1 Making 25.00 mL of 0.900 % (m/v) saline solution from the 9.00 % (m/v) stock solution.Q2)How many milliliters of 9.00 % stock NaCl solution are needed to create 25.00 mL of 0.900 %(m/v) Nacl solution? Use factor-label and show all work.

C1V1 = C2V2 as number of moles remain same after dilution .or we can say amount of solute remain…

Answered: How many milliliters of 9.00 % stock…

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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During lab, a student used a Mohr pipet to add the following solutions into a 25 mL volumetric flask. They calculated the final volumes added, which are recorded below. The student then followed the directions in the manual to make the stock solution. Volumes Used to Create Stock Solution Volume 0.200 M Fe(NO3)3 (mL) Volume 0.00200 M KSCN (mL) Stock Solution 8.99 mL 2.38 mL Using the stock solution above, the student made additional dilutions, with the final volumes below. Calculate the [FeSCN2+] in Standard 2. Report your answer in mM. Volumes Used to Create Standard Solutions Solution Volume Stock solution (mL) Volume Water (mL) Standard 1 7.04 3.47 Standard 2 4.72 5.13 Standard 3 2.71 7.43 Standard 4 1.41 9.14 Note: Reporting your answer in mM is for grading purposes only. It is not necessary during lab. Report your answer to three places after the decimal.
What's the differences between two questions? Q1) How much calcium would you ingest by drinking one 8 oz glass of your tap water? Show all calculations. -->Tap water 8Oz = 8 x 0.0296L = 0.2368L Hardness = 66.73ppm = 66.73mg/L CaCO3 1L has 66.73mg CaCO3 0.2368L has 66.73mg x 0.2368 = 15.8017mg MW of CaCO3 = 100g/mol MW of Ca = 40g/mol 100g CaCO3 has 40gf of Ca 15.8017mg CaCO3 has 40/100 x 15.8017mg Ca We would ingest 6.321mg of Ca. Q2) What percentage of the recommended daily dose of calcium (1,150 mg/day) does 1.0 L of your water provide? Show all calculations. --> 66.73mg/1150mg x 100 = 5.80% My Question) Why this calculation is wrong? I think this calculation is same with question 1. Isn't it? CaCO3 = 100g/mol, Ca = 40g/mol 100g CaCO3 has 40g Ca. 66.73 CaCO3 has 40/100 x 66.73mg Ca Ca = 26.70mg 26.70mg/1150mg x 100 = 2.32%
Cedrick and Astrid a 20.00 ml aliquot of grapefruit juice with a 0.165 M NaOH solution to the end point. The initail buret reading was 1.72ml and final buret reading was 15.51ml. They calculated that there was 0.1457g of citric acid present in the juice sample. What is the amount mg of citric acid present per ml of juice? the answer is 7.29mg/ml. (can you please show me how to calculate this answer)
Standardization of Sodium Thiosulfate Solution Primary Standard used: Potassium Dichromate Formula mass of 1o standard: __________________ % Purity of 1o standard: 99.80% Trials 1 2 3 Weight of K2Cr2O7 (g)Weight of K2Cr2O7 (g) 0.0315 0.0331 0.0380 Final Volume Reading Na2S2O3 (ml) 27.50 27.50 34.90 Initial Volume Reading Na2S2O3 (ml) 1.10 0.00 1.00 Net Volume Na2S2O3 used (ml) Molarity of Na2S2O3
b. How would a student prepare 25.0 mL of 40.0% standard solution from a 100.0 % stock solution. What is the volume of stock solution needed? a. 10ml b. 20ml c. 25ml d. 15ml Please show work
Data of milk: (first trial) Mass of milk: 104.4579g Concentration of NaOH (M): 0.09639 Volume of NaOH solution used: 5.5 mL Data of milk: (2nd trial) Mass of milk: 103.8405g Concentration of NaOH (M): 0.09639 Volume of NaOH solution used: 5.3 mL
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You have a micro tube containing 1mL of a solution with 4.3x10^4 cells/mL and you are to produce a solution that contains 43 cells/mL. The most accurate way to do this is to preform a series of 1:10 dilutions (add 1mL of stock solution to 9mL of water to achieve a factor of 10 dilution). How many of these dilutions must you preform to achieve the desired solution?
6) 100.01 mg Cu(NO3)2 is diluted to 100.00 mL with distilled water. Calculate the ppm of the resulting solution and also calculate the uncertainty of the result. Report the result with the suitable number of significant figures (the uncertainty of 100.00 mL capacity volumetric flask is 0.07 mL, the uncertainty coming from the weighing is 0.05 mg).
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Using dimensional analysis, find the mass of acetylalicylic acid in one tablet of aspirin. The grams of aspirin used in a titration is .325g before being dissolved in 10mL of water and then added to a base, NaOH, with a molarity of .01M and a volume of 10.1 mL. In Chem2.png, the actual question is boxed in red Video used for titration assignment (Not needed for question): https://www.youtube.com/watch?v=x9jgjdizTaY

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How many milliliters of 9.00 % stock NaCl solution are needed to create 25.00 mL of 0.900 % (m/v) Nacl solution? Use factor-label and show all work. Q2)