Trial 1 Trial 2 Trial 3 Mass of empty flask (grams) 77.566 77.682 77.564 Mass of flask + vinegar (grams) Mass of vinegar (grams) Concentration of NaOH (mol/L) 87.193 87.246 87.024 9.627 9.564 9.46 0.4 0.4 0.4 Initial volume of NaOH (mL) Final volume of NaOH (mL) 21 21 21 Volume of NaOH added (mL) 21 21 21 Volume of NaOH added (L) 0.021 0.021 0.021 Moles of NaOH used (mol) 0.0084 0.0084 0.0084 Moles of acetic acid (mol) Mass of acetic acid (grams) Mass percent of acetic acid Average mass percent Standard Deviation

Trial 1 Trial 2 Trial 3 Mass of empty flask (grams) 77.566 77.682 77.564 Mass of flask + vinegar (grams) Mass of vinegar (grams) Concentration of NaOH (mol/L) 87.193 87.246 87.024 9.627 9.564 9.46 0.4 0.4 0.4 Initial volume of NaOH (mL) Final volume of NaOH (mL) 21 21 21 Volume of NaOH added (mL) 21 21 21 Volume of NaOH added (L) 0.021 0.021 0.021 Moles of NaOH used (mol) 0.0084 0.0084 0.0084 Moles of acetic acid (mol) Mass of acetic acid (grams) Mass percent of acetic acid Average mass percent Standard Deviation

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

Fill in the blanks please
Your lab group needs to make 25.0 mL of a 2.5 M Cu(NO3)2 solution, which piece of glassware should be used to accurately measure the 25.0 mL solution? 25.0 mL Volumetric Flask 25.0 mL Beaker 25.0 mL Erlenmeyer Flask 25.0 mL Graduated Cylinder
Determine the volume of 0.240 MM KOHKOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is:H2SO4(aq)+2KOH(aq)→H2SO4(aq)+2KOH(aq)→ K2SO4(aq)+2H2O(l) 160 mL of 0.155 M H2SO4 Express your answer using three significant figures.
Hi! Could you please help me into putting the formula into the format as above? Thank you!
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.
0.400 ✓ STARTING AMOUNT 0.400 L X 0.350 mol KBr 1 L X 16.7 g KBr 0.350 mol KBr ✓ What is the mass in grams of KBr in 0.400 = ADD FACTOR x( ) X 0.400 0.140 16.7 5.47 16.7 mol KBr g KBr mL DELETE X A 39.10 1 6.022 × 1023 1.18 × 10-³ M KBr L L of a 0.350 M solution? ANSWER 0.350 136 7.09 × 102⁰ 9.60 × 10-³ g KBr RESET 3 8.43 × 10²² g KBr/mol 119
In this experiment you will use a 3.0 x 10–5 M stock solution of red dye. 3.0 x 10–5 M means that the solution contains 3.0 x 10–5 moles of dye in one liter of solution. How many moles of dye molecules are in 2.0 mL of the 3.0 x 10–5 M stock solution?Express your answer to 2 significant figures
How do I need to rearrange this to have a number and unit in the starting amount? Please draw out the squares so I know how to order everything
O CHEMICAL REACTIONS Solving limiting reactant problems in solution Suppose 1.75 g of potassium nitrate is dissolved in 250. mL of a 48.0 m Maqueous solution of sodium chromate. Calculate the final molarity of nitrate anion in the solution. You can assume the volume of the solution doesn't change when the potassium nitrate is dissolved in it. Be sure your answer has the correct number of significant digits. OM x10 3/5 X
Equal volumes of Solutions 2 and 3 were mixed in the lab. Suggest a measurement that could be made in the lab to provide evidence that a chemical reaction occurred when Solutions 2 and 3 were mixed.
Calculating molarity using solute moles chemist prepares a solution of potassium dichromate (K₂Cr₂O₂) by measuring out 37. μmol of potassium dichromate into a 350. mL volumetric flask and ling the flask to the mark with water. Calculate the concentration in mmol/L of the chemist's potassium dichromate solution. Round your answer to 2 significant digits. mmol L Explanation 10 Check X S 4 99+ 11 Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessib
The molarity of a solution is 0.0200 M or mol/L. Its molar mass is 345.32 g/mol. If you have 50.0 mL of this solution, how many micrograms are contained in it? Hint: You have four conversion factors. 0.0200 moles = 1 liter 345.32 grams = 1 mole 106 micrograms = 1 gram 1000 milliliters = 1 liter Group of answer choices 3.95 x 10^5 micrograms 0.00632 micrograms 5.79 x 10^4 micrograms 1.58 x 10^-4 micrograms