150.0 mL of 0.2105 M nitric acid was added to 1.3415 g calcium carbonate. The excess acid was back titrated with 0.1055 M sodium hydroxide. It required 75.5 mL of the base to reach the end point. Calculate the percentage (%w/w) of calcium carbonate in the sample. HNO; + NAOH NaNO3 + H2O 2HNO3 + CaCO3- Ca(NO3)2 + H2O + CO2

150.0 mL of 0.2105 M nitric acid was added to 1.3415 g calcium carbonate. The excess acid was back titrated with 0.1055 M sodium hydroxide. It required 75.5 mL of the base to reach the end point. Calculate the percentage (%w/w) of calcium carbonate in the sample. HNO; + NAOH NaNO3 + H2O 2HNO3 + CaCO3- Ca(NO3)2 + H2O + CO2

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...

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Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
A 250.0-mg sample of an organic weak acid was dissolved in an appropriate solvent and titrated with 0.0556 M NaOH, requiring 32.58 mL to reach the end point. Determine the compound’s equivalent weight.
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Total acidity of commercial white wine was determined by titration with 0.1512 M NaOH. A. Write the balanced chemical equation between tartaric acid and NaOH. B. If 3.00mL of the sample required 3.35mL NaOH, calculate the total acidity as % (w/v) tartaric acid (H2C4H4O6) of the commercial white wine.
A 100 mL sample contains Na2CO3 and NaOH. A 25 mL aliquot was taken and phenolphthalein was added as indicator into the solution. The sample solution was titrated with 13.0 mL of 0.10 M HCl. After the disappearance of the pink color, methyl orange was added and the sample solution was titrated with 4.0 mL of 0.10 M HCl. Calculate the amounts of Na2CO3 and NaOH in the sample as mg/100 mL. (write all chemical reactions, Na:23, C:12, O:16, H:1 g/mol).
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I want to make a buffer solution containing 1 M glycene pH = 10 (Na+), 1 mM ZnCl2 , 1 mM NaOH. I have the stock solutions 1 M glycene, 1 M MgCl2, 1 M ZnCl2, and 10 M NaOH. My final volume of buffer solution needs to be 250ml. how much (in ml) of each solution should i put into my buffer?
4) Students were asked to perform a lab to identify an unknown acid.The experiment has several parts. First the students had to make a sodium hydroxide solution with a molarity of approximately 0.2M. Then the students had to perform a titration with potassium hydrogen phthalate to standardize their solution. Finally they had to perform a titration with the unknown acid to find the pKa and the molar mass, then using theirdata they had to determine which of the weak acids they had used.Part 1) Make a sodium hydroxide solutionA student measured 4.03 grams of NaOH in a tared weigh boat. They then dissolved it into approximately 200 mL of deionizedwater in a beaker. Once it was completely dissolved the student poured the solution into a 500.0 mL volumetric flask. The student rinsed the beaker with deionized water and added the rinse water to the volumetric flask. They repeated with process, adding the rinse water to the volumetric flask again, they mixed this thoroughly. Finally, they…
5. 25.00 mL of HCN (K₂=4.90 x 10-10) was titrated with 18.50 mL of 0.0125 M Ca(OH)2. a) What is the concentration of HCN in the original sample? b) What is the pH after 9.25 mL of base have been added? c) What is the pH of the solution at the endpoint of the titration?
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