A chemist prepares a solution of potassium iodide (KI) by measuring out 3.0 x 10 umol of potassium iodide into a 350. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in umol/L of the chemist's potassium iodide solution. Round your answer to 2 significant digits. u mol

A chemist prepares a solution of potassium iodide (KI) by measuring out 3.0 x 10 umol of potassium iodide into a 350. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in umol/L of the chemist's potassium iodide solution. Round your answer to 2 significant digits. u mol

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

An aqueous stock solution is 72.0% HNO3 by mass and its density is 1.42 g/mL. What volume of this solution is required to make 1.50 L of 1.05 mol/L HNO3(aq)? Give your answer in millilitres, accurate to three significant figures. Enter the correct symbol for millilitres in the units box. Molar masses(in g mol−1) HNO3, 63.018 H2O, 18.016
Calculate the final molarity of bromide anion in the solution. You can assume the volume of the solution doesn't change when the zinc bromide is dissolved in it. Be sure your answer has the correct number of significant digits.
A buret is used to measure the volume of FeCl3 aqueous solution. The starting volume is recorded to be 5.28 mL. The ending volume is recorded as 17.44 mL. What is the total volume of FeCl3 solution dispensed?
A 25.0 mL sample of phosphoric acid requires 22.5 mL of 1.1 M sodium hydroxide for complete neutralization. What is the molarity of the phosphoric acid? The neutralization reaction : H3PO4 + 3NaOH ----> Na3PO4 + 3H2O Write your numerical answer without unit inside the box. The answer should be in Two Significant figures and in standard, not scientific notation.
A solution containing 405.6 mM CaCl₂ is combined with an equal volume of 176.1 mM NaCl. What is the concentration of chloride (CI) ions in the resulting solution? Express your answer using units of millimolar (mM) using at least three significant figures.
A chemist prepares a solution of potassium bromide KBr by measuring out 0.17g of KBr into a 300.mL volumetric flask and filling to the mark with distilled water. Calculate the molarity of Br− anions in the chemist's solution. Be sure your answer is rounded to 2 significant digits.
The average concentration of dissolved gold in earth's oceans is 5.8 x 10^−9 g/L. of ocean water.How many micrograms of gold are in 1.1x10^3 m^3 of ocean water? (1 ml = 1 cm3)
A chemist prepares a solution of potassium chloride KCl by measuring out 0.23g of KCl into a 300.mL volumetric flask and filling to the mark with distilled water. Calculate the molarity of Cl− anions in the chemist's solution. Be sure your answer is rounded to the correct number of significant digits.
A chemist adds 435.0 mL of a 0.0630 mmol/L potassium permanganate (KMnO4) solution to a reaction flask. Calculate the mass in milligrams of potassium permanganate the chemist has added to the flask. Round your answer to 3 significant digits.
An aqueous solution of nickel(II) bromide, NiBr2, is made by dissolving 11.2 grams of nickel(II) bromide in sufficient water In a 250. mL volumetric flask, and then adding enough water to fill the flask to the mark. What is the weight/volume percentage of nickel(II) bromide in the solution? Welght/volume percentage =
An analytical chemist weighs out 0.061 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1900 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 3.3 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits. g 0 x10 mol C X Ś 2.
Suppose 3.30 g of barium acetate is dissolved in 100. mL of a 0.50 M aqueous solution of ammonium sulfate. Calculate the final molarity of acetate anion in the solution. You can assume the volume of the solution doesn't change when the barium acetate is dissolved in it. Be sure your answer has the correct number of significant digits.