Consider the following Imagine you start with a 1.40 M stock solution and then take 59.0 mL of the stock solution and dilute it to a total volume of 238 mL. You then take a 119 mL aliquot of that solution and dilute it by adding 143 mL of water. What are the concentrations of the second and final solutions? Initial stock solution = Type your answer here Second solution = Type your answer here Final solution = Type your answer here Unanswered submit Fullscreen

Consider the following Imagine you start with a 1.40 M stock solution and then take 59.0 mL of the stock solution and dilute it to a total volume of 238 mL. You then take a 119 mL aliquot of that solution and dilute it by adding 143 mL of water. What are the concentrations of the second and final solutions? Initial stock solution = Type your answer here Second solution = Type your answer here Final solution = Type your answer here Unanswered submit Fullscreen

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

25.14 ml of 0.2220 M phosphoric acid is neutralized by 38.77 ml of barium hydroxide solution. Determine the Molarity of the barium hydroxide solution.
If 0.500 mL of an 0.219 M NaCl solution is added to 100.0 mL of pure water. what is the concentration of the new solution? Your answer should have 3 sig figs
SIMPLE REACTIONS Shamma V Determining the volume of base neede... A chem student weighs out 0.0999 g of acetic acid (HCH,CO,) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1100 M NAOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits. ||mL O ml. x10 dlo 18 Ar Explanation Check O 2021 Mcolaw- LUutatioI. All RightS RESEIVEU. Privacy Accessibility
2. A 1.25 g sample of impure sodium carbonate requires 18.20 mL of 0.480 M HCI to become completely neutralized. What is the percentage of the sodium carbonate in the original sample?
How many mL of 0.925 M nitric acid are necessary to completely react with 964.0 mL of a 0.250 M calcium hydroxide solution? A) 13.02 mL B) 0.521 mL C) 26.05 mL D) 6.51 mL 身

Hydrobromic acid can be purchased as 50.0% solution. The density of this solution is 1.07 g mL-1. What is the molar concentration of hydrobromic acid in this solution? The molar concentration = i M
Water is added to 68.0 mL of a 1.50 M solution to give a volume of 218 mL. 109 mL is taken from that solution and 143 mL of water is added. Calculate the concentration of this final solution. concentration: M
You may want to reference (Pages 306 - 308) Section 9.5 while completing this problem. Part A Determine the volume, in milliliters, required to prepare each of the following diluted solutions. 23.0 mL of a 0.250 M KNO3 solution from a 6.50 M KNO3 solution Express your answer with the appropriate units. HÁ Value Units Submit Request Answer Part B 28.0 mL of a 2.50 M H2SO4 solution from a(n) 12.4 M H2SO4 solution Express your answer with the appropriate units. HA ? Value Units
A standard solution of HCI is 1.000 M. What mass of HCL is present in 157.0 ml of this solution?
What volume of 0.0521 M Ba(OH)2 is required to neutralize exactly 14.20 mL of 0.141 M HC1? a. 95.2 mL Ob. 19.2 mL OC. 191 mL Od. 38.4 mL
11. If you have 25.0 mL of 8.0M HCl solution, and then dilute it to a final volume of 100.0 ml, what will the new concentration be?