6. A sample of hydrochloric acid is standardized using sodium bicarbonate.ExperimentWrite the balanced chemical equation for the reaction of hydrochloric acid with sodium bi-a.carbonate, NaHCO,.b. Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric acidwas required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point.Calculate the mass percent concentration of hydrochloric acid using the molar concentrationcalculated in part b and assuming the density of the solution is 1.01 g/mL.с.7. Malonic acid, H,C¸H,O,(aq), is a diprotic acid, so 2 moles of hydroxide ions are required per moleof malonic acid for complete neutralization.Write the balanced chemical equation for the reaction of malonic acid with potassium hy-droxide. ea.79Quantitative Analysis of Vinegar via Titration

We have to give the reaction of HCl with NaHCO3

6. A sample of hydrochloric acid is standardized using sodium bicarbonate. Write the balanced chemical equation for the reaction of hydrochloric acid with sodium bi- carbonate, NaHC,. a. b. Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point.

6. A sample of hydrochloric acid is standardized using sodium bicarbonate. Write the balanced chemical equation for the reaction of hydrochloric acid with sodium bi- carbonate, NaHC,. a. b. Calculate the molar concentration of the hydrochloric acid if 35.18 mL of hydrochloric acid was required to neutralize 0.450 g of sodium bicarbonate to a phenolphthalein end point.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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6. Sodium sulfide reacts with hydrochloric acid to produce hydrogen sulfide and sodium chloride. How many grams of sodium sulfide are required for complete reaction with 15.0 mL of 0.250 M hydrochloric acid? The molar mass of sodium sulfide is 78.046 g/mol. (Hint: start by writing the balanced equation for the reaction.)
A sample of 3.0600 grams contains a mixture of sodium carbonate and calcium carbonate. This sample was dissolved with 92.81 mL hydrochloric acid, heated to completely remove the reaction gases. After cooling to room temperature, this solution is put in a volumetric flask and diluted to a volume exactly 100.00 mL. This solution is acidic. a. Write down the equation for the ionic reaction in the process of dissolving the sample of the carbonate mixture. The excess acid in the dissolving process is neutralized by alkaline, how: 10.00 mL of the mixed solution is titrated with 0.1072 M sodium hydroxide solution and 37.31 mL is needed to neutralize it properly. b. Write down the equation for this neutralizing reaction. The titrated solution is reacted with an excess of ammonium oxalate, (NH4) 2C2O4, to separate the calcium ions. The resulting precipitate was filtered, washed and dried and then weighed as much as 0.2560 g. c. Write down the equation for the reaction in this calcium separation…
12. A 4.00 g sample of KCl is added to 10.0 mL flask, which is then filled to the calibration mark with water to form Solution 1. Next, 2.00 mL of Solution 1 is then added to a 2.00 L flask and the flask is filled with water to the calibration mark to form Solution 2. What is the molarity of Solution 2?
1. Write a chemical equation for the dissolution of sodium chloride in water 2. What is the concentration (in moles per litre, mol L−1 or M) of 20.0 g of NaCl in 500.0 mL of distilled water? Show your working. 3. What is the concentration of each of the ions (in moles per litre, mol L−1 or M) in this solution?
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2. A 0.5192 g sample of a solid monoprotic acid (molar mass of 180.0 g/mole) was dissolved in water and titrated by the addition of an aqueous solution of NaOH. To reach the equivalence point, 15.96 mL of NaOH solution were required. a. Calculate the molarity of the NaOH solution. de Im 00.01 A b. Write the generic representation of the reaction of a monoprotic acid with NaOH. Then, calculate the molar mass of an unknown monoprotic acid if 15.64 mL of the NaOH solution from (a) was required to titrate 0.8256 g of the acid. Reaction:
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