a) State the number of significant figures in the following examples: i) 17.4 x 104 mg ii) 0.00650 b) Give the answer in the correct number of the significant figures for the following calculation. (1.76 m + 7.8 m) x 3.05 m = c) Briefly describe two ways in which systematic error might occur when using a pipette to transfer a known volume of solution.

a) State the number of significant figures in the following examples: i) 17.4 x 104 mg ii) 0.00650 b) Give the answer in the correct number of the significant figures for the following calculation. (1.76 m + 7.8 m) x 3.05 m = c) Briefly describe two ways in which systematic error might occur when using a pipette to transfer a known volume of solution.

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 standard acid was prepared by placing 5.98 grams of H2C2O42H2O (molar mass: 126.07 g/mole) into a 250.00-milliliter volumetric flask. H2C2O4 (molar mass: 90.04 g/mole) For the blanks in this question: Report here only your numerical answers (without units), if the value is less than zero as a decimal (not in scientific notation), to the correct number of significant figures. Calculate the moles of H2C2O4 in the flask. Calculate the grams H2C2O4 in the flask. Calculate the molarity of the solution if the volumetric flask is filled to the mark with water.
A:If 100 mL of a 0.15 M Mg(NO3)2(aq) solution has a density of 1.09 g/mL, which of the following statements is false? Group of answer choices The mass of Mg(NO3)2 in this solution can be determined from this information. If the solution density was not given, it is usually reasonable to assume 1.00 g/mL The mass of the water in this solution is 109 g It is possible to determine the mole fraction of water in this solution. B: In the body, cell membranes act like semipermeable membranes discussed in class. If a red blood cell is surrounded by fluid with a higher electrolyte concentration than what is inside the cell, which of the following statements is true? Group of answer choices The cell will shrink because water will pass from the inside of the cell to the fluid The surrounding fluid has a lower osmotic pressure than what is inside the cell The cell will swell up because water will pass from the fluid to the inside of the cell Nothing will happen to the…
Suppose 4.47 g of barium acetate is dissolved in 350. mL of a 69.0 m M aqueous solution of ammonium sulfate. Calculate the final molarity of barium cation in the solution, You can assume the volume of the solution doesn't change when the barium acetate is dissolved in it. Round your answer to 3 significant digits. | M
Report your answer to 3 significant figures in scientific notation (example: 1.23E+4) unless stated otherwise. DO NOT include the units in your answer. 1. Consider a reaction of 827 mL of a 6.14×10-2 M K,S04 solution completely reacts with 131 mL of a 3.54x102 M CaI, solution according to the following UNBALANCED chemical equation. K2SO4(aq) + Cal2(aq) → CaSO4(s) + KI(aq) (a) Balance the chemical equation using the lowest integer coefficients. Be sure to include all coefficients including those of 1. 1 K2SO4(aq) + 1 Cal2(aq) 1 CaSO4(s) + 2 KI(aq) You are correct. Your receipt no. is 155-6200 ? Previous Tries (b) Determine the mass (in g) of CaSO4 that is formed in the reaction. Report your answer to 3 significant figures in standard notation (example: 1.23). g Submit Answer Tries 0/99 (c) If 3.58x10-1 g of CaSO4 is produced, what is the percent yield of the reaction? Report your answer to 3 significant figures in standard notation (example: 1.23).
Suppose 4.73g of barium nitrate is dissolved in 350. mL of a 73.0mM aqueous solution of ammonium sulfate. Calculate the final molarity of barium cation in the solution. You can assume the volume of the solution doesn't change when the barium nitrate is dissolved in it. Be sure your answer has the correct number of significant digits
A chemist must prepare 800. mL of 69.0 µM aqueous mercury(II) iodide (HgI,) working solution. He'll do this by pouring out some 0.000101 M aqueous mercury(II) iodide stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the mercury(II) iodide stock solution that the chemist should pour out. Round your answer to 3 significant digits.
A sample with a mass of 1.340 g was dissolved in water, releasing chlorine ions. The aqueous solution was treated with access AgNO3(aq), the AgCl precipitate collected and weighted. Its mass was 2.709 g. What percentage by mass was the original sample? Make sure to use the correct number of significant figures in your answer.
A chemist must dilute 99.9 mL of 161. mM aqueous silver perchlorate (AgClio,) solution until the concentration falls to 117. mM. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in liters. Round your answer to 3 significant digits.
Suppose 13.0g of potassium sulfate is dissolved in 250.mL of a 0.20 M aqueous solution of sodium chromate. Calculate the final molarity of sulfate anion in the solution. You can assume the volume of the solution doesn't change when the potassium sulfate is dissolved in it. Be sure your answer has the correct number of significant digits.
umol A chemist must prepare 450. mL of 15.0 µM aqueous mercury(II) iodide (Hgl,) working solution. She'll do this by pouring out some 24.0 aqueous L mercury(II) iodide stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the mercury(II) iodide stock solution that the chemist should pour out. Be sure your answer has the correct number of significant digits. O ml FEB W 606 19 MacBook Air 888 DII DD F7 FB F2 F3 F4 %23 2$ 4 5 6 7 8
A student sets up and solves the following equation to solve a problem in solution stoichiometry. Fill in the missing part of the student's equation. 6.9 ml)(0.11 1) (119.86|[]) = 91. g x10 X μ 00 5
A chemistry student must write down in her lab notebook the concentration of a solution of sodium thiosulfate. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: • The label on the graduated cylinder says: empty weight: 5.0 g She put some solid sodium thiosulfate into the graduated cylinder and weighed it. With the sodium thiosulfate added, the cylinder weighed 61.167 g. • She added water to the graduated cylinder and dissolved the sodium thiosulfate completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 10.64 mL. What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits. - 1 g•mL х10