3) In the treatment of myasthenia gravis, 10 mg of guanidine (NH-C(NH2)2) per kilogram of body weight is given. Nitrogen in a sample with a total mass of 7.50 g and containing 4 tablets is converted to ammonia by Kjeldahl decomposition. It is then distilled into 100 mL of 0.1750 M HCI. Performed analysis; titration of excess acid with 11.37 mL of 0.180 M NaOH solution. Accordingly, in which option is the number of tablets at the appropriate dose given for a 48 kg patient? (C-12.0 g/mol; H=1 g/mol; N = 14.0 g/mol; CI-35,5 g/mol) a) 3 b) 6 c) 9 d) 12 f) 15

3) In the treatment of myasthenia gravis, 10 mg of guanidine (NH-C(NH2)2) per kilogram of body weight is given. Nitrogen in a sample with a total mass of 7.50 g and containing 4 tablets is converted to ammonia by Kjeldahl decomposition. It is then distilled into 100 mL of 0.1750 M HCI. Performed analysis; titration of excess acid with 11.37 mL of 0.180 M NaOH solution. Accordingly, in which option is the number of tablets at the appropriate dose given for a 48 kg patient? (C-12.0 g/mol; H=1 g/mol; N = 14.0 g/mol; CI-35,5 g/mol) a) 3 b) 6 c) 9 d) 12 f) 15

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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Direct titration: 10.90 ± 0.02 mL of an unknown KHP solution required 11.72 ± 0.02 mL of 0.1090 ± 0.0006 M NaOH to reach the end point. What is the concentration of KHP in the unknown solution reported with absolute uncertainty? If the unknown solution was prepared by dissolving 5.128 g of the unknown KHP (204.22 g/mol) in 100.00 mL of water, what is the weight percent of KHP in the sample?
In the titration of a volume of 50 mL of a hydrochloric acid solution with Solution density 1.045 g / mL; 29.71 mL of potassium hydroxide with a concentration of 1,963 M were needed, using phenolphthalein as an indicator. Calculate the% m / m of the hydrochloric acid.
A 300mg sample containing Na2CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1M HCl. The titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67mL to reach the methyl red end point. Determine the composition of the sample and calculate the percent of each titrated component.
I titrate a 5.00mL aliquot of Arsenic acid with 36.09 mL 0.126M sodium hydroxide. Calculate the molarity of the arsenic acid sample.
We dissolve 2.77 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution of HA(aq) is 1.33. We titrate this solution with a 0.250 M solution of NaOH. It takes 41.8 mL of the NaOH solution to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the pKa value of HA(aq)? (c) What is the pH at the equivalence point? (d) What is the pH one third along the titration when you still have twice as much HA(aq) as A-(aq)?
7.7 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation. H3C6H5O7 (aq) + NaOH(aq) → H2O(l) + Na H2C6H5O7(aq) what would the curve for the titration of the neutralization of the three hydrogens of this acid with NaOH look like?
Rainwater is slightly acidic due to dissolved CO₂. Use the following data to calculate the pH of unpolluted rainwater at 22.6°C: vol % in air of CO₂ = 0.063 vol%; solubility of CO2 in pure water at 22.6°C and 1.09 atm is 79.29 mL CO2 per 100 mL, K₁1 of H₂CO3 = 5.27x10-7. Express the pH with 2 decimals. You might have to solve a quadratic.
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
In a titration of 50.00 mL of 0.1000 M ethylamine with 0.1000 M HClO4, the titration error must be no more than 0.05 mL. What indicator can be chosen to realize this goal?
A dilute solution of NaOH is titrated with 0.9050 g primary standard potassium hydrogen phthalate (KHP, C8H5K04, FW=204.23 g/mol) which required 10.50 mL of the base using phenolphthalein indicator. (a) What is the color at the endpoint? (b) What is the molar concentration of the titrant?
A mixture was known to contain three of the four compounds in the table. After the mixture of the three solids was extracted with hot water and filtered, Compound A was obtained by evaporating the filtrate to dryness. When 3M HCl was added to the solid residue, a clear solution resulted. After adding excess 3M NaOH solution to the acid solution, a precipitate was formed. After filtration, the insoluble solid was found to be Compound B. Compound C was recovered by evaporation of the filtrate. None of the compounds (A, B, or C) was soluble in all of the solvents; water, 3M HCl, and 3M NaOH. Identify Compounds A, B, and C. Justify your answer.
50 mL sample solution containing Na2CO3 and NaOH is titrated with 0.2 M HCl solution. Acid consumption is 15 mL in the presence of phenolphthalein indicator. Then, the titration is continued by adding bromocresol green indicator and in the presence of this indicator, the acid consumption is 10 mL. Accordingly, which of the following is the amount of Na2CO3 (in grams) in the sample? (NaOH: 40 g / mol; Na2CO3: 106 g / mol)