Complete the given data sheet in determination of total alkaline strength in soda Show your computations. Wt. of soda ash Vf HCI Vi HCI Vf NaOH Vi NaOH %Na₂CO3 %Na₂O %Na₂CO3 Percentage purity of sample: mLs x Ns x me.wt.xx 100 wt.sample 0.4 g x% 4.6 mL 0 mL 0 mL 0 mL I 0.4 g Alkaline strength of sample in terms of %Na2CO3 or %Na2O: mLs x Nsx me.wt.Na₂0 X 100 wt.sample 10.2 mL 4.6 mL 0 mL 0 mL ||

Complete the given data sheet in determination of total alkaline strength in soda Show your computations. Wt. of soda ash Vf HCI Vi HCI Vf NaOH Vi NaOH %Na₂CO3 %Na₂O %Na₂CO3 Percentage purity of sample: mLs x Ns x me.wt.xx 100 wt.sample 0.4 g x% 4.6 mL 0 mL 0 mL 0 mL I 0.4 g Alkaline strength of sample in terms of %Na2CO3 or %Na2O: mLs x Nsx me.wt.Na₂0 X 100 wt.sample 10.2 mL 4.6 mL 0 mL 0 mL ||

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...

See similar textbooks

Similar questions

y Song - CHEM-1405 63... pter 9 Assignment 3 Dok nt nt nces Solubility Song - YouTube % KF ezto.mheducation.com G carbonates examples - Google Search Saved M Question Determine the mass percent composition of a solution made by dissolving 21.1 g of KF in 415 g of H₂O.
A 25.190 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is diluted with 74.348 g of water. A 10.405 g aliquot of this solution is then titrated with 0.1058 M HCI. It required 28.58 ml. of the HCI solution to reach the methyl red endpoint. Calculate the weight percent NH, in the aqueous waste. wt% NH, %3D Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid-base titrations. If 19.15 ml.L NAOH is required to neutralize 0.427 g KHP, what is the concentration of the NaOH? M concentration:
A student prepares a 3.2M aqueous solution of benzoic acid (C,H,CO,H). Calculate the fraction of benzoic acid that is in the dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. | % x10
Consider a 1.000-L stock solution of 9.69 M Na3PO4. A 2.000-mL aliquot is taken from this stock solution and diluted to a final volume of 1.000 L. A 5.000-mL aliquot is then taken from this new solution and further diluted to make a new solution with a final volume of 750.0 mL. Calculate Na+ in the final solution.
A 10.00 ml sample with an unknown concentration of KNO3 was studied at 60° C. If an additional 2.4 g of KNO, were added to reach saturation. What was initial concentration of Q3 KNO, in M.
Please help I'm not sure how to solve these. A solution is prepared by dissolving 20g of NaCl (f.w.= 58.44 g mol^-1), a nonvolatile solute, in enough water (m.w. = 18.02 g mol^-1) to result in exactly 1 L of solution at 25 C. The density of the solution is 1 g mL ^-1. How do you calculate freezing point of the solution as well as vapor pressure and the osmotic pressure? I understand boiling point.
Are you completing this experiment online? Yes Part A Data. Standardization of a Sodium Hydroxide Solution Data Table 1. Measurements for standardization of NaOH Data Table 1. Measurements for standardization of NaOH Trial 1 Trial 2 Trial 3 [1] Tared mass of KHC8H404 (g) 0.335 0.308 0.383 [2] Burette reading of NaOH, initial (mL) 3.75 3.91 4.15 [3] Burette reading of NaOH, final (mL) 19.83 18.14 21.36 Part B Data. Molar Concentration of an Acid Solution Enter the number corresponding to the type of acid you have 1. НА 1 2. H2А 3. НзА
The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g Volume of H2C2O4•2H2O solution = 250.0mL What is the Molarity H2C2O4 standard solution ?
Solution X 100 mL of 0.10 M NaOH(aq) is mixed with 100 mL of 0.10 M HBr(aq) Solution Y 100 mL of 0.10 M NaBr(aq) is mixed with 100 mL of 0.10 M HBr(aq) Solution Z 100 mL of 0.10 M HC,H,O,(aq) is mixed with 100 mL of 0.10 M NaC,H3O,(aq) 6. A student prepares three solutions, X, Y, and Z, as described in the table above. The values of Ka for the acidic species in the solutions are given in the table below. Species Ka HBr(aq) >>I (very large) HC,H;O,(aq) 1.8 x 10-5 a. Using the information above, write the letters of the solutions in the boxes below to rank the solutions in order of increasing pH. Explain your reasoning for the ranking Lowest pH Highest pH b. Does the pH of solution Y increase, decrease, or remain the same when 100 mL of water is added? Justify your answer. c. The student adds 0.0010 mol of NaOH(s) to solution Y, and adds 0.0010 mol of NaOH(s) to solution Z. Assume that the volume of each solution does not change when the NaOH(s) is added. The pH of solution Y changes…
The molecular weight of acetylcholine chloride is 181.7. A stock solution of 1.817 g acetylcholine is 10.0mL was prepared by the stockroom. What is the concentration of this stock solution in % w/v and in molarity? From this stock solution of acetylcholine chloride, 0.40 mL was added to the sample tube brining the total volume in the sample tube to 3.0 mL. What is the concentration of the acetylcholine chloride in the sample tube in g/mL and in molarity?
Ksp(CaF2) = 3.9 x 10-11. Assume that we add enough amount of CaF2 into the following 3 solutions so that CaF2 will become saturated in each solution. Solution A. 0.30 M Ca(NO3)2 (aq). Ca(NO3)2 is highly soluble in water. Solution B. 0.30 M NaF (aq). NaF is highly soluble in water. Solution C. 0.30 M NaNO3 (aq). NaNO3 is highly soluble in water. Which of the following statements is true about the solubility of CaF2 in the above 3 solutions? Choose one option only. Options: a. CaF2 (s) has the lowest solubility in Solution B. b. CaF2 (s) has the highest solubility in Solution B. c. CaF2 (s) has the highest solubility in Solution A. d. CaF2 (s) has the lowest solubility in Solution C. e. CaF2 (s) has the lowest solubility in Solution A.
The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g what is the Number of moles of H2C2O4•2H2O?