The calcium in a 200 ml sample of water was determined by precipitating the cation as CaC204. The precipitate was filtered, washed and ignited in a crucible with an empty mass of 26.6002 g. The mass of the crucible plus CaO (56.077 g/mol) was 26.7134 g. Calculate the concentration of Ca (40.078 g/mol) in water in units of g/100 mL H2O 0.6040 g/ 100 ml 0.01009 g/ 100 mL O 0.0704 g/ 100 mL 0.0804 g/ 100 mL O 0.0404 g/ 100 ml

The calcium in a 200 ml sample of water was determined by precipitating the cation as CaC204. The precipitate was filtered, washed and ignited in a crucible with an empty mass of 26.6002 g. The mass of the crucible plus CaO (56.077 g/mol) was 26.7134 g. Calculate the concentration of Ca (40.078 g/mol) in water in units of g/100 mL H2O 0.6040 g/ 100 ml 0.01009 g/ 100 mL O 0.0704 g/ 100 mL 0.0804 g/ 100 mL O 0.0404 g/ 100 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

A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 13.mg of oxalic acid H2C2O4, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 11.9mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits.
In a titration experiment, a 5.00-mL sample of sulfuric acid, H2SO4, from a car battery is diluted with de-ionized water to 100.0 mL. A 20.00-mL portion of the diluted acid is titrated with 0.2025 MNaOH solution. If 42.00 mL of the NaOH solution is required to neutralize the dilute acid, what is the molar concentration of H2SO4 in the original solution taken from the battery? The acid-base reaction occurs as follows: H2SO(aq) + 2NaOH(aq) --> Na2SO4(aq) + 2H2O(l) (A) 0.2126 M (B) 0.4252 M (C) 4.25 M (D) 8.50 M
A solution of 655 mL of 0.852 M CO(NH2)2 is mixed with a solution of 432 mL of 0.487 M CO(NH2)2. It is then evaporated on a hotplate to a volume of 825 mL. What is the molarity of CO(NH2)2 in this final solution? [Be aware that evaporation only changes the amount of water, not the amount of CO(NH2)2, because the boiling point of CO(NH2)2 is nearly 200 °C, too high to evaporate out of the solution to a significant extent].
The calcium in a 200 mL sample of water sample was determined by precipitating the cation as CaC2O4. The precipitate was filtered, washed and ignited in a crucible with an empty mass of 26.6002 g. The mass of the crucible plus Cao (56.077 g/mol) was 26.7134 g. Calculate the Molarity of Ca. a. 0.005 M O b. 0.040 M O c. 0.100 M O d. 0.080 M O e. 0.010 M
In the laboratory you are given the task of separating Ag+ and Co2+ ions in aqueous solution.For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No Y or N Reagent Formula of Precipitate if YES 1. fill in the blank 1 NaOH 2. fill in the blank 3 Na2CO3 3. fill in the blank 5 NaI
4. The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration, 34.67 mL of the sodium hydroxide solution was required to react with 0.1082 g KHP. Calculate the molarity of the sodium hydroxide.
To a 25.00 mL volumetric flask, a lab technician adds a 0.125 g sample of a weak monoprotic acid, HA, and dilutes to the mark with distilled water. The technician then titrates this weak acid solution with 0.0802 M KOH. She reaches the endpoint after adding 42.61 mL of the KOH solution.Determine the number of moles of the weak acid in the solution. moles of weak acid: mol Determine the molar mass of the weak acid. molar mass = g/mol After the technician adds 17.07 mL of the KOH solution, the pH of the mixture is 5.71. Determine the pKa of the weak acid. p?a=
You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. You prepared solutions of both NaOH and HCl. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 32.35 mL of HCl solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCl solution?
To a 25.00 mL volumetric flask, a lab technician adds a 0.425 g sample of a weak monoprotic acid, HA, and dilutes to the mark with distilled water. The technician then titrates this weak acid solution with 0.0810 M KOH. She reaches the endpoint after adding 48.89 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: mol Determine the molar mass of the weak acid. molar mass = g/mol After the technician adds 18.61 mL of the KOH solution, the pH of the mixture is 4.65. Determine the pK, of the weak acid. pKa
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 316.mg of oxalic acid H2C2O4 , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 93.2mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.
0.3456 g of a solid acid is dissolved in 50 mL of water in a flask and a few drops of phenolphthalein are added to the solution. A buret containing 0.2545 M NaOH is prepared with an initial volume of 10.50 mL. The acid is accidentally titrated with the base beyond the end point, so 1.52 mL of 0.187 M HCl are added to the flask. The titration with the base is continued to a final volume reading of 40.55 mL. Calculate the molar mass of the solid acid.
40.00 mL of a solution of MgCl2 with a molar volume concentration of 0.933 mol/L is mixed with 100.0 mL of a solution of AlCl3 with a molar volume concentration of 0.211 mol/L. What is the final molar volume concentration of chloride ions (Cl-) in the mixture in mol/L? Note: The density of pure water is 1.000 g/mL.