanced equation, determine how many moles of HCI will react with 1 mol of CaCO,. moles of HCl: mol Calculate how many moles 750.0 mg CaCO, is. 750.0 mg CaCO, = mol CaCO, Using your answers from the first two questions, calculate how many moles of HCI are neutralized when 750.0 mg CACO, reacts. moles of HCI: mol

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 98AP

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Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the unbalanced chemical equation for this process.
Many over-the-counter antacid tablets are now formulated using calcium carbonate as die active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting die stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a burp). Write die balanced chemical equation for this process.
3.94 Calcium carbonate (limestone, CaCO3) dissolves in hydrochloric acid, producing water and carbon dioxide. An unbalanced net ionic equation for this reaction is given below. Balance it. CaCO3(s)+H3O+(aq)H2O(l)+CO2(g)+Ca2+(aq)
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Ammonia can be formed from a combination reaction of its elements. A small fraction of an unreacted mixture of elements is illustrated in the following diagram, in which white spheres represent hydrogen atoms and blue spheres represent nitrogen atoms. The temperature is such that all species are gases. a Write and balance the equation for the reaction. b Which of the following correctly represents the product mixture? c Which species is the limiting reactant? Explain.
The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
A possible practical way to eliminate oxides of nitrogen(such as NO2 ) from automobile exhaust gases uses cyanuricacid, C3N3(OH)3 . When heated to the relatively lowtemperature of 625°F, cyanuric acid converts to gaseousisocyanic acid (HNCO). Isocyanic acid reacts with NO2 inthe exhaust to form nitrogen, carbon dioxide, and water,all of which are normal constituents of the air. (a) Write balanced equations for these two reactions. (b) If the process described earlier became practical, howmuch cyanuric acid (in kilograms) would be requiredto absorb the 1.71010kgNO2 generated annuallyin auto exhaust in the United States?
In a common experiment in the general chemistry laboratory, magnesium metal is heated in air to produce MgO. MgO is a white solid, but in these experiments it often looks gray, due to small amounts of Mg3N2, a compound formed as some of the magnesium reacts with nitrogen. Write a balanced equation for each reaction.
Consider the following particulate-level representation of a chemical equation: The white spheres represent hydrogen atoms, the black sphere represents a carbon atom, and the red spheres represent oxygen atoms. a Write a balanced chemical equation representing this reaction. b Write a word description of the reaction on the particulate and molar levels.
Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
A solution containing 1.63g of barium chloride is added to a solution containing 2.40g of sodium chromate chromate ion, CrO42. Find the mass in grams of barium chromate that can precipitate. Also determine which reactant was in excess, as well as the mass in grams in excess of the amount required by the limiting reactant.