All of the following chemical laboratory practices are correct except A We must avoid weighing corrosive substances in an analytical balance. B We should always weigh hygroscopic substances using a weighing bottle We should always wait for the substance (to be weighed) to cool down first to room temperature before weighing D We should always prepare the stock solution from the working solution

All of the following chemical laboratory practices are correct except A We must avoid weighing corrosive substances in an analytical balance. B We should always weigh hygroscopic substances using a weighing bottle We should always wait for the substance (to be weighed) to cool down first to room temperature before weighing D We should always prepare the stock solution from the working 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

Which of these reactions is not a redox reaction? a. 2K + Cl₂ ⟶ 2KCl b. KOH + HCl ⟶ KCl + H₂O c. 2KClO₃ ⟶ 2KCl + 3O₂ d. 2K + 2H₂O ⟶ 2KOH + H₂ e. C₆H₁₄ + O₂ ⟶ 6CO₂ + 7H₂O
Imagine you were working as a laboratory technician and your principal investigator asked you to develop Benedict’s test into a quantitative measure of the concentration of reducing sugar in a solution. To do this, you would first need to decide what to measure and then establish the relationship between your measurements and different concentrations of reducing sugars. Explain generally what you would decide to measure and how you would go about determining the relationship of your measurements to the concentration of reducing sugar.
Determine which two of the following reactions are redox reactions. If the reaction is a redox reaction, indicate which element is being oxidized. Briefly explain your answers. Mg + Cl2 ⟶ MgCl2 MgO + 2HCl ⟶ MgCl2 + H2O 2CuCl2 + 4KBr ⟶ 2CuBr + 4KCl + Br2
Table 6.1 (data and report) Samples Reacted Observations Mg(combustion) HCI and NH3 Blank 1 Blank 2
Converting Concentrations to Different Units Introduction: Depending on how the concentration unit is defined, concentration can serve as a conversion between the amount of a solute and the amount of a solution or solvent. Concentrations can therefore be helpful in a number of stoichiometry issues. The original definition of the concentration unit is frequently preferred because it contains the conversion factor. Today, for chemists, it is suitable to make a solution in the lab using a specific concentration unit like molarity, and then convert the concentration to another unit. Today in the lab, I will prepare a sodium bicarbonate (baking soda) solution with a specific molarity. I will then translate the concentration into molality, mass percent, and mole fraction. Procedure The first step of this lab was to make sure I had everything I needed and that my surroundings were safe. I then looked at an empty beaker weighing paper and a balance. I first took a piece of weighing…
Balanced chemical equations show________. A. whether a chemical reaction will occur. B. the concentration of reactants and products. C. that molecules are conserved. D. the relative number of reactant molecules which can take part in a chemical reaction.
Masses : Ca = 40.08 g S= 32.07 g O= 16.00 g A 35.0 mL sample of CaSO4 was evaporated to dryness, leaving 0.967 g of residue. What was the molarity of the original solution? step by step please
Answer the 4 questions on the second pictured based on the data table provided. PPT means precipitate and NR is NO REACTION. POST PICTUREs OF YOUR WORK PLEASE.
please answer this and provide the correct amount of sig figs
1. Write complete balanced equations for the following. Write the net ioni equation when appropriate. a. liquid methanol (CH,OH) is ignited b. magnesium oxide powder is mixed with an acetic acid solution c. solutions of lead(II) nitrate and ammonium iodide are mixed producing a precipitate