2) A student investigated the neutralisation of dilute hydrochloric acid, using an excessof calcium carbonate.Step 1 Excess calcium carbonate was added to hydrochloric acid.calcium carbonateBdilute hydrochloric acidStep 2. Excess calcium carbonate was removed from the solution.excess calcium carbonatesolution of calcium chloride(a) Identify the pieces of apparatus labelled:A.В..С.(3)

Answered: Image /qna-images/answer/19b5d6ec-e559-4163-826c-11e52b58563a.jpg

2) A student investigated the neutralisation of dilute hydrochloric acid, using an excess of calcium carbonate. Step 1 Excess calcium carbonate was added to hydrochloric acid. A calcium carbonate dilute hydrochloric acid Step 2. Excess calcium carbonate was removed from the solution. excess calcium carbonate solution of calcium chloride (a) Identify the pieces of apparatus labelled: А. В... С...

2) A student investigated the neutralisation of dilute hydrochloric acid, using an excess of calcium carbonate. Step 1 Excess calcium carbonate was added to hydrochloric acid. A calcium carbonate dilute hydrochloric acid Step 2. Excess calcium carbonate was removed from the solution. excess calcium carbonate solution of calcium chloride (a) Identify the pieces of apparatus labelled: А. В... С...

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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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?
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What is the difference between a solute and a solvent?
A student was given a 1.6240-g sample of a mixture of sodium nitrate and sodium chloride and was asked to find the percentage of each compound in the mixture. She dissolved the sample and added a solution that contained an excess of silver nitrate. The silver ion precipitated all of the chloride ion in the mixture as silver chloride. It was filtered, dried, and weighed. Its mass was 2.056g. What was the percentage of each compound in the mixture?
Apply Students conducted a lab to investigate limiting and excess reactants. The students added different volumes of sodium phosphate solution (Na3PO4) to a beaker. They then added a constant volume of cobalt(ll) nitrate solution (CO(NO3)2) stirred the contents, and allowed the beakers to sit overnight. The next day, each beaker had a purple precipitate at the bottom. The students decanted the supernatant from each beaker, divided it into two samples, and added one drop Of sodium phosphate solution to one sample and one drop of cobalt(ll) nitrate solution to the second sample. Their results are shown in Table 11.5. a. Write a balanced chemical equation for the reaction. b. Based on the results, identify the limiting reactant and the excess reactant for each trial.
ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.
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.