Recall that the test solutions were prepared according to Table KEQ.2. Table KEQ.2:Volumes for the Test Solutions Test Solution 6 7 8 9 10 2.00x10-3 M Fe(NO3)3 5.00 mL 5.00 mL 5.00 mL 5.00 mL 5.00 mL Molar concentration of Fe(NO3)3 stock solution: 2.00 x 10-¹ M Molar concentration of KSCN stock solution:2.00 x 10-³ M 2.00x10-3 M NaSCN 1.00 mL 2.00 mL 3.00 mL 4.00 mL 5.00 mL 0.100 M HNO3 4.00 mL 3.00 mL 2.00 mL 1.00 mL 0.00 mL Use the ICE tables below to calculate the equilibrium concnetrations for each solution. You will use your absorbance reading and best-fit line from the calibration curve to determine the equilibrium concentration of Fe(NCS)²+

44. You have three sodium carbonate solutions on a lab table in front of you. All of the solutions came from a 500.0-mL volumetric flask containing 3.00 M sodium carbonate. Solution 1: 100.0 mL of the 3.00 M solution. Solution 2: 50.0 mL of the 3.00 M solution. Solution 3: 10.0 mL of the 3.00 M solution. What is the new concentration of Solution 2 if 14.8 g of solid sodium carbonate is added and dissolved? (Assume no volume change.) a. 11.8 M b. 0.579 M c. 5.79 M d. 2.79 M e. 1.81 M

How do I find the moles excess HCl titrated and Moles HCl absorbed by Tablet

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Exactly 10.00-mL aliquots of a solution containing phenobarbital were measured into 50.00-mL volumetric flasks and made basic with KOH. The following volumes of a standard solution of phenobarbital containing 2.000μg/mL of phenobarbital were then introduced into each flask and the mixture was diluted to volume: 0.000, 0.500, 1.00, 1.50, 2.00 mL. The fluorescence of each of these solutions was measured with a fluorimeter, which gave values of 3.26, 4.80, 6.41, 8.02, 9.56, respectively. a. plot the data.  b. derive a least squares equation for the data plotted in (a). c. find the concentration of phenobarbital from the equation in (b). d. calculate a standard deviation for the concentration obtained in (c).

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To determine the concentration of a NaOH (39.997 g/mol) solution, 1.42 g of C8H5KO4 (a commonly used standard, 204.22 g/mol) was used. The volume of NaOH solution needed to reach the endpoint was 33.54 mL. What was the concentration (in molarity) of the NaOH solution? The mole:mole ratio for NaOH and KHP neutralization is 1:1. Report your answer to the thousandths place and do not include units.

280 mL of 1.08 M CrCl₂ is mixed with with 160 mL of 2.2 M KOH. Write out the balanced molecular, ionic, and net ionic equations. Then determine what mass of precipitate will form. Edit Format Table 12pt Paragraph V BIU A v T²V | V E✓ ✓ To ✓ √x

A student performed three H2SO4 titrations in Part 2 using their 0.1276 M NaOH solution which they previously standardized in Part 1. They reported the following measurements:   Determination #1 Determination #2 Determination #3 Final NaOH Burette Reading 20.72 mL 41.54 mL 21.59 mL Initial NaOH Burette Reading 0.12 mL 20.72 mL 0.83 mL What was the total number of moles of H2SO4 in their second titration? Report your answer to the correct number of significant figures and only report the numerical value (no units).

A 12.7g sample of vinegar is titrated.  It requires 19.75 mL of 0.205 M NaOH to neutralize the acetic acid (CH3COOH) in the vinegar.  Calculate the weight percent (w/w) of acetic acid in the vinegar.  Note: 1 mole of base neutralizes 1 mole of acid.