3. It is used to convert the known weight of the precipitate to the corresponding weight of the analyte. a. Gravimetric factor b. Mole ratio c. Mass ratio d. All of the choices 4. Which of the following is used to express the ppm of the solution? a. Kg analyte/liter solution b. Mg analyte/liter solution x 10^6 G analyte/ g sample x 10^6 d. Kg analyte/kg sample C.

3. It is used to convert the known weight of the precipitate to the corresponding weight of the analyte. a. Gravimetric factor b. Mole ratio c. Mass ratio d. All of the choices 4. Which of the following is used to express the ppm of the solution? a. Kg analyte/liter solution b. Mg analyte/liter solution x 10^6 G analyte/ g sample x 10^6 d. Kg analyte/kg sample C.

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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At 90°C, if 51 g of potassium chloride are completely dissolved, the solution is considered to be SOLUBILITY CURVES KI 140 130 120 100 NONO, KNO3 90. HCI, 70 NH CI 60 KCI 50 40 Naci KCIO, 30 20 10 O 10 20 30 40 50 do 70 80 9o 100 TEMPERATURE °C A. supersaturated B. saturated C. uncool GRAMS OF SOLUTE /100g H,0
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12. An unknown precipitate of sulfide from the Group II cations dissolves upon the addition of 20 drops of 3M KOH, this unknown cation may be a. Bismuth b. Tin с. Сорper d. Cadmium e. Iron
KNO3 at 60oC
a. Solid sodium hydroxide is slowly added to 125 mL of a 0.275 M iron(II) sulfate solution until the concentration of hydroxide ion is 0.0204 M. The mass of iron(II) ion remaining in solution is ?grams. b. Solid silver nitrate is slowly added to 150 mL of a 0.196 M sodium carbonate solution until the concentration of silver ion is 0.0673 M. The percent of carbonate ion remaining in solution is ?%. c. Solid sodium carbonate is slowly added to 75.0 mL of a 0.435 M magnesium acetate solution until the concentration of carbonate ion is 0.0465 M. The percent of magnesium ion remaining in solution is ?%.
9. A 50.0 mL solution of acetic acid (CH3COOH) was titrated. In the process 35 mL of a 1.00 M NaOH standard were consumed. find the molarity of the acetic acid. If the density of the acetic acid solution is 1.08 g/mL, calculate the % acetic acid in the sample. CH3COOH + NaOH CH3COONa + H2O
A 0.02198 M AgNO3 solution is used to titrate a 25 mL sample of an unknown chloride solution. Three drops of potassium chromate solution is added to the unknown. It requires 33.59 mL of the AgNO3 solution to change the color of the solution from yellow to peach. Compute the molarity of chloride ion in the unknown. (Note tha Ag+ reacts with Cl- in a 1:1 mole ratio)
Q19: what is the correct answer answer, please follow the rules when answering the question